Building a Better Research Poster Step-by-Step Guide

Progressive reorganization, deletion, and edits reveal a clearer design and more effective poster.

1. Objectives Understanding the chemical behavior of everyday compounds is essential for safe laboratory practices and effective experimental design. This study investigates the physical states, molar masses, pH levels, and reactivity with hydrochloric acid (HCl) of six widely used substances: ethanol, sodium chloride, acetic acid, ammonia, calcium carbonate, and benzene. By comparing their properties, we aim to highlight trends in acid-base behavior and reactivity that can inform both educational and industrial applications. Methods Sample Selection: Six compounds were chosen based on their prevalence in undergraduate chemistry labs and industrial settings. Physical Characterization: Each compound’s state at room temperature and molar mass were recorded using standard reference data. pH Measurement: Aqueous solutions (0.1 M) of each compound were prepared and measured using a calibrated digital pH meter. Reactivity Testing: Reactivity with HCl was assessed by adding 1 mL of 1 M HCl to 10 mL of each compound solution and observing qualitative changes (e.g., gas evolution, precipitate formation, temperature change). Data Recording: Observations were documented, and results were tabulated for comparative analysis. Special Thanks We gratefully acknowledge the guidance, support, and inspiration provided by the following individuals throughout the course of this project: *Dr. Helena Voss – Department of Chemical Sciences, for her mentorship in experimental design *Dr. Rajiv Patel – Analytical Chemistry Division, for his insights on pH calibration techniques *Dr. Miriam Cho – History of Science Program, for her contributions to the historical context section *Dr. Thomas Nguyen – Organic Chemistry Lab Coordinator "The important thing in science is not so much to obtain new facts as to discover new ways of thinking about them." — Sir William Lawrence Bragg, Nobel Laureate in Physics, 1915 Ethanol (C₂H₅OH) and benzene (C₆H₆) were both liquid at room temperature, consistent with their relatively low molecular weights and non-ionic nature. Ethanol’s molar mass of 46.07 g/mol and benzene’s 78.11 g/mol reflect their compact molecular structures, which contribute to their volatility and widespread use as solvents. "Nothing is lost, nothing is created, everything is transformed." — Antoine Lavoisier, 18th-century French chemist and father of modern chemistry Sodium chloride (NaCl) and calcium carbonate ( CaCO ₃) appeared as crystalline solids, indicative of their strong ionic bonds and lattice structures. Their molar masses—58.44 g/mol and 100.09 g/mol, respectively—align with their roles in mineralogy and industrial chemistry. Reactivity with Hydrochloric Acid Acetic acid reacted vigorously with HCl, producing heat and a noticeable shift in solution clarity, indicative of proton exchange and equilibrium disruption. Ammonia formed ammonium chloride upon reaction, a classic acid-base neutralization that releases minimal heat and no gas. By comparing their properties, we aim to highlight trends in acid-base behavior and reactivity that can inform both educational and industrial applications. Conclusion The study revealed distinct patterns in acid-base behavior and reactivity: Acetic acid showed the highest reactivity with HCl due to its acidic nature, while sodium chloride remained inert. Ammonia exhibited moderate reactivity, consistent with its basic properties. Calcium carbonate reacted visibly with HCl, producing carbon dioxide gas—a classic acid-carbonate reaction. pH values correlated well with expected acid-base classifications, reinforcing the reliability of simple pH testing in compound identification. These findings underscore the importance of understanding chemical profiles for safe handling and predictive modeling in both academic and industrial chemistry settings. This comparative study highlights the diverse chemical behaviors of common laboratory compounds under standardized conditions. The observed variations in pH and reactivity with hydrochloric acid reflect fundamental acid-base interactions and molecular structure influences. Notably, compounds like acetic acid and calcium carbonate demonstrated pronounced reactivity, aligning with their known acidic and basic properties, respectively. These findings reinforce the value of simple qualitative tests in predicting chemical behavior and underscore the importance of molecular composition in determining compound reactivity. Such insights are vital for both instructional settings and preliminary screening in applied chemical research. The comparative evaluation of six laboratory compounds revealed clear distinctions in their acid-base characteristics and chemical reactivity. These insights contribute to a deeper understanding of compound behavior and support safer, more informed laboratory practices. Acetic acid showed the highest reactivity with HCl due to its acidic nature, while sodium chloride remained inert. Ammonia exhibited moderate reactivity, consistent with its basic properties. Calcium carbonate reacted visibly with HCl, producing carbon dioxide gas—a classic acid-carbonate reaction. These insights contribute to a deeper understanding of compound behavior and support safer, more informed laboratory practices. Ammonia (NH₃), a gas at room temperature with a molar mass of 17.03 g/mol, is notable for its pungent odor and historical significance in the Haber-Bosch process, which revolutionized fertilizer production in the early 20th century. Calcium carbonate underwent a visible effervescent reaction, releasing carbon dioxide gas—a reaction first documented by Joseph Black in the 18th century during his studies on “fixed air.” The behaviors observed in this study echo foundational discoveries in chemistry: The acid-base reactions mirror the work of early pioneers like Robert Boyle, Antoine Lavoisier, and Justus von Liebig, who laid the groundwork for understanding chemical reactivity. The inertness of sodium chloride and the volatility of benzene reflect principles of ionic bonding and aromatic stability, respectively—concepts that emerged from 19th-century structural chemistry. The effervescence of calcium carbonate with HCl remains a staple demonstration in classrooms, bridging historical pedagogy with modern analytical techniques. The effervescence of calcium carbonate with HCl remains a staple demonstration in classrooms. Molecular Behavior in Acidic Environments: A Comparative Study of Common Laboratory Compounds Helena Voss¹, Rajiv Patel², Miriam Cho³, Thomas Nguyen⁴, Evelyn Brooks⁵ ¹Eastbridge University, ²Northpoint Institute, ³Westvale College, ⁴Central State University This study presents a comparative analysis of six widely used laboratory compounds—ethanol, sodium chloride, acetic acid, ammonia, calcium carbonate, and benzene—focusing on their physical states, molar masses, pH levels, and reactivity with hydrochloric acid (HCl). Through standardized testing and qualitative observation, we identified distinct patterns in acid-base behavior and molecular reactivity. Acetic acid and calcium carbonate demonstrated high reactivity, consistent with their known acidic and basic properties, while sodium chloride remained inert. Historical context was integrated to highlight the evolution of acid-base theory from Lavoisier to Brønsted and Lowry. The findings reinforce foundational chemical principles and emphasize the value of simple diagnostic tests in both educational and industrial settings. This poster aims to bridge classical theory with modern lab practice, offering insights into how molecular structure governs chemical behavior. Compound Name Molecular Formula Molar Mass (g/mol) State at Room Temp pH Level Reactivity with HCl Ethanol C₂H₅OH 46.07 Liquid 7.33 Low Sodium Chloride NaCl 58.44 Solid 7.00 None Acetic Acid CH₃COOH 60.05 Liquid 2.87 High Ammonia NH₃ 17.03 Gas 11.60 Moderate Calcium Carbonate CaCO₃ 100.09 Solid 9.00 Moderate Benzene C₆H₆ 78.11 Liquid 6.50 Low Remove background color .

2. Objectives Understanding the chemical behavior of everyday compounds is essential for safe laboratory practices and effective experimental design. This study investigates the physical states, molar masses, pH levels, and reactivity with hydrochloric acid (HCl) of six widely used substances: ethanol, sodium chloride, acetic acid, ammonia, calcium carbonate, and benzene. By comparing their properties, we aim to highlight trends in acid-base behavior and reactivity that can inform both educational and industrial applications. Methods Sample Selection: Six compounds were chosen based on their prevalence in undergraduate chemistry labs and industrial settings. Physical Characterization: Each compound’s state at room temperature and molar mass were recorded using standard reference data. pH Measurement: Aqueous solutions (0.1 M) of each compound were prepared and measured using a calibrated digital pH meter. Reactivity Testing: Reactivity with HCl was assessed by adding 1 mL of 1 M HCl to 10 mL of each compound solution and observing qualitative changes (e.g., gas evolution, precipitate formation, temperature change). Data Recording: Observations were documented, and results were tabulated for comparative analysis. Special Thanks We gratefully acknowledge the guidance, support, and inspiration provided by the following individuals throughout the course of this project: *Dr. Helena Voss – Department of Chemical Sciences, for her mentorship in experimental design *Dr. Rajiv Patel – Analytical Chemistry Division, for his insights on pH calibration techniques *Dr. Miriam Cho – History of Science Program, for her contributions to the historical context section *Dr. Thomas Nguyen – Organic Chemistry Lab Coordinator "The important thing in science is not so much to obtain new facts as to discover new ways of thinking about them." — Sir William Lawrence Bragg, Nobel Laureate in Physics, 1915 Ethanol (C₂H₅OH) and benzene (C₆H₆) were both liquid at room temperature, consistent with their relatively low molecular weights and non-ionic nature. Ethanol’s molar mass of 46.07 g/mol and benzene’s 78.11 g/mol reflect their compact molecular structures, which contribute to their volatility and widespread use as solvents. "Nothing is lost, nothing is created, everything is transformed." — Antoine Lavoisier, 18th-century French chemist and father of modern chemistry Sodium chloride (NaCl) and calcium carbonate ( CaCO ₃) appeared as crystalline solids, indicative of their strong ionic bonds and lattice structures. Their molar masses—58.44 g/mol and 100.09 g/mol, respectively—align with their roles in mineralogy and industrial chemistry. Reactivity with Hydrochloric Acid Acetic acid reacted vigorously with HCl, producing heat and a noticeable shift in solution clarity, indicative of proton exchange and equilibrium disruption. Ammonia formed ammonium chloride upon reaction, a classic acid-base neutralization that releases minimal heat and no gas. By comparing their properties, we aim to highlight trends in acid-base behavior and reactivity that can inform both educational and industrial applications. Conclusion The study revealed distinct patterns in acid-base behavior and reactivity: Acetic acid showed the highest reactivity with HCl due to its acidic nature, while sodium chloride remained inert. Ammonia exhibited moderate reactivity, consistent with its basic properties. Calcium carbonate reacted visibly with HCl, producing carbon dioxide gas—a classic acid-carbonate reaction. pH values correlated well with expected acid-base classifications, reinforcing the reliability of simple pH testing in compound identification. These findings underscore the importance of understanding chemical profiles for safe handling and predictive modeling in both academic and industrial chemistry settings. This comparative study highlights the diverse chemical behaviors of common laboratory compounds under standardized conditions. The observed variations in pH and reactivity with hydrochloric acid reflect fundamental acid-base interactions and molecular structure influences. Notably, compounds like acetic acid and calcium carbonate demonstrated pronounced reactivity, aligning with their known acidic and basic properties, respectively. These findings reinforce the value of simple qualitative tests in predicting chemical behavior and underscore the importance of molecular composition in determining compound reactivity. Such insights are vital for both instructional settings and preliminary screening in applied chemical research. The comparative evaluation of six laboratory compounds revealed clear distinctions in their acid-base characteristics and chemical reactivity. These insights contribute to a deeper understanding of compound behavior and support safer, more informed laboratory practices. Acetic acid showed the highest reactivity with HCl due to its acidic nature, while sodium chloride remained inert. Ammonia exhibited moderate reactivity, consistent with its basic properties. Calcium carbonate reacted visibly with HCl, producing carbon dioxide gas—a classic acid-carbonate reaction. These insights contribute to a deeper understanding of compound behavior and support safer, more informed laboratory practices. Ammonia (NH₃), a gas at room temperature with a molar mass of 17.03 g/mol, is notable for its pungent odor and historical significance in the Haber-Bosch process, which revolutionized fertilizer production in the early 20th century. Calcium carbonate underwent a visible effervescent reaction, releasing carbon dioxide gas—a reaction first documented by Joseph Black in the 18th century during his studies on “fixed air.” The behaviors observed in this study echo foundational discoveries in chemistry: The acid-base reactions mirror the work of early pioneers like Robert Boyle, Antoine Lavoisier, and Justus von Liebig, who laid the groundwork for understanding chemical reactivity. The inertness of sodium chloride and the volatility of benzene reflect principles of ionic bonding and aromatic stability, respectively—concepts that emerged from 19th-century structural chemistry. The effervescence of calcium carbonate with HCl remains a staple demonstration in classrooms, bridging historical pedagogy with modern analytical techniques. The effervescence of calcium carbonate with HCl remains a staple demonstration in classrooms. Molecular Behavior in Acidic Environments: A Comparative Study of Common Laboratory Compounds Helena Voss¹, Rajiv Patel², Miriam Cho³, Thomas Nguyen⁴, Evelyn Brooks⁵ ¹Eastbridge University, ²Northpoint Institute, ³Westvale College, ⁴Central State University This study presents a comparative analysis of six widely used laboratory compounds—ethanol, sodium chloride, acetic acid, ammonia, calcium carbonate, and benzene—focusing on their physical states, molar masses, pH levels, and reactivity with hydrochloric acid (HCl). Through standardized testing and qualitative observation, we identified distinct patterns in acid-base behavior and molecular reactivity. Acetic acid and calcium carbonate demonstrated high reactivity, consistent with their known acidic and basic properties, while sodium chloride remained inert. Historical context was integrated to highlight the evolution of acid-base theory from Lavoisier to Brønsted and Lowry. The findings reinforce foundational chemical principles and emphasize the value of simple diagnostic tests in both educational and industrial settings. This poster aims to bridge classical theory with modern lab practice, offering insights into how molecular structure governs chemical behavior. Compound Name Molecular Formula Molar Mass (g/mol) State at Room Temp pH Level Reactivity with HCl Ethanol C₂H₅OH 46.07 Liquid 7.33 Low Sodium Chloride NaCl 58.44 Solid 7.00 None Acetic Acid CH₃COOH 60.05 Liquid 2.87 High Ammonia NH₃ 17.03 Gas 11.60 Moderate Calcium Carbonate CaCO₃ 100.09 Solid 9.00 Moderate Benzene C₆H₆ 78.11 Liquid 6.50 Low Remove borders .

3. Objectives Understanding the chemical behavior of everyday compounds is essential for safe laboratory practices and effective experimental design. This study investigates the physical states, molar masses, pH levels, and reactivity with hydrochloric acid (HCl) of six widely used substances: ethanol, sodium chloride, acetic acid, ammonia, calcium carbonate, and benzene. By comparing their properties, we aim to highlight trends in acid-base behavior and reactivity that can inform both educational and industrial applications. Methods Sample Selection: Six compounds were chosen based on their prevalence in undergraduate chemistry labs and industrial settings. Physical Characterization: Each compound’s state at room temperature and molar mass were recorded using standard reference data. pH Measurement: Aqueous solutions (0.1 M) of each compound were prepared and measured using a calibrated digital pH meter. Reactivity Testing: Reactivity with HCl was assessed by adding 1 mL of 1 M HCl to 10 mL of each compound solution and observing qualitative changes (e.g., gas evolution, precipitate formation, temperature change). Data Recording: Observations were documented, and results were tabulated for comparative analysis. Special Thanks We gratefully acknowledge the guidance, support, and inspiration provided by the following individuals throughout the course of this project: *Dr. Helena Voss – Department of Chemical Sciences, for her mentorship in experimental design *Dr. Rajiv Patel – Analytical Chemistry Division, for his insights on pH calibration techniques *Dr. Miriam Cho – History of Science Program, for her contributions to the historical context section *Dr. Thomas Nguyen – Organic Chemistry Lab Coordinator "The important thing in science is not so much to obtain new facts as to discover new ways of thinking about them." — Sir William Lawrence Bragg, Nobel Laureate in Physics, 1915 Ethanol (C₂H₅OH) and benzene (C₆H₆) were both liquid at room temperature, consistent with their relatively low molecular weights and non-ionic nature. Ethanol’s molar mass of 46.07 g/mol and benzene’s 78.11 g/mol reflect their compact molecular structures, which contribute to their volatility and widespread use as solvents. "Nothing is lost, nothing is created, everything is transformed." — Antoine Lavoisier, 18th-century French chemist and father of modern chemistry Sodium chloride (NaCl) and calcium carbonate ( CaCO ₃) appeared as crystalline solids, indicative of their strong ionic bonds and lattice structures. Their molar masses—58.44 g/mol and 100.09 g/mol, respectively—align with their roles in mineralogy and industrial chemistry. Reactivity with Hydrochloric Acid Acetic acid reacted vigorously with HCl, producing heat and a noticeable shift in solution clarity, indicative of proton exchange and equilibrium disruption. Ammonia formed ammonium chloride upon reaction, a classic acid-base neutralization that releases minimal heat and no gas. By comparing their properties, we aim to highlight trends in acid-base behavior and reactivity that can inform both educational and industrial applications. Conclusion The study revealed distinct patterns in acid-base behavior and reactivity: Acetic acid showed the highest reactivity with HCl due to its acidic nature, while sodium chloride remained inert. Ammonia exhibited moderate reactivity, consistent with its basic properties. Calcium carbonate reacted visibly with HCl, producing carbon dioxide gas—a classic acid-carbonate reaction. pH values correlated well with expected acid-base classifications, reinforcing the reliability of simple pH testing in compound identification. These findings underscore the importance of understanding chemical profiles for safe handling and predictive modeling in both academic and industrial chemistry settings. This comparative study highlights the diverse chemical behaviors of common laboratory compounds under standardized conditions. The observed variations in pH and reactivity with hydrochloric acid reflect fundamental acid-base interactions and molecular structure influences. Notably, compounds like acetic acid and calcium carbonate demonstrated pronounced reactivity, aligning with their known acidic and basic properties, respectively. These findings reinforce the value of simple qualitative tests in predicting chemical behavior and underscore the importance of molecular composition in determining compound reactivity. Such insights are vital for both instructional settings and preliminary screening in applied chemical research. The comparative evaluation of six laboratory compounds revealed clear distinctions in their acid-base characteristics and chemical reactivity. These insights contribute to a deeper understanding of compound behavior and support safer, more informed laboratory practices. Acetic acid showed the highest reactivity with HCl due to its acidic nature, while sodium chloride remained inert. Ammonia exhibited moderate reactivity, consistent with its basic properties. Calcium carbonate reacted visibly with HCl, producing carbon dioxide gas—a classic acid-carbonate reaction. These insights contribute to a deeper understanding of compound behavior and support safer, more informed laboratory practices. Ammonia (NH₃), a gas at room temperature with a molar mass of 17.03 g/mol, is notable for its pungent odor and historical significance in the Haber-Bosch process, which revolutionized fertilizer production in the early 20th century. Calcium carbonate underwent a visible effervescent reaction, releasing carbon dioxide gas—a reaction first documented by Joseph Black in the 18th century during his studies on “fixed air.” The behaviors observed in this study echo foundational discoveries in chemistry: The acid-base reactions mirror the work of early pioneers like Robert Boyle, Antoine Lavoisier, and Justus von Liebig, who laid the groundwork for understanding chemical reactivity. The inertness of sodium chloride and the volatility of benzene reflect principles of ionic bonding and aromatic stability, respectively—concepts that emerged from 19th-century structural chemistry. The effervescence of calcium carbonate with HCl remains a staple demonstration in classrooms, bridging historical pedagogy with modern analytical techniques. The effervescence of calcium carbonate with HCl remains a staple demonstration in classrooms. Molecular Behavior in Acidic Environments: A Comparative Study of Common Laboratory Compounds Helena Voss¹, Rajiv Patel², Miriam Cho³, Thomas Nguyen⁴, Evelyn Brooks⁵ ¹Eastbridge University, ²Northpoint Institute, ³Westvale College, ⁴Central State University This study presents a comparative analysis of six widely used laboratory compounds—ethanol, sodium chloride, acetic acid, ammonia, calcium carbonate, and benzene—focusing on their physical states, molar masses, pH levels, and reactivity with hydrochloric acid (HCl). Through standardized testing and qualitative observation, we identified distinct patterns in acid-base behavior and molecular reactivity. Acetic acid and calcium carbonate demonstrated high reactivity, consistent with their known acidic and basic properties, while sodium chloride remained inert. Historical context was integrated to highlight the evolution of acid-base theory from Lavoisier to Brønsted and Lowry. The findings reinforce foundational chemical principles and emphasize the value of simple diagnostic tests in both educational and industrial settings. This poster aims to bridge classical theory with modern lab practice, offering insights into how molecular structure governs chemical behavior. Compound Name Molecular Formula Molar Mass (g/mol) State at Room Temp pH Level Reactivity with HCl Ethanol C₂H₅OH 46.07 Liquid 7.33 Low Sodium Chloride NaCl 58.44 Solid 7.00 None Acetic Acid CH₃COOH 60.05 Liquid 2.87 High Ammonia NH₃ 17.03 Gas 11.60 Moderate Calcium Carbonate CaCO₃ 100.09 Solid 9.00 Moderate Benzene C₆H₆ 78.11 Liquid 6.50 Low Reduce content to only what’s necessary.

4. Exploring Acid-Base Trends in Common Substances This study explores the chemical behavior of six common compounds—ethanol, sodium chloride, acetic acid, ammonia, calcium carbonate, and benzene—by examining their physical states, molar masses, pH levels, and reactivity with hydrochloric acid. The goal is to identify trends in acid-base behavior relevant to both education and industry. Methods Compound Selection: Six substances were chosen for their frequent use in teaching and industry. Characterization: Physical state and molar mass were noted using reference data. pH Testing: 0.1 M aqueous solutions were measured with a calibrated pH meter. HCl Reactivity: Each solution received 1 mL of 1 M HCl; reactions were observed for gas, precipitate, or heat. Data Collection: Observations were recorded and compiled for comparison. Special Thanks We gratefully acknowledge the guidance, support, and inspiration provided by the following individuals throughout the course of this project: *Dr. Helena Voss – Department of Chemical Sciences, for her mentorship in experimental design *Dr. Rajiv Patel – Analytical Chemistry Division, for his insights on pH calibration techniques *Dr. Miriam Cho – History of Science Program, for her contributions to the historical context section *Dr. Thomas Nguyen – Organic Chemistry Lab Coordinator Reactivity with Hydrochloric Acid Conclusion Simple tests revealed clear differences in acid-base behavior. Reactivity and pH values aligned with expectations, reinforcing how molecular structure influences chemical response. These results support the use of basic diagnostics in teaching and lab safety. These findings reaffirm that molecular structure is key to predicting chemical behavior in acidic environments. Future Directions Explore reaction rates and temperature effects Include more diverse compounds Use spectroscopy for deeper analysis Assess educational impact in lab settings Acetic acid (CH₃COOH) exhibited the strongest acidic behavior with a pH of 2.87 and vigorous reaction with HCl, consistent with its role in early acid-base studies dating back to the work of Svante Arrhenius in the late 19th century. Ammonia (NH₃), a historically significant base used in the Haber-Bosch process, showed a high pH of 11.60 and moderate reactivity, reinforcing its classification as a weak base. Calcium carbonate ( CaCO ₃) reacted visibly with HCl, producing effervescence due to CO₂ release—a reaction famously used by early chemists like Joseph Black to study carbonates. Sodium chloride (NaCl) remained inert in acidic conditions, confirming its stability as a neutral salt. Ethanol (C₂H₅OH) and benzene (C₆H₆) showed minimal reactivity, with near-neutral pH values, reflecting their non-ionic nature and historical use as solvents in organic chemistry. The experimental analysis of six common laboratory compounds revealed distinct trends in physical state, molar mass, pH levels, and reactivity with hydrochloric acid (HCl): Molecular Behavior in Acidic Environments and the Reactivity of Common Laboratory Compounds Helena Voss¹, Rajiv Patel², Miriam Cho³, Thomas Nguyen⁴, Evelyn Brooks⁵ ¹Eastbridge University, ²Northpoint Institute, ³Westvale College, ⁴Central State University Compound Name Molecular Formula Molar Mass (g/mol) State at Room Temp pH Level Reactivity with HCl Ethanol C₂H₅OH 46.07 Liquid 7.33 Low Sodium Chloride NaCl 58.44 Solid 7.00 None Acetic Acid CH₃COOH 60.05 Liquid 2.87 High Ammonia NH₃ 17.03 Gas 11.60 Moderate Calcium Carbonate CaCO₃ 100.09 Solid 9.00 Moderate Benzene C₆H₆ 78.11 Liquid 6.50 Low Align content to columns.

5. Exploring Acid-Base Trends in Common Substances This study explores the chemical behavior of six common compounds—ethanol, sodium chloride, acetic acid, ammonia, calcium carbonate, and benzene—by examining their physical states, molar masses, pH levels, and reactivity with hydrochloric acid. The goal is to identify trends in acid-base behavior relevant to both education and industry. Methods Compound Selection: Six substances were chosen for their frequent use in teaching and industry. Characterization: Physical state and molar mass were noted using reference data. pH Testing: 0.1 M aqueous solutions were measured with a calibrated pH meter. HCl Reactivity: Each solution received 1 mL of 1 M HCl; reactions were observed for gas, precipitate, or heat. Data Collection: Observations were recorded and compiled for comparison. Special Thanks We gratefully acknowledge the guidance, support, and inspiration provided by the following individuals throughout the course of this project: Dr. Helena Voss – Department of Chemical Sciences, for her mentorship Dr. Rajiv Patel – Analytical Chemistry Division, for his insights on pH calibration techniques Dr. Miriam Cho – History of Science Program, for her contributions to the historical context section Dr. Thomas Nguyen – Chemistry Lab Coordinator Conclusion Simple tests revealed clear differences in acid-base behavior. Reactivity and pH values aligned with expectations, reinforcing how molecular structure influences chemical response. These results support the use of basic diagnostics in teaching and lab safety. These findings reaffirm that molecular structure is key to predicting chemical behavior in acidic environments. Future Directions Explore reaction rates and temperature effects Include more diverse compounds Use spectroscopy for deeper analysis Assess educational impact in lab settings Reactivity with Hydrochloric Acid Six compounds were analyzed for physical state, molar mass, pH, and reactivity with hydrochloric acid: Acetic acid showed strong reactivity and a low pH, confirming its acidic nature. Ammonia had a high pH and moderate reactivity, consistent with its basic properties. Calcium carbonate reacted visibly with HCl, releasing CO₂—a classic acid-carbonate response. Sodium chloride remained inert, reflecting its neutral salt status. Ethanol and benzene had near-neutral pH and low reactivity, typical of non-ionizing organic compounds. Molecular Behavior in Acidic Environments and the Reactivity of Common Laboratory Compounds Helena Voss¹, Rajiv Patel², Miriam Cho³, Thomas Nguyen⁴, Evelyn Brooks⁵ ¹Eastbridge University, ²Northpoint Institute, ³Westvale College, ⁴Central State University Compound pH Reactivity with HCl Ethanol 7.33 Low Sodium Chloride 7.00 None Acetic Acid 2.87 High Ammonia 11.60 Moderate Calcium Carbonate 9.00 Moderate Benzene 6.50 Low Left align text.

6. Exploring Acid-Base Trends in Common Substances This study explores the chemical behavior of six common compounds—ethanol, sodium chloride, acetic acid, ammonia, calcium carbonate, and benzene—by examining their physical states, molar masses, pH levels, and reactivity with hydrochloric acid. The goal is to identify trends in acid-base behavior relevant to both education and industry. Methods Compound Selection: Six substances were chosen for their frequent use in teaching and industry. Characterization: Physical state and molar mass were noted using reference data. pH Testing: 0.1 M aqueous solutions were measured with a calibrated pH meter. HCl Reactivity: Each solution received 1 mL of 1 M HCl; reactions were observed for gas, precipitate, or heat. Data Collection: Observations were recorded and compiled for comparison. Special Thanks We gratefully acknowledge the guidance, support, and inspiration provided by the following individuals throughout the course of this project: Dr. Helena Voss – Department of Chemical Sciences, for her mentorship Dr. Rajiv Patel – Analytical Chemistry Division, for his insights on pH calibration techniques Dr. Miriam Cho – History of Science Program, for her contributions to the historical context section Dr. Thomas Nguyen – Chemistry Lab Coordinator Conclusion Simple tests revealed clear differences in acid-base behavior. Reactivity and pH values aligned with expectations, reinforcing how molecular structure influences chemical response. These results support the use of basic diagnostics in teaching and lab safety. These findings reaffirm that molecular structure is key to predicting chemical behavior in acidic environments. Future Directions Explore reaction rates and temperature effects Include more diverse compounds Use spectroscopy for deeper analysis Assess educational impact in lab settings Reactivity with Hydrochloric Acid Six compounds were analyzed for physical state, molar mass, pH, and reactivity with hydrochloric acid: Acetic acid showed strong reactivity and a low pH, confirming its acidic nature. Ammonia had a high pH and moderate reactivity, consistent with its basic properties. Calcium carbonate reacted visibly with HCl, releasing CO₂—a classic acid-carbonate response. Sodium chloride remained inert, reflecting its neutral salt status. Ethanol and benzene had near-neutral pH and low reactivity, typical of non-ionizing organic compounds. Molecular Behavior in Acidic Environments and the Reactivity of Common Laboratory Compounds Helena Voss¹, Rajiv Patel², Miriam Cho³, Thomas Nguyen⁴, Evelyn Brooks⁵ ¹Eastbridge University, ²Northpoint Institute, ³Westvale College, ⁴Central State University Compound pH Reactivity with HCl Ethanol 7.33 Low Sodium Chloride 7.00 None Acetic Acid 2.87 High Ammonia 11.60 Moderate Calcium Carbonate 9.00 Moderate Benzene 6.50 Low Select a clear font .

7. Methods Compound Selection: Six substances were chosen for their use in teaching and industry. Characterization: Physical state and molar mass were noted using reference data. pH Testing: 0.1 M aqueous solutions were measured with a calibrated pH meter. HCl Reactivity: Each solution received 1 mL of 1 M HCl; reactions were observed for gas, precipitate, or heat. Data Collection: Observations were recorded and compiled for comparison. Molecular Behavior in Acidic Environments and the Reactivity of Common Laboratory Compounds Helena Voss¹, Rajiv Patel², Miriam Cho³, Thomas Nguyen⁴, Evelyn Brooks⁵ ¹Eastbridge University, ²Northpoint Institute, ³Westvale College, ⁴Central State University Compound pH Reactivity with HCl Ethanol 7.33 Low Sodium Chloride 7.00 None Acetic Acid 2.87 High Ammonia 11.60 Moderate Calcium Carbonate 9.00 Moderate Benzene 6.50 Low Simplify graphics and use accessible colors. Exploring Acid-Base Trends in Common Substances This study explores the chemical behavior of six common compounds—ethanol, sodium chloride, acetic acid, ammonia, calcium carbonate, and benzene—by examining their physical states, molar masses, pH levels, and reactivity with hydrochloric acid. The goal is to identify trends in acid-base behavior relevant to both education and industry. Conclusion Simple tests revealed clear differences in acid-base behavior. Reactivity and pH values aligned with expectations, reinforcing how molecular structure influences chemical response. These results support the use of basic diagnostics in teaching and lab safety. These findings reaffirm that molecular structure is key to predicting chemical behavior in acidic environments. Reactivity with Hydrochloric Acid Six compounds were analyzed for physical state, molar mass, pH, and reactivity with hydrochloric acid. Sodium chloride remained inert, reflecting its neutral salt status. Acetic acid showed strong reactivity and a low pH, confirming its acidic nature. Ammonia had a high pH and moderate reactivity, consistent with its basic properties. Calcium carbonate reacted visibly with HCl, releasing CO₂—a classic acid-carbonate response. Ethanol and benzene had near-neutral pH and low reactivity, typical of non-ionizing organic compounds. Special Thanks We gratefully acknowledge the guidance, support, and inspiration provided by the following individuals throughout the course of this project: Dr. Helena Voss – Department of Chemical Sciences, for her mentorship Dr. Rajiv Patel – Analytical Chemistry Division, for his insights on pH calibration techniques Dr. Miriam Cho – History of Science Program, for her contributions to the historical context section Dr. Thomas Nguyen – Chemistry Lab Coordinator Future Directions Explore reaction rates and temperature effects Include more diverse compounds Use spectroscopy for deeper analysis Assess educational impact in lab settings

8. Methods Compound Selection: Six substances were chosen for their use in teaching and industry. Characterization: Physical state and molar mass were noted using reference data. pH Testing: 0.1 M aqueous solutions were measured with a calibrated pH meter. HCl Reactivity: Each solution received 1 mL of 1 M HCl; reactions were observed for gas, precipitate, or heat. Data Collection: Observations were recorded and compiled for comparison. Molecular Behavior in Acidic Environments and the Reactivity of Common Laboratory Compounds Helena Voss¹, Rajiv Patel², Miriam Cho³, Thomas Nguyen⁴, Evelyn Brooks⁵ ¹Eastbridge University, ²Northpoint Institute, ³Westvale College, ⁴Central State University Compound pH Reactivity with HCl Ethanol 7.33 Low Sodium Chloride 7.00 None Acetic Acid 2.87 High Ammonia 11.60 Moderate Calcium Carbonate 9.00 Moderate Benzene 6.50 Low Sodium chloride remained inert, reflecting its neutral salt status. Acetic acid showed strong reactivity and a low pH, confirming its acidic nature. Ammonia had a high pH and moderate reactivity, consistent with its basic properties. Calcium carbonate reacted visibly with HCl, releasing CO₂—a classic acid-carbonate response. Ethanol and benzene had near-neutral pH and low reactivity, typical of non-ionizing organic compounds. Apply minimal formatting to add emphasis. Exploring Acid-Base Trends in Common Substances This study explores the chemical behavior of six common compounds—ethanol, sodium chloride, acetic acid, ammonia, calcium carbonate, and benzene—by examining their physical states, molar masses, pH levels, and reactivity with hydrochloric acid. The goal is to identify trends in acid-base behavior relevant to both education and industry. Conclusion Simple tests revealed clear differences in acid-base behavior. Reactivity and pH values aligned with expectations, reinforcing how molecular structure influences chemical response. These results support the use of basic diagnostics in teaching and lab safety. These findings reaffirm that molecular structure is key to predicting chemical behavior in acidic environments. Reactivity with Hydrochloric Acid Six compounds were analyzed for physical state, molar mass, pH, and reactivity with hydrochloric acid. Special Thanks We gratefully acknowledge the guidance, support, and inspiration provided by the following individuals throughout the course of this project: Dr. Helena Voss – Department of Chemical Sciences, for her mentorship Dr. Rajiv Patel – Analytical Chemistry Division, for his insights on pH calibration techniques Dr. Miriam Cho – History of Science Program, for her contributions to the historical context section Dr. Thomas Nguyen – Chemistry Lab Coordinator Future Directions Explore reaction rates and temperature effects Include more diverse compounds Use spectroscopy for deeper analysis Assess educational impact in lab settings

9. Methods Compound Selection: Six substances were chosen for their use in teaching and industry. Characterization: Physical state and molar mass were noted using reference data. pH Testing : 0.1 M aqueous solutions were measured with a calibrated pH meter. HCl Reactivity : Each solution received 1 mL of 1 M HCl; reactions were observed for gas, precipitate, or heat. Data Collection: Observations were recorded and compiled for comparison. Molecular Behavior in Acidic Environments and the Reactivity of Common Laboratory Compounds Helena Voss¹, Rajiv Patel², Miriam Cho³, Thomas Nguyen⁴, Evelyn Brooks⁵ ¹Eastbridge University, ²Northpoint Institute, ³Westvale College, ⁴Central State University Sodium chloride remained inert, reflecting its neutral salt status. Acetic acid showed strong reactivity and a low pH, confirming its acidic nature. Ammonia had a high pH and moderate reactivity, consistent with its basic properties. Calcium carbonate reacted visibly with HCl, releasing CO₂—a classic acid-carbonate response. Ethanol and benzene had near-neutral pH and low reactivity, typical of non-ionizing organic compounds. Add contact information . Exploring Acid-Base Trends in Common Substances This study explores the chemical behavior of six common compounds—ethanol, sodium chloride, acetic acid, ammonia, calcium carbonate, and benzene—by examining their physical states, molar masses, pH levels, and reactivity with hydrochloric acid. The goal is to identify trends in acid-base behavior relevant to both education and industry. Conclusion Simple tests revealed clear differences in acid-base behavior. Reactivity and pH values aligned with expectations, reinforcing how molecular structure influences chemical response. These results support the use of basic diagnostics in teaching and lab safety. Reactivity with Hydrochloric Acid Six compounds were analyzed for physical state, molar mass, pH, and reactivity with hydrochloric acid. Special Thanks We gratefully acknowledge the guidance, support, and inspiration provided by the following individuals throughout the course of this project: Dr. Helena Voss – Department of Chemical Sciences, for her mentorship Dr. Rajiv Patel – Analytical Chemistry Division, for his insights on pH calibration techniques Dr. Miriam Cho – History of Science Program, for her contributions to the historical context section Dr. Thomas Nguyen – Chemistry Lab Coordinator Future Directions Explore reaction rates and temperature effects Include more diverse compounds Use spectroscopy for deeper analysis Assess educational impact in lab settings These findings reaffirm that molecular structure is key to predicting chemical behavior in acidic environments. Compound pH Reactivity with HCl Ethanol 7.33 Low Sodium Chloride 7.00 None Acetic Acid 2.87 High Ammonia 11.60 Moderate Calcium Carbonate 9.00 Moderate Benzene 6.50 Low

10. Exploring Acid-Base Trends in Common Substances This study explores the chemical behavior of six common compounds—ethanol, sodium chloride, acetic acid, ammonia, calcium carbonate, and benzene—by examining their physical states, molar masses, pH levels, and reactivity with hydrochloric acid. The goal is to identify trends in acid-base behavior relevant to both education and industry. Methods Compound Selection: Six substances were chosen for their use in teaching and industry. Characterization: Physical state and molar mass were noted using reference data. pH Testing : 0.1 M aqueous solutions were measured with a calibrated pH meter. HCl Reactivity : Each solution received 1 mL of 1 M HCl; reactions were observed for gas, precipitate, or heat. Data Collection: Observations were recorded and compiled for comparison. Special Thanks We gratefully acknowledge the guidance, support, and inspiration provided by the following individuals throughout the course of this project: Dr. Helena Voss – Department of Chemical Sciences, for her mentorship Dr. Rajiv Patel – Analytical Chemistry Division, for his insights on pH calibration techniques Dr. Miriam Cho – History of Science Program, for her contributions to the historical context section Dr. Thomas Nguyen – Chemistry Lab Coordinator Conclusion Simple tests revealed clear differences in acid-base behavior. Reactivity and pH values aligned with expectations, reinforcing how molecular structure influences chemical response. These results support the use of basic diagnostics in teaching and lab safety. Reactivity with Hydrochloric Acid Six compounds were analyzed for physical state, molar mass, pH, and reactivity with hydrochloric acid. Molecular Behavior in Acidic Environments and the Reactivity of Common Laboratory Compounds Helena Voss¹, Rajiv Patel², Miriam Cho³, Thomas Nguyen⁴, Evelyn Brooks⁵ ¹Eastbridge University, ²Northpoint Institute, ³Westvale College, ⁴Central State University Compound pH Reactivity with HCl Ethanol 7.33 Low Sodium Chloride 7.00 None Acetic Acid 2.87 High Ammonia 11.60 Moderate Calcium Carbonate 9.00 Moderate Benzene 6.50 Low Future Directions Explore reaction rates and temperature effects Include more diverse compounds Use spectroscopy for deeper analysis Assess educational impact in lab settings These findings reaffirm that molecular structure is key to predicting chemical behavior in acidic environments. Sodium chloride remained inert, reflecting its neutral salt status. Acetic acid showed strong reactivity and a low pH, confirming its acidic nature. Ammonia had a high pH and moderate reactivity, consistent with its basic properties. Calcium carbonate reacted visibly with HCl, releasing CO₂—a classic acid-carbonate response. Ethanol and benzene had near-neutral pH and low reactivity, typical of non-ionizing organic compounds. Get in Touch Maya Chen [email protected] https://orcid.org/0000-0002-5478-1934 mayachenlab.org Lab Website