DPP(Concentration+Terms).pdf chemistry neet practice pdf

Dpp

1. DPP-3
Concentration Terms

2. 40.25 g of Glauber’s salt is dissolved in water to obtain 500 mL of
solution of density 1077.5 g dm
–3
. The molality of Na
2
SO
4
in solution
is about
A
C
D
B
0.25 mol kg
–1
0.24 mol kg
–1

0.26 mol kg
–1

0.27 mol kg
–1

3. 40.25 g of Glauber’s salt is dissolved in water to obtain 500 mL of
solution of density 1077.5 g dm
–3
. The molality of Na
2
SO
4
in solution
is about
A
C
D
B
0.25 mol kg
–1
0.24 mol kg
–1

0.26 mol kg
–1

0.27 mol kg
–1

4. Solution:

5. An aqueous solution of acetic acid has density 1.1 g mol
–1
and
molality 4.6 mol kg
–1
. The molarity of acetic acid would be
A
C
D
B
3.2 M

3.5 M
3.97 M
4.6 M

6. An aqueous solution of acetic acid has density 1.1 g mol
–1
and
molality 4.6 mol kg
–1
. The molarity of acetic acid would be
A
C
D
B
3.2 M

3.5 M
3.97 M
4.6 M

7. Solution:

8. The volume of 82.5 mass percent of H
2
SO
4
(density 1.6 g cm
–3
) to
prepare 200 cm
3
of 15 mass percent of H
2
SO
4
(density 1.1 g cm
–3
) is
A
C
D
B
162 cm
3
173 cm
3

180 cm
3

193 cm
3

9. The volume of 82.5 mass percent of H
2
SO
4
(density 1.6 g cm
–3
) to
prepare 200 cm
3
of 15 mass percent of H
2
SO
4
(density 1.1 g cm
–3
) is
A
C
D
B
162 cm
3
173 cm
3

180 cm
3

193 cm
3

10. Solution:

11. 115 ml of ethanol (density = 0.8 g ml
–1
) on mixing with 99 mL of
water gives 200 mL of solution. The numerical values molarity,
molality and mole fraction of ethanol, respectively, are
A
C
D
B
10, 20.2, 0.267

20.2, 10, 0.267
10, 20.2, 0.733
20.2, 10, 0.733

12. 115 ml of ethanol (density = 0.8 g ml
–1
) on mixing with 99 mL of
water gives 200 mL of solution. The numerical values molarity,
molality and mole fraction of ethanol, respectively, are
A
C
D
B
10, 20.2, 0.267

20.2, 10, 0.267
10, 20.2, 0.733
20.2, 10, 0.733

13. Solution:

14. The mole fraction of ethanol in water is 0.08. Its molality will be
A
C
D
B
2.41 mol kg
–1
4.83 mol kg
–1

3.33 mol kg
–1


6.41 mol kg
–1

15. The mole fraction of ethanol in water is 0.08. Its molality will be
A
C
D
B
2.41 mol kg
–1
4.83 mol kg
–1

3.33 mol kg
–1


6.41 mol kg
–1

16. Solution:

17. The volume of H
2
evolved at STP when 0.9 g of Al (molar mass: 27 g
mol
–1
) is dissolved in excess of dilute H
2
SO
4
is
A
C
D
B
0.58 L

1.12 L
2.40 L
2.9 L

18. The volume of H
2
evolved at STP when 0.9 g of Al (molar mass: 27 g
mol
–1
) is dissolved in excess of dilute H
2
SO
4
is
A
C
D
B
0.58 L

1.12 L
2.40 L
2.9 L

19. Solution:

20. Which of the concentration units is temperature dependent?
A
C
D
B
Molality

Amount fraction

Molarity

Parts per million

21. Which of the concentration units is temperature dependent?
A
C
D
B
Molality

Amount fraction

Molarity

Parts per million

22. The molarity of concentrated sulphuric acid (density = 1.834 g cm
–3
)
containing 95% of H
2
SO
4
by mass is
A
C
D
B
4.44 M

8.88 M

13.32 M

17.78 M

23. The molarity of concentrated sulphuric acid (density = 1.834 g cm
–3
)
containing 95% of H
2
SO
4
by mass is
A
C
D
B
4.44 M

8.88 M

13.32 M

17.78 M

24. Solution:

25. Calculate molality(m) of pure water if its density is
0.936 g/mL.
A
C
D
B
50
55.56
57.56
56.56

26. Calculate molality(m) of pure water if its density is
0.936 g/mL.
A
C
D
B
50
55.56
57.56
56.56

27. Solution :

28. The volume (in mL) of 0.5 M NaOH required for the
complete reaction with 150 mL of 1.5M H
3
PO
3
solution
is
A
C
D
B
1350
900
1250
1150

29. The volume (in mL) of 0.5 M NaOH required for the
complete reaction with 150 mL of 1.5M H
3
PO
3
solution
is
A
C
D
B
1350
900
1250
1150

30. Solution :

31. What is the relationship between mole fraction of of a
solute (X
A
) and its molality (m). If molar mass of
solvent is 100. (g/mol).
A
C D
B

32. What is the relationship between mole fraction of of a
solute (X
A
) and its molality (m). If molar mass of
solvent is 100. (g/mol).
A
C D
B

33. Solution :

34. If in a sample of oleum, mole fraction of SO
3
is 0.5,
label the oleum sample.
A
C
D
B
109 %
110.11 %
104.5 %
114.22

35. If in a sample of oleum, mole fraction of SO
3
is 0.5,
label the oleum sample.
A
C
D
B
109 %
110.11 %
104.5 %
114.22

36. Solution :

37. Which of the following option(s) is incorrect?
[Take H
2
O to be solvent in every case and solute is
completely soluble]
A
C
D
B
If mass fraction of CaBr
2
and H
2
O are same then molality of
CaBr
2
is 5 m.
If equal moles of NaCl and H
2
O are taken then molality of NaCl is
55.55 m.
If in place of NaCl we use NaBr as solute in option (2) then
molality of NaCl changes.
If mole fraction of NaCl is same as that of H
2
O then molality of
NaCl will be 55.55 m.

38. Which of the following option(s) is incorrect?
[Take H
2
O to be solvent in every case and solute is
completely soluble]
A
C
D
B
If mass fraction of CaBr
2
and H
2
O are same then molality of
CaBr
2
is 5 m.
If equal moles of NaCl and H
2
O are taken then molality of NaCl is
55.55 m.
If in place of NaCl we use NaBr as solute in option (2) then
molality of NaCl changes.
If mole fraction of NaCl is same as that of H
2
O then molality of
NaCl will be 55.55 m.

39. Solution :

40. If 200 mL of 0.1 M Na
2
SO
4
is mixed with 100 mL of 0.2
M Na
3
PO
4
solution, what is the molarity of Na
+
in the
final solution, if final solution has a density of 1.2
g/mL.
A
C
D
B
0.196 M
0.33 M
1.5 M
0 .66 M

41. If 200 mL of 0.1 M Na
2
SO
4
is mixed with 100 mL of 0.2
M Na
3
PO
4
solution, what is the molarity of Na
+
in the
final solution, if final solution has a density of 1.2
g/mL.
A
C
D
B
0.196 M
0.33 M
1.5 M
0 .66 M

42. Solution :

43. Find the number of iodine atoms present in 40 mL of
its 0.1 M solution.
A
C
D
B
48.1 × 10
20
4.81 × 10
20
6.02 × 10
23
None of these

44. Find the number of iodine atoms present in 40 mL of
its 0.1 M solution.
A
C
D
B
48.1 × 10
20
4.81 × 10
20
6.02 × 10
23
None of these

45. Solution :

46. A solution of H
2
O
2
is labelled as 11.2 V. If the density of
solution is 1.034 g/mL then identity the correct
option.
A
C
D
B
Molarity of solution = 2M
Molality of solution =1/1.034

47. A solution of H
2
O
2
is labelled as 11.2 V. If the density of
solution is 1.034 g/mL then identity the correct
option.
A
C
D
B
Molarity of solution = 2M
Molality of solution =1/1.034

48. Solution :

49. Which of the following options does not represent
concentration of semi-molal aqueous solution of
NaOH having d
solution
= 1.02 g/mL?
A
C
D
B
Molarity =½ M
X
NaOH
= 9/1009
% w/w = 10%
% w/v = 2%

50. Which of the following options does not represent
concentration of semi-molal aqueous solution of
NaOH having d
solution
= 1.02 g/mL?
A
C
D
B
Molarity =½ M
X
NaOH
= 9/1009
% w/w = 10%
% w/v = 2%

51. Solution :

52. Statement 1: As temperature increases, molality of solution
decreases.
Statement 2: Molality of a solution is dependent on
the mass of solute and solvent.
A
C
D
B
Statements 1 and 2 are true. Statement 2 is the correct explanation
for statement 1.
Statements 1 and 2 are true. Statement 2 is NOT the correct
explanation for statement 1.
Statement 1 is true, statement 2 is false.
Statement 1 is false, statement 2 is true.

53. Statement 1: As temperature increases, molality of solution
decreases.
Statement 2: Molality of a solution is dependent on
the mass of solute and solvent.
A
C
D
B
Statements 1 and 2 are true. Statement 2 is the correct explanation
for statement 1.
Statements 1 and 2 are true. Statement 2 is NOT the correct
explanation for statement 1.
Statement 1 is true, statement 2 is false.
Statement 1 is false, statement 2 is true.

54. Solution :
No of moles of solute in 1 Kg of solvent independent
of volume or temp.

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