Solutions Ch 15 Review 2007
1.
Calculate the molarity of a solution of 0.0716 g of KMnO 4 in 2.50 mL of solution.
(Atomic weights: K = 39.09, Mn = 54.94, O = 16.00).
2.
The solubility of hexanol, CH3(CH2)5OH, is 0.60 g per 0.10 L. What is the molarity
of the solution?
(Atomic weights: C = 12.01, O = 16.00, H = 1.008).
3.
The trigylceride (C57H110O6) content of a blood sample is 125 mg in 10.0 mL. What
is the molarity of the trigylceride?
(Atomic weights: C = 12.01, H = 1.08, O = 16.00).
4.
The density of a 72.0% by weight aqueous solution of ethanol (CH3CH2OH) is
0.8644 g/cm3. What is the molarity of the solution?
(Atomic weights: C = 12.01, H = 1.008, O = 16.00).
5.
The solubility of NH3 gas in water is 33.1% by weight and the density is 0.998 g/cm3.
What is the molarity of a saturated solution of ammonia in water?
(Atomic weights: N = 14.01, H = 1.008, O = 16.00).
6.
The density of a 64.0% by weight aqueous solution of glycerol (C 3H8O3) is 1.1663
g/cm3. What is the molarity of the solution?
(Atomic weights: C = 12.01, H = 1.008, O = 16.00).
7.
Determine the number of moles of solute present in 255 mL of 1.25 M H 2SO4.
(Atomic weights: S = 32.06, H = 1.008, O = 16.00).
8.
Determine the number of moles of solute present in 416 mL of 3.75 M HBr solution.
(Atomic weights: Br = 79.9, H = 1.008).
9.
Determine the number of moles of solute present in 2.50 mL of 0.1812 M KMnO 4
solution.
(Atomic weights: K = 39.10, Mn = 54.94, O = 16.00).
10. Determine the mass (g) of solute required to form 275 mL of a 0.5151 M KClO 4
solution.
(Atomic weights: K = 39.10, O = 16.00, Cl = 35.45).
11. How many grams of C6H12O6 are required to prepare 250.0 mL of a 0.250 M
solution?
(Atomic weights: C = 12.01, H = 1.008, O = 16.00).
12. Determine the mass (g) of solute required to form 500.0 mL of a 0.480 M MgCl2.
(Atomic weights: Mg = 24.30, Cl = 35.45).
13. A 25.0 mL sample of concentrated HCl (12.0 M) is diluted to a final volume of 750.0
mL. What is the molarity of the final solution?
(Atomic weights: H = 1.008, Cl = 35.45).
14. A 25.0 mL sample of concentrated HBr (7.42 M) is diluted to a final volume of 500.0
mL. What is the molarity of the final solution?
(Atomic weights: H = 1.008, Br = 79.9).
15. A 10.0 mL sample of concentrated HI (5.51 M) is diluted to a final volume of 250.0
mL. What is the molarity of the final solution?
(Atomic weights: H = 1.008, I = 126.9).
16. What volume (mL) of 1.57 M AgNO 3 should be used to prepare 250.0 mL of a 0.200
M solution?
(Atomic weights: Ag = 107.87, N = 14.01, O = 16.00).
17. A 40.0% NaBr solution has a density of 1.42 g/mL. What is the molality of this
solution?
(Atomic weights: Na = 23.0, Br = 79.9).
18. A 50.0 mL sample of a 37.0% HCl solution has a density of 1.19 g/mL. The sample is
diluted to a volume of 0.400 L. What is the molarity of the final solution?
(Atomic weights: H = 1.008, Cl = 35.45).
19. A 30.0% KBr solution has a density of 1.50 g/mL. What is the molality of this
solution?
(Atomic weights: K = 39.0, Br = 79.9).
20. A solution of benzene, C6H6, dissolved in chloroform, CHCl3, has a mole fraction of
C6H6 equal to 0.254. What is the molality of C6H6?
(Atomic weights: C = 12.00, H = 1.008, Cl = 35.45).
21. A solution of benzene, C6H6, dissolved in chloroform, CHCl3, has a mole fraction of
C6H6 equal to 0.254. What is the molality of C6H6?
(Atomic weights: C = 12.00, H = 1.008, Cl = 35.45).
22. What is the mole fraction of AgNO3 in a solution prepared from 0.162 moles of
AgNO3 and 5.43 moles of water?
(Atomic weights: Ag = 107.87, N = 14.01, O = 16.00).
23. What is the mole fraction of urea, (NH2)2CO in an aqueous solution that is 10.0%
urea by mass?
(Atomic weights: C = 12.01, N = 14.01, H = 1.008, O = 16.00).
24. What is the mole fraction of CH3OH in a solution containing 40.0 g of CH3OH and
54.0 g of H2O?
(Atomic weights: C = 12.01, O = 16.00, H = 1.008).
25. The freezing point of an aqueous solution of a nonvolatile nonelectrolyte is -0.072oC.
What is the normal boiling point of the same solution? (K f = -1.86oC/m, Kb =
+0.512oC/m).
26. A 0.100 m solution of K2SO4 in water freezes and boils at what temperatures? (Kf =
-1.86oC/m).
27. The solubility of a gas in a liquid is 50g/100ml at 500 mm Hg, what will the solubility be at
760 mm Hg?
28. Define solution, suspension and colloid by particle size, filterability, settling and Tyndall
effect.
29. What does a point in a solubility graph represent if on the line, below the line, above the
line?
30. The freezing point of a 0.01 m aqueous solution of a nonvolatile electrolyte is 0.072oC. What is the normal boiling point of the same solution? (K f = -1.86oC/m, Kb
= +0.512oC/m).