Practice Problems
Chpt. 10-13 (Bauer)
1.
Calculate the amount of heat energy required to transform 7.50 g of ice (H2O (s))
at 0OC to steam (H2O (g)) at 100.0OC.
2.
Rank the following in order of increasing melting point.
HF , MgO, H2 , HBr , KBr,
3.
4.
Give the concentrations of all ions in each of the following solutions.
(a)
0.50 M Co(NO3)2
(b)
1.0 M FeCl3
Calculate the number of moles of each ion present in each of the following
solutions.
(a)
Na+ ion in 1.00 L of a 0.251 M Na2SO4 solution.
(b)
Cl ion in 5.50 L of a 0.10 M FeCl3 solution.
(c)
NO3 ion in 100.0 mL of a 0.55 M barium nitrate solution.
(d)
NH4+ ion in 250.0 mL of a 0.350 ammonium sulfate solution.
5.
What volume of 3.0 M H2SO4 can be prepared from 100.0 mL of 18.0 M H2SO4?
6.
What volume of 12 M HCl must be used in order to prepare 750 mL of 0.25 M
HCl?
7.
When 5.0 L of water is addd to 1.0 L of 6.0 M HCl what is the concentration of
the resulting solution?
8.
What volume of 0.25 M Na2SO4 is needed to precipitate all of the barium, as
barium sulfate, from 12.5 mL of 0.15 M Ba(NO3)2?
9.
Calculate the mass of CaCO3 precipitate produced when 37.5 mL of 0.149 M
Na2CO3 is mixed with 36.2 mL of 0.158 M CaCl2.
10.
Molarity is defined as,
(a)
grams of solute per liter of water.
(b)
grams of solute per liter of solution.
(c)
moles of solute per liter of water.
(d)
moles of solute per liter of solution.
11.
What mass of K2CrO4 is needed to prepare 5.00 x 102 mL of 0.250 M K2CrO4?
12.
Consider the following reaction.
PCl5 (g)  PCl3 (g) + Cl2 (g)
Suppose that 0.90 mol of PCl5 is placed in a 2.0 L container. Calculate the
equilibrium concentrations of all species once equilibrium is attained assuming
that K=2.0 x 10-4.
13.
For barium fluoride, Ksp = 1.0 x 10-6. Calculate the concentration of fluoride ion
in a saturated solution of barium fluoride. Calculate the solubility of barium
fluoride in mol/L and in g/L.
14.
In a saturated solution of zinc hydroxide the concentration of zinc ion is
7.2 x 10-9 M. Calculate Ksp for zinc hydroxide.
15.
Consider the following reaction.
N2 (g) + O2 (g)

2 NO (g)
Suppose that 6.0 mol of N2 and 6.0 mol of O2 are placed in 2.00 L container.
Calculate the equilibrium concentrations of all species assuming that
K=2.5 x 10-3.
16.
What volume of 1.00 M NaOH is required to titrate 25.0 mL of 0.154 M acetic
acid?
17.
Calculate the pH of each of the following solutions.
(a)
1.00 x 10-3 M Ba(OH)2
(b)
3.50 x 10-2 M HCl
(c)
6.00 M HCl
18.
Calculate the pH of a 1.00 x 10-2 M HC2H3O2 solution. For acetic acid
Ka = 1.8 x 10-5.
19.
The pH of a 0.10 M solution of a weak acid is 3.57. Calculate Ka for the acid.