1. Solutions and Molarity

2. 1. 13. 8 L of CO2 @ STP is dissolved in 250. 0 mL of water
L of STP is dissolved in mL of water. What is the molarity of the resulting solution?
13.8 L CO2
x 1 mol CO2
Molarity
22.4 L =
0.250 L
= M

3. If a 1. 89 M solution is made by dissolving chlorine gas in 600
If a 1.89 M solution is made by dissolving chlorine gas in mL of water, what volume of Cl2 gas was dissolved?
0.600 L
x mol
x L
= L of Cl2 gas
1 mol
1 L

4. 3. Calculate the molarity of a solution when 2
3. Calculate the molarity of a solution when 2.96 x 1024 FU’s of CaF2 are dissolved in L of water?
2.96 x 1024 FU
x 1 mol
6.02 x 1023 FU
Molarity =
= M
0.500 L

5. 4. How many molecules are dissolved in 1.00 L of water if the molarity of the H2SO4 solution is 0.2 M?
1.00 L
x mol
x x 1023 molecules
= 1 x1023 molecules
1 mol 1L

6. 5. Excess sodium hydroxide solution is added to 80. 0 mL of 0. 336 M
5. Excess sodium hydroxide solution is added to 80.0 mL of M ZnCl2, calculate the mass of zinc hydroxide that will precipitate.
2 NaOH (aq) +ZnCl2(aq) → Zn(OH)2(s) NaCl (aq) L
? g
L ZnCl2
x mole
x mole Zn(OH)2
x g
1 L
1 mole ZnCl2
1 mol
= 2.67 g Zn(OH)2

7. 6. Calculate the volume of 0. 100 M HCl solution that is required to
6. Calculate the volume of M HCl solution that is required to completely neutralize mL of M Ba(OH)2 solution.
2HCl(aq) Ba(OH)2 (aq) → BaCl2(aq) H2O (l)
? L L
0.2500L Ba(OH)2
x mole
x mole HCl
x L
1 L
1 mole Ba(OH)2
0.100 mol
= 1.00 L