Stoichiometry 2 review

SOLUTION CONCENTRATIONS
Show calculation setups and answers for all problems.
1. What will be the percent composition by mass of a solution made by
dissolving 12.0 g of zinc nitrate, ZN(NO3)2, in 45.0 g of water?
Zn(NO3)2 _____________________________________________________
H2O ______________________________________
2. How many moles of sodium hydroxide, NaOH, are required to prepare 2.00
L of 0.380 M solution?
____________________________________
3. What will be the molarity of a solution if 3.50 g of potassium hydroxide,
KOH, are dissolved in water to make 150. mL of solution?
________________________________________
4. How many milliliters of 0.400 M solution can be prepared by dissolving
5.00 g of KOH in water?
________________________________________
5. How many grams of potassium bromide, KBr, could be recovered by
evaporating 650.g of 15 percent KBr solution to dryness?
_______________________________________

6. How many millilites of 1.00 M HCl is needed to prepare 300. m: of 0.250
M HCl solution?
________________________________________
7. A sample of potassium hydrogen oxalate, KHC2O4, weighing 0.717 g, was
dissolved in water and titrated with 18.47 mL of an NaOH solution.
Calculate the molarity of the NaOH solution.
____________________________________
8. How many grams of hydrogen chloride are in 35 mL of concentrated (12
M) HCl solution?
_________________________________________
9. A sulfuric acid solution has a density of 1.73 g/mL and contains 80. percent
H2SO4 by mass. What is the molarity of this solution?
_________________________________________
10. Sulfuric acid reacts with sodium hydroxide according to this equation:
H2SO4 + 2 NaOH → Na2SO4 + 2 H2O
A 10.00 mL of the H2SO4solution required 13.71 mL of 0.309 M NaOH
for neutralization. Calculate the molarity of the acid.
___________________________________________