CHM 40
Thursday 2/11/10
HW chapter 15
Name
1.
Calculate the molarity of each of the following solutions
a. 22.6 g LiCl in a 2.8 L solution
b. 4.3 moles of NaBr in a 154.4 mL solution
2.
A laboratory procedure calls for making 400.0 mL of a 1.1 M NaNO3 solution. What mass of NaNO3
(in g ) is needed?
3.
a. If 123 mL of a 1.1M glucose solution is diluted to 500.0 mL, what is the molarity of the diluted
solution?
b. To what volume should you dilute 25.0 mL of a 10.0 M H2SO4 solution to obtain a 0.150 M H2SO4
4.
Calculate the mass in grams of solute present in each of the following
a. 225 g of 2.91% ammonium nitrate solution
b. 1.00 kg of 4.95% potassium bromide solution
5.
Many metal ions are precipitated from solution by the sufide ion. As an example, consider treating a
solution of copper (II) sulfate with sodium sulfide solution
CuSO4(aq) + Na2S(aq)  CuS(s) + Na2SO4(aq)
What volume of 0.105 M Na2S solution would be required to precipitate all of the copper (II) ion from 27.5
mL of 0.121 M CuSO4 solution?
6.
Consider the following reaction:
2Na3PO4(aq) + 3 CuCl2(aq)  Cu3(PO4)2(s) + 6 NaCl(aq)
How much Cu3(PO4)2 (in grams) will be produced when 80.0 mL of 0.175 M Na3PO4 reacted with
95.4 mL of 0.102 M CuCl2?
7.
What volume of 0.101 M HCl is required to neutralize 12.7 mL of 0.501 M Ca(OH)2?
*hint: write a balanced chemical equation
8.
A solution of the sparingly soluble base Ca(OH)2 is prepared in a volumetric flask by dissolving 5.21 mg
of Ca(OH)2 to a total volume of 1000.0 mL. Calculate the molarity and normality of the solution