This document discusses solubility rules and concepts related to concentration of solutions including molarity, percent composition by mass and volume, and how to calculate amounts of solute and solvent needed to prepare solutions of a given concentration. It also provides examples of solubility rules for various ionic compounds in water and problems involving calculations to determine the mass of solute needed or the volume or concentration of a prepared solution.

1. Solubility, solubility rules, % and Molarity
1.- How do temperatue and pressure affect the solubility of solids and gases in wáter?
2.- If NaCl has a solubility of 36 g /100 g of water at 20 C, how many grams of water are
needed to prepare a saturated solution containing 80 g of NaCl?
3.- KNO3 has a solubility of 32 g of KNO3/100 g of water at 20 C. State if the following forms a
saturated or unsaturated solution at 20 C:
a)32 g of KNO3 and 200 g of water
b)19 g of KNO3 and 50 g of water
4.- Indicate whether each of the following ionic compounds is soluble or insoluble in water:
a)KCl b)MgSO4 c)CuS d)AgNO3 e)Ca(OH)2
5.- How many milliliters of a 12% (v/v) propyl alcohol solution would you take to obtain 4.5 ml
of propyl alcohol?
6.- A solution is prepared with 70 g of HNO3 and 130 g of water. What is the %(m/m) of the
solution?
7.- How many liters of a 2.5 M KNO3 solution can be prepared from 60 g of KNO3?
8.- How would you prepare 250 ml of a 2 M KCl solution?
9.- What is the molarity of a solution containing 15.6 g of KCl in 274 ml of solution?
10.- How many grams of Na2SO4 are in 428 ml of a 0.45 M Na2SO4 solution?