This document discusses concentration of solutions and different ways to measure concentration. It defines dilute and concentrated solutions, and introduces molarity and molality as units of concentration. Molarity is defined as moles of solute per liter of solution. The document provides examples of how to calculate the molarity of a solution given the mass of solute and volume of solution. It also gives practice problems calculating molarity and molality.

1. Concentration of Solutions Chapter 13.3

2. Objectives Given the mass of solute and volume of solvent, calculate the concentration of a solution Given the concentration of a solution, determine the amount of solute in a given amount of solution Given the concentration of a solution, determine the amount of solution that contains a given amount of solute

5. Practice Problems You have 3.50 L of solution that contains 90.0 g of sodium chloride, NaCl. What is the molarity of that solution? You have 0.8 L of a 0.5 M HCl solution. How many moles of HCl does this solution contain? To produce 40.0 g of silver chromate, you will need at least 23.4 g of potassium chromate in solution as a reactant. All you have on hand in the stock room is 5 L of 6.0 M K2CrO4 solution. What volume of the solution is needed to give you the 23.4 g K2CrO4 need for the reaction?

6. Molality Concentration of a solution expressed in moles of solute per kilogram of solvent. m - symbol Written as 1 m solution of NaOH One molal solution of sodium hydroxide 1 mol NaOH in 1 kg of solvent moles solute (mol) molality = mass of solvent (Kg)

7. Practice Problems A solution was prepared by dissolving 17.1 g of sucrose (table sugar, C12H22O11) in 125 g of water. Find the molal concentration of this solution. A solution of iodine, I2, in carbon tetrachloride, CCl4, is used when iodine is needed for certain chemical tests. How much iodine must be added to prepare a 0.489 m solution of iodine in CCl4 if 100.0 g of CCl4 is used?