1. INTRODUCTION TO SOLUTIONS/ACIDS AND BASES HONORS CHEMISTRY MAY 27 TH, 2014

2. WHAT IS A SOLUTION? A solution is a homogenous mixture of to or more substances. The most common solutions are aqueous solutions, those with a solid, liquid, or gas in water. A solution has at least two components: - Solvent: The majority component - Solute: The minority component

3. CONCENTRATION The amount of solute in a solution is an important property of a solution. A dilute solution contains small amounts of solute relative to solvent. A concentrated solution contains large amounts of solute relative to solvent.

4. MOLARITY Molarity (M) is a way to express solution concentration. Molarity is defined as the number of moles of solute per liter of solution.

5. PREPARING A SOLUTION Note that molarity is moles of solute/liters of solution, not solvent. To make a solution of a specific molarity, you usually put the solute into a flask and then add water to desired volume of solution.

6. PRACTICE PROBLEMS! Calculate the molarity of a solution made by putting 15.5 g of NaCl into a beaker and adding water to make 1.50L of NaCl solution.

7. DILUTION EQUATION M 1 V 1 = M 2 V 2 Where… - M 1 and V 1 are the molarity and volume of the initial concentrated solution - M 2 and V 2 are the molarity and volume of the final diluted solution

8. PRACTICE PROBLEM To what volume should you dilute 0.100 L of a 15 M NaOH solution to obtain a 1.0 M NaOH solution?

9. SOLUTION STOICHIOMETRY Many chemical reactions take place in aqueous solutions. We know from stoichiometry that coefficients in chemical equations are conversion factors between moles of reactants and moles of products.

10. PRACTICE PROBLEM! How much 0.125 M NaOH solution do we need to completely neutralize 0.225 L of 0.175 M H 2 SO 4 solution?