Leave space between each step to add more information. 1.Write a balance chemical equation between the acid and the base. Remember it’s a double replacement reaction with water and a salt forming. 2. Convert the molarity (M) to moles using the volume. You will need to change the volume to Liters (divide by 1000) Directions for solving titration problems

3. Convert the moles of acid to moles of base (base to acid) using molar ratios from the balanced chemical equation. 4. To get concentration (molarity), divide the moles by the volume. Directions for solving titration problems

Objectives Predict the product of an acid-base reaction. Calculate the molarity of an unknown acid or base. Chapter 15 - Section 3 Neutralization and Titrations

Standards IE 1e Solve scientific problems by using quadratic equations and simple trigonometric, exponential and logarithmic function Chapter 15 - Section 3 Neutralization and Titrations

Neutralization - All Neutralizations Are the Same Reaction A neutralization reaction is the reaction between an acid and base to form water molecules and a salt. When solutions of a strong acid and a strong base, having exactly equal amounts of H 3 O + (aq) and OH − (aq) ions, are mixed, the hydronium and hydroxide ions react to form water. H 3 O + (aq) + OH − (aq)  2H 2 O(l) Chapter 15 - Section 3 Neutralization and Titrations

Suppose that hydrochloric acid, HCl, and the base was sodium hydroxide, NaOH are mixed. The result will be a solution of water and a salt HCl + NaOH  HOH + NaCl Chapter 15 - Section 3 Neutralization and Titrations Neutralization - All Neutralizations Are the Same Reaction

If 20.0 mL of M aqueous hydrochloric acid is required to neutralize 30.0 mL of an aqueous solution of calcium hydroxide, what is the concentration of the calcium hydroxide solution? 1. Write a balance chemical equation between the acid and the base. Remember it’s a double replacement reaction with water and a salt forming. HCl + Ca(OH) 2  CaCl 2 + HOH 2 2

If 20.0 mL of M aqueous hydrochloric acid is required to neutralize 30.0 mL of an aqueous solution of calcium hydroxide, what is the concentration of the calcium hydroxide solution? 2. Convert the molarity (M) to moles using the volume. You will need to change the volume to Liters (divide by 1000)

If 20.0 mL of M aqueous hydrochloric acid is required to neutralize 30.0 mL of an aqueous solution of calcium hydroxide, what is the concentration of the calcium hydroxide solution? 3. Convert the moles of acid to moles of base (base to acid) using molar ratios from the balanced chemical equation. HCl + Ca(OH) 2  CaCl 2 + HOH 22

If 20.0 mL of M aqueous hydrochloric acid is required to neutralize 30.0 mL of an aqueous solution of calcium hydroxide, what is the concentration of the calcium hydroxide solution? 4. To get concentration (molarity), divide the moles by the volume. 2 Sig figs

Now you try! A 25.0 mL solution of H 2 SO 4 is completely neutralized by 18.0 mL of 1.5 M NaOH using phenolphthalein as an indicator. What is the concentration of the H 2 SO 4 solution?

H 2 SO 4 + NaOH  Na 2 SO 4 + HOH 2 2

A 25.0 mL solution of H 2 SO 4 is completely neutralized by 18.0 mL of 1.5 M NaOH using phenolphthalein as an indicator. What is the concentration of the H 2 SO 4 solution? H 2 SO 4 + NaOH  Na 2 SO 4 + HOH 2 2

A 25.0 mL solution of H 2 SO 4 is completely neutralized by 18.0 mL of 1.5 M NaOH using phenolphthalein as an indicator. What is the concentration of the H 2 SO 4 solution? H 2 SO 4 + NaOH  Na 2 SO 4 + HOH Sig figs