DO NOW!!! What is the molarity of a 500mL solution that contains 0.29 moles of hydrochloric acid, HCl? 2. What is the pH and pOH of that solution? 3. If you were to use cabbage juice to test human blood, what color and pH do you expect it to be? And why? (If you don’t know the pH of human blood, look it up…) Agenda -Turn in your completed cabbage pH lab from yesterday -DO NOW -Chapter 15-3 Titration

Chp 15-3 Titrations Key Concept: How much acid and base are required to “cancel” each other out?

Neutralization Reactions A neutralization reaction between a strong acid and a strong base in aqueous solution produces an ionic compound (a salt) and water. Examples: 1. NaOH (aq) + HCl (aq)  2. KOH (s) + HNO 3 (aq) 

Check-in Sulfuric acid, H 2 SO 4 (aq), reacts with magnesium hydroxide, Mg(OH) 2 (aq). Write a balanced equation for the reaction that occurs. ________ + ________  ______+_______

Titrations Titration: a procedure in which a neutralization reaction is monitored with an indicator allowing you to calculate the unknown concentration of an acid or base. –Equivalence point: when the number of moles of [H + ] is equal to the number of moles of [OH - ] in the solution –Use the equation: (M= molarity, V= volume) M acid V acid = M base V base

Example If 25.0 mL of M nitric acid, HNO3, solution is required to neutralize 62.0 mL of sodium hydroxide, NaOH, what is the molarity of the NaOH?

Check-in If 20.6 mL of 0.010M aqueous NaOH is required to titrate 30.0 mL of HCl (aq) to the equivalence point, what is the molarity of the HCl solution?