Monday May 18 Objective: Calculate the pH of any solution. Checkpoint:

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Monday May 18 Objective: Calculate the pH of any solution. Checkpoint: Write the dissociation equations for the following acids and bases: HCO3-  NaOH  Calculate the pH of the following solutions: An HCl solution that is 1.0 x 10-3 M. [HBr] = 1.0 x 10-5 M. [H+] = 6.32 x 10-4 M Homework: pH worksheet (due Tuesday)

Arrhenius Acids and Bases Acid: increases [H+] in solution. Base: increases [OH-] in solution Checkpoint: HCO3-  NaOH  H+ + CO32- Na+ + OH-

pH = -log[H+] pH = -log[1.0 x 10-3] pH = -(-3) pH = 3, acidic What is the pH of a solution of an HCl solution that is 1.0 x 10-3 M? pH = -log[1.0 x 10-3] pH = -(-3) pH = 3, acidic

pH = -log[H+] pH = -log[1.0 x 10-5] pH = -(-5) pH = 5, acidic What is the pH of [HBr] = 1.0 x 10-5 M? pH = -log[1.0 x 10-5] pH = -(-5) pH = 5, acidic

pH = -log[H+] pH = 3.2, acidic pH = -log[6.32 x 10-4 ] What is the pH of [H+] = 6.32 x 10-4 M? pH = -log[6.32 x 10-4 ] pH = 3.2, acidic

5/5 with color, 4/5 without color pH poster due today 5/5 with color, 4/5 without color

HCl  H+ + Cl- NaOH  Na+ + OH- Strong Acids and Bases 100 100 100 100 1000 1000 1000 1000 1000 1000 1,000,000 1,000,000 1,000,000 1,000,000 1,000,000 1,000,000

HCN  H+ + CN- NH3 + HOH  NH4 + + OH- Weak Acids and Bases 100 5 5 50 5% dissociation HCN  H+ + CN- 100 5 5 50 1000 50 1% dissociation NH3 + HOH  NH4 + + OH- 100 1 1 1,000,000 10,000 10,000

pH = -log[H+] pH = -log[0.012] pH = 1.92, acidic = What is the pH of a solution that is made from dissolving 0.87 grams HCl into 2.0 L of water? 0.87 grams 1 mol M = 0.024 mol / 2.0 L = 0.012 M = x 0.024 mol 36.46 g pH = -log[0.012] pH = 1.92, acidic

pOH = -log[OH-] pH + pOH = 14 What is the pH of a solution that has 1.0 x 10-3 M NaOH concentration? Is it acidic, basic, or neutral? pOH = -log[1.0 x 10-3] pOH = -(-3) pH + 3 = 14 pH = 11, basic

pOH = -log[OH-] pH + pOH = 14 What is the pH of a solution that has 1.0 x 10-2 M KOH concentration? Is it acidic, basic, or neutral? pOH = -log[1.0 x 10-2] pOH = -(-2) pH + 2 = 14 pH = 12, basic

pOH = -log[OH-] pH + pOH = 14 What is the pH of a solution that has [OH-] = 3.4 x 10-5 Is it acidic, basic, or neutral? pOH = -log[3.4 x 10-5] pOH = 4.47 pH + (4.47) = 14 pH = 9.53, basic

pH = -log[H+] pH = -log[0.20] pH = 0.70, acidic 2.0 x 0.10 = 0.20 M What is the pH of a solution that has 2.0 M of HF, a weak acid? Assume 10% dissociation. Is it acidic, basic, or neutral? 2.0 x 0.10 = 0.20 M [H+] = 0.20 M pH = -log[0.20] pH = 0.70, acidic

“Having fun with pH” answer key skip