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1. Calculate the pH of a solution prepared by mixing 30.00 mL of a 0.15-M KOH solution with 50.00 mL of a .39-M HBr solution. Ã‚

2. Ã‚ 45.0 mL of a 0.10-M formic acid (HCHO2, Ka=1.7x10^-4) solution was titrated with a 0.20-M NaOH solution. Ã‚ What is the equivalent volume? Ã‚ Calculate which is in excess.

3. Ã‚ What is the pH of the acidic solution before titration?

4. Ã‚ What is the pH of the reaction mixture after 10.0 mL of NaOH was added?

5. Ã‚ What is the pH of the reaction mixture at the equivalence point?

6. Ã‚ What is the pH of the reaction mixture after 25.0 mL of base was added?

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