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Buffers and Buffer Type Solutions

1. The Common Ion Effect. What is the pH of a solution that contains 0.250-M benzoic acid and 0.600-M sodium benzoate?

2. Buffers. A buffer solution is made of 0.100 M HOCl and 0.250 M NaOCl. What is the pH of the resulting solution when a 15.0-mL portion of 0.200 M HCl is added to 100.0 mL of the buffer?

3. Preparing a Buffer. The pH of blood is 7.40. Calculate the [HCO3-] / [H2CO3] ratio of a bicarbonate-carbonic acid buffer system that will effectively maintain a sample of blood at a pH of 7.40. Hint: the Henderson-Hasselbalch equation is useful for this type of problem.

4. Weak Acid - Strong Base Titration. A 50.0-mL portion of 0.200 M HCOOH is titrated with 35.0 mL of 0.200 M KOH. What is the pH of the resulting solution?

5. Weak Acid - Strong Base Titration. Now consider a titration that is similar to problem 4, except that a 50.0-mL portion of 0.200 M HCOOH has been titrated with 0.200 M KOH to the equivalence point. What is the pH at the equivalence point?

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Category:- Chemistry
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