Chemistry, 26.06.2020 15:01 haileymaree
Calculate the following buffer solutions. A buffer solution was made by dissolving 10.0 grams of sodium acetate in 200.0 mL of 1.00 M acetic acid. Assuming the change in volume when the sodium acetate is not significant, estimate the pH of the acetic acid/sodium acetate buffer solution. The Ka for acetic acid is 1.7 x 10-5. Calculate the ratio of ammonium chloride to ammonia that is required to make a buffer solution with a pH of 9.00. The Ka for ammonium ion is 5.6 x 10-10. After completing the calculations answer the following questions 1) Is the pH of the solution consistent with the Ka or is there a better Ka that could be used? 2) If 100 mL of buffered solution is used, what is the pH change if 20 mL of 0.5M HCl is added? Does the pH change exceed the buffering capacity of the solution? Explain 3) If 100 mL of buffered solution is used, what is the pH change if 20 mL of 0.5M NaOH is added? Does the pH change exceed the buffering capacity of the soltuion? Explain
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