A 350-ml buffer solution was prepared by a chemist from mixing 0.135 M CH3COOH and 0.100 M CH3COOK. Accidentally, during the experiment, you added 12 ml of an unlabeled solution to the buffer solution. This was later on identified by your groupmate to be 1.5 M HCl which was mistakenly left unlabeled when she went out to urinate. Compute for the following; use the pkb value of 7.62. C: 12.01 H: 1.01 Cl: 35.45 O: 15.99 K: 39.10
A 350-ml buffer solution was prepared by a chemist from mixing 0.135 M CH3COOH and 0.100 M CH3COOK. Accidentally, during the experiment, you added 12 ml of an unlabeled solution to the buffer solution. This was later on identified by your groupmate to be 1.5 M HCl which was mistakenly left unlabeled when she went out to urinate. Compute for the following; use the pkb value of 7.62. C: 12.01 H: 1.01 Cl: 35.45 O: 15.99 K: 39.10
Chapter15: Acid-base Equilibria
Section: Chapter Questions
Problem 8ALQ: You have a solution of the weak acid HA and add some of the salt NaA to it. What are the major...
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1. The number of moles of HCl contained in the 12-mL solution added
2. The number of moles of CH3COOH which participated in the reaction upon adding 12-mL of 1.5 M HCl
3. The number of moles of CH3COOK which participated in the reaction upon adding 12-mL of 1.5 M HCl
4. The pH of the original buffer solution
5. The pH of the final buffer solution
6. The final ratio of the CH3COOH and CH3COOK
7. The change in pH, in percentage
*Use 2 decimal places
Transcribed Image Text:A 350-ml buffer solution was prepared by a chemist from mixing 0.135 M
CH3COOH and 0.100 M CH3COOK. Accidentally, during the experiment, you
added 12 ml of an unlabeled solution to the buffer solution. This was later
on identified by your groupmate to be 1.5 M HCl which was mistakenly left
unlabeled when she went out to urinate. Compute for the following; use the
pkb value of 7.62.
C: 12.01 H: 1.01 Cl: 35.45 O: 15.99
K: 39.10
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