25. In a titration 17ml of 0.2M NaOH was used to neutralize 10ml of acetic acid (CH3 COOH) What is the molarity of the acetic ac
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Answer:
Final pH: 9.49.
Round to two decimal places as in the question: 9.5.
Explanation:
The conjugate of B is a cation that contains one more proton than B. The conjugate of B is an acid. As a result, B is a weak base.
What's the pKb of base B?
Consider the Henderson-Hasselbalch equation for buffers of a weak base and its conjugate acid ion.
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What's the new salt-to-base ratio?
The 0.005 mol of HCl will convert 0.005 mol of base B to its conjugate acid ion BH⁺.
Initial:
;
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After adding the HCl:
;
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Assume that the volume is still 0.5 L:
.
.
What's will be the pH of the solution?
Apply the Henderson-Hasselbalch equation again:
.
The final pH is slightly smaller than the initial pH. That's expected due to the hydrochloric acid. However, the change is small due to the nature of buffer solutions: adding a small amount of acid or base won't significantly impact the pH of the solution.