Suppose we titrate 20.0 mL of 0.100 M HCHO2 (Ka = 1.8 × 10–4) with 0.100 M NaOH. Calculate the pH. After a total of 15.0 mL of base has been added: pH = Please only answer the incorrect question, thank you so much!

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Suppose we titrate 20.0 mL of 0.100 M HCHO(Ka = 1.8 × 10–4) with 0.100 NaOH. Calculate the pH.

After a total of 15.0 mL of base has been added: pH =

Please only answer the incorrect question, thank you so much!

Suppose we titrate 20.0 ml of 0.100 M HCHO2 (K, - 1.8 x 10-4) with 0.100 M NAOH. Calculate the pH.
Your answer is correct.
Before any base is added:
pH =
2,37
Hint
Your answer is correct.
When half of the HCHO2 has been neutralized:
pH =
3.74
Hint
* Your answer is incorrect.
After a total of 15.0 mL of base has been added:
pH =
i
1,54
Hint
Assistance Used
Recall the relationship between K, and HCHO2, CH02.
Your answer is correct.
At the equivalence point:
pH =
8.22
Hint
Transcribed Image Text:Suppose we titrate 20.0 ml of 0.100 M HCHO2 (K, - 1.8 x 10-4) with 0.100 M NAOH. Calculate the pH. Your answer is correct. Before any base is added: pH = 2,37 Hint Your answer is correct. When half of the HCHO2 has been neutralized: pH = 3.74 Hint * Your answer is incorrect. After a total of 15.0 mL of base has been added: pH = i 1,54 Hint Assistance Used Recall the relationship between K, and HCHO2, CH02. Your answer is correct. At the equivalence point: pH = 8.22 Hint
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