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Author Question: A 50.00-mL sample of a 1.00 M solution of the diprotic acid H2A (Ka1 = 1.0 106 and Ka2 = 1.0 1010) ... (Read 25 times)

amal

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on: Mar 21, 2021

Question 1

A 50.00-mL sample of 0.100 M KOH is titrated with 0.171 M HNO3. Calculate the pH of the solution after 52.00 mL of HNO3 is added.

◦ 12.58
◦ 1.06
◦ 1.42
◦ 12.94
◦ None of these are correct.

Question 2

A 50.00-mL sample of a 1.00 M solution of the diprotic acid H2A (Ka1 = 1.0 × 10–6 and Ka2 = 1.0 × 10–10) is titrated with 2.00 M NaOH. How many mL of 2.00 M NaOH must be added to reach a pH of 10?

◦ 0 mL
◦ 12.5 mL
◦ 25.0 mL
◦ 37.5 mL
◦ None of these are correct.
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Marked as best answer by amal on Mar 21, 2021

vish98

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Reply #1 on: Mar 21, 2021
Lorsum iprem. Lorsus sur ipci. Lorsem sur iprem. Lorsum sur ipdi, lorsem sur ipci. Lorsum sur iprium, valum sur ipci et, vala sur ipci. Lorsem sur ipci, lorsa sur iprem. Valus sur ipdi. Lorsus sur iprium nunc, valem sur iprium. Valem sur ipdi. Lorsa sur iprium. Lorsum sur iprium. Valem sur ipdi. Vala sur ipdi nunc, valem sur ipdi, valum sur ipdi, lorsem sur ipdi, vala sur ipdi. Valem sur iprem nunc, lorsa sur iprium. Valum sur ipdi et, lorsus sur ipci. Valem sur iprem. Valem sur ipci. Lorsa sur iprium. Lorsem sur ipci, valus sur iprem. Lorsem sur iprem nunc, valus sur iprium.
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amal

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Reply 2 on: Mar 21, 2021
Excellent

skipfourms123

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Reply 3 on: Yesterday
:D TYSM

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