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Author Question: 40.0 ml of an acetic acid of unknown concentration is titrated with 0.100 M NaOH. After 20.0 mL of ... (Read 54 times)

curls713

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on: Nov 5, 2023
40.0 ml of an acetic acid of unknown concentration is titrated with 0.100 M NaOH.  After 20.0 mL of the base solution has been added, the pH in the titration flask is 5.10.  What was the concentration of the original acetic acid solution?  [Ka(CH3COOH) = 1.8 × 10–5]
◦ 0.11 M
◦ 0.022 M
◦ 0.072 M
◦ 0.050 M
◦ 0.015 M
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Marked as best answer by curls713 on Nov 5, 2023

psuniv

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Reply #1 on: Nov 5, 2023
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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curls713

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Reply 2 on: Nov 5, 2023
Gracias!

parker125

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Reply 3 on: Yesterday
Great answer, keep it coming :)

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