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Author Question: In a solution prepared by dissolving 0.100 mole of propanoic acid in enough water to make 1.00 L of ... (Read 97 times)

tingc95

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on: Mar 21, 2021

Question 1

If you know Kb for ammonia, NH3, you can calculate the equilibrium constant, Ka, for the following reaction: NH4+ NH3 + H+ by the equation:

◦ Ka = Kw× Kb.
◦ Ka = Kw / Kb.
◦ Ka = 1 / Kb.
◦ Ka = Kb / Kw.
◦ None of these are correct.

Question 2

In a solution prepared by dissolving 0.100 mole of propanoic acid in enough water to make 1.00 L of solution, the pH is observed to be 2.793. The Ka for propanoic acid (HC3H5O2) is:

◦ 1.61 × 10–3.
◦ 2.60 × 10–5.
◦ 1.64 × 10–2.
◦ 3.79 × 10–10.
◦ None of these are correct.
Chemistry: An Atoms First Approach ¦ Zumdahl, DeCoste ¦ 3rd Edition
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Marked as best answer by tingc95 on Mar 21, 2021

johnharpe

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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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tingc95

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Reply 2 on: Mar 21, 2021
Excellent

komodo7

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Reply 3 on: Yesterday
:D TYSM

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