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Author Question: What is the pH of a 0.40 mol L-1 H2Se solution that has the stepwise dissociation constants Ka1 = ... (Read 111 times)

Tazate

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on: Nov 18, 2019

Question 1

Calculate the concentration of bicarbonate ion, HCO3-, in a 0.010 mol L-1 H2CO3 solution that has the stepwise dissociation constants Ka1 = 4.3 × 10-7 and Ka2 = 5.6 × 10-11.
◦ 4.3 × 10-9 mol L-1
◦ 5.6 × 10-11 mol L-1
◦ 4.3 × 10-7 mol L-1
◦ 6.6 × 10-5 mol L-1

Question 2

What is the pH of a 0.40 mol L-1 H2Se solution that has the stepwise dissociation constants Ka1 = 1.3 × 10-4 and
◦ 5.57
◦ 4.28
◦ 2.14
◦ 3.89
Chemistry: A Molecular Approach (Canadian) ¦ Tro, Fridgen, Shaw ¦ 2nd Edition
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Marked as best answer by Tazate on Nov 18, 2019

otokexnaru

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Reply #1 on: Nov 18, 2019
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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Tazate

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Reply 2 on: Nov 18, 2019
:D TYSM

kalskdjl1212

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

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