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Author Question: The pH of a Ba(OH)2 solution is 10.00. What is the H+ ion concentration of this solution? (Read 37 times)

camac77

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Question 1

The pH of a 0.14 M solution of an unknown monoprotic acid is 5.85. Calculate the Ka of the acid.
◦ 1.4 x 10-6

◦ 1.4 x 10-11

◦ 1.0 x 10-5

◦ 7.1 x 10-9

◦ 2.0 x 10-7


Question 2

The pH of a Ba(OH)2 solution is 10.00.  What is the H+ ion concentration of this solution?
◦ 4.0 × 10–11 M
◦ 1.6 × 10–10 M
◦ 1.3 × 10–5 M
◦ 1.0 × 10–10 M
◦ 10. M


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Marked as best answer by camac77 on Nov 5, 2023

gwisel

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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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camac77

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Reply 2 on: Nov 5, 2023
Thanks for the timely response, appreciate it


emsimon14

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Reply 3 on: Yesterday
Wow, this really help

 

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