Calculate the pH to the correct number of significant figures for solutions with the following concentrations of H3O+ or OH? . |
Part A Part complete [H3O+] = 2.5×10?5 M SubmitPrevious AnswersRequest Answer Part B Part complete [OH?] = 10?3 M
SubmitPrevious AnswersRequest Answer Part C Part complete [H3O+] = 3.50×10?9 M
SubmitPrevious AnswersRequest Answer Part D Part complete [H3O+] = 9×10?3 M
SubmitPrevious AnswersRequest Answer Part E Part complete [OH?] = 15 M
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Answer - Part A
[H3O+] = 2.5×10?5 M
pH = -log[H3O+]
pH = -log[2.5*10-5]
pH = 4.6
Part - B
[OH?] = 10?3 M
pOH = -log[10-3]
pOH = 3
pH = 14-3 = 11
pH+pOH = 14
Part C. [H3O+] = 3.5*10-9 M
pH = -log[H3O+]
pH = -log[ 3.5*10-9]
pH = 8.4559
Part D -
[H3O+] = 9*10-3 M
pH = -log[H3O+]
pH = -log[ 9*10-3]
pH = 2.0457
Part E - [OH-] = 15M
Here it seems mistake beacause pOH beaceme (-1.176), which is not possible.
let us assume,
[OH-] = 0.15M
pOH = -log[0.15]
pOH = 0.823
pH = 14-0.823 = 13.176
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