Solution Found!
Calculate [OH ] given [H3O+] in each aqueous solution and
Chapter 14, Problem 63P(choose chapter or problem)
Calculate \(\mathrm{[OH^-]}\) given \(\mathrm{[H_3O^+]}\) in each aqueous solution and classify the solution as acidic or basic.
(a) \(\mathrm{[H_3O^+]=1.5 \times 10^{-9} ~M}\)
(b) \(\mathrm{[H_3O^+]=9.3 \times 10^{-9} ~M}\)
(c) \(\mathrm{[H_3O^+]=2.2 \times 10^{-6} ~M}\)
(d) \(\mathrm{[H_3O^+]=7.4 \times 10^{-4} ~M}\)
Equation Transcription:
Text Transcription:
[OH^-]
[H_3O^+]
[H_3O^+]=1.5 x 10^{-9} M
[H_3O^+]=9.3 x 10^{-9} M
[H_3O^+]=2.2 x 10^{-6} M
[H_3O^+]=7.4 x 10^{-4} M
Questions & Answers
QUESTION:
Calculate \(\mathrm{[OH^-]}\) given \(\mathrm{[H_3O^+]}\) in each aqueous solution and classify the solution as acidic or basic.
(a) \(\mathrm{[H_3O^+]=1.5 \times 10^{-9} ~M}\)
(b) \(\mathrm{[H_3O^+]=9.3 \times 10^{-9} ~M}\)
(c) \(\mathrm{[H_3O^+]=2.2 \times 10^{-6} ~M}\)
(d) \(\mathrm{[H_3O^+]=7.4 \times 10^{-4} ~M}\)
Equation Transcription:
Text Transcription:
[OH^-]
[H_3O^+]
[H_3O^+]=1.5 x 10^{-9} M
[H_3O^+]=9.3 x 10^{-9} M
[H_3O^+]=2.2 x 10^{-6} M
[H_3O^+]=7.4 x 10^{-4} M
ANSWER:
Step 1 of 5
Here, we are going to calculate hydroxyl ion concentration in each of the solutions.
In pure water, one molecule donates a proton and acts as an acid and another water molecule accepts a proton and acts as a base at the same time. The following equilibrium exists:
The equilibrium constant for the reaction is given by:
Where, is called the ionic product of water and its value is
We can distinguish acidic, neutral and basic aqueous solutions by the relative values of the 
Acidic:
Neutral:
Basic:
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