Multiple Choice
Calculate [OH-] in a solution given that [H+] is 1.0 x 10-11.8 M.
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- 1. Introduction to Biochemistry4h 36m
- What is Biochemistry?7m
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- Review 4: Amino Acid Oxidation, Oxidative Phosphorylation, & Photophosphorylation1h 48m
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- Photophosphorylation 29m
- Photophosphorylation 310m
- Practice: Amino Acid Oxidation 12m
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- Practice: Oxidative Phosphorylation 15m
- Practice: Oxidative Phosphorylation 24m
- Practice: Oxidative Phosphorylation 35m
- Practice: Photophosphorylation 15m
- Practice: Photophosphorylation 21m
2. Water
Autoionization of Water
Multiple Choice
Calculate [H+] in a solution given that [OH-] is 1.0 x 10-10 M.
A
1.0 x 10-2 M
B
1.0 x 10-3 M
C
1.0 x 10-4 M
D
1.0 x 10-5 M
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Verified step by step guidance1
Understand the relationship between [H+] and [OH-] in water, which is governed by the ion product of water (Kw). At 25°C, Kw is 1.0 x 10^-14 M^2.
Use the formula Kw = [H+][OH-] to find [H+]. Rearrange the formula to solve for [H+]: [H+] = Kw / [OH-].
Substitute the given [OH-] value into the equation: [H+] = 1.0 x 10^-14 M^2 / 1.0 x 10^-10 M.
Perform the division to calculate [H+]. This involves dividing the ion product of water by the hydroxide ion concentration.
Compare the calculated [H+] with the provided options to identify the correct answer.
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