if a solution has a proton concentration of 10-11 M, what is the hydroxide ion concentration?
Please choose the correct answer from the following choices, and then select the submit answer button.

Question

BlackTom AI · Accepted Answer

To evaluate the hydroxide ion concentration when the proton concentration is 1e-11 M, we use the water autoionization constant, Kw, which is 1e-14 at standard conditions.

Option 1: 10-11 M (interpreted as 1e-11 M). This value corresponds to [H+], not [OH-], since [H+] is given as 1e-11 M. It does not represent the hydroxide concentration sought here.

Option 2: 3 M. This would imply an extremely high concentration of hydroxide ions and is incompatible with the very small [H+] given; such a drastic mismatch would violate Kw and typical aqueous equilibria.

Option 3: 0.001 M (1e-3 M). Calculating via Kw = [H+][OH-], we rearrange to [OH-] = Kw / [H+] = 1e-14 / 1e-11 = 1e-3 M, which is 0.001 M. This is the consistent result for the given [H+].

Option 4: 0.01 M (1e-2 M). If [OH-] were this value, the product [H+][OH-] would be 1e-11 × 1e-2 = 1e-13, which is not equal to Kw, so this option does not satisfy the equilibrium constraint.

In summary, the calculation relies on the fundamental relation [OH-] = Kw / [H+], and substituting the provided values yields 1e-3 M. The other options fail to satisfy either the definition of Kw or the correspondence to [H+].

if a solution has a proton concentration of 10-11 M, what is the hydroxide ion concentration? Please choose the correct answer from the following choices, and then select the submit answer button.

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if a solution has a proton concentration of 10-11 M, what is the hydroxide ion concentration? Please choose the correct answer from the following choices, and then select the submit answer button.

查看解析

登录即可查看完整答案

类似问题

What is true about an acidic solution at 25°C?

What is the pH of a solution when [OH−] = 3.8 × 10−5. Is this solution acidic or basic?

Match the correct response When the pH of a solution rises what happens to the followings 1: [H3O+] [H3O+] 2: pOH 3: [OH-] [OH-] 4: [H3O+]x [OH-] [H3O+] x [OH-]

In a 1.2 M solution of KOH, a strong base, [H3O+] = _____, and [OH−] = _____.

As the pH of a solution rises, [H3O+] _____, pOH _____, and [OH−] _____.

A vinegar sample had a pH of 3.88. This corresponds to [OH-] =

Which of the following represents the most acidic solution?

In a 1.2 M solution of KOH, a strong base, [H3O+] = _____, and [OH−] = _____.

更多留学生实用工具

考试浏览器助手

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希望你的学习变得更简单

In a 1.2 M solution of KOH, a strong base, [H3O+] = _, and [OH−] = _.

As the pH of a solution rises, [H3O+] ___, pOH _, and [OH−] ___.

In a 1.2 M solution of KOH, a strong base, [H3O+] = _, and [OH−] = _.