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. Single choice

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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. Single choice

Similar Questions

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−] _____.

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

More Practical Tools for Students Powered by AI Study Helper

Making Your Study Simpler

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