What is the [OH–] in an aqueous solution at 25 °C in which [H3O+] = 1.9 10–9 M?

Question

What is the [OH–] in an aqueous solution at 25 °C in which [H3O+] = 1.9  10–9 M?

BlackTom AI · Accepted Answer

First, identify the given data: at 25 °C, the ion-product of water, Kw, is 1.0 × 10^-14. The hydronium concentration is [H3O+] = 1.9 × 10^-9 M.

Next, use the relationship for water autoionization: [H3O+][OH-] = Kw. Solving for [OH-], we get [OH-] = Kw / [H3O+].

Plug in the values: [OH-] = (1.0 × 10^-14) / (1.9 × 10^-9).

Perform the division: 1.0 / 1.9 ≈ 0.5263, and 10^-14 / 10^-9 = 10^-5, so [OH-] ≈ 0.5263 × 10^-5 M.

Expressing with proper significant figures, 0.5263 × 10^-5 M ≈ 5.26 × 10^-6 M. Rounding to two significant figures consistent with the given data, [OH-] ≈ 5.3 × 10^-6 M.

Interpretation: because [H3O+] is greater than the very small neutral-water value (1.0 × 10^-7 M), the solution is acidic enough that [OH-] is suppressed below 1.0 × 10^-7 M, yet the product with [H3O+] still equals Kw. The calculation demonstrates how altering one ion concentration directly dictates the other through Kw.

Chem 1C General Chemis... Self Assessment Quiz 11

What is the [OH–] in an aqueous solution at 25 °C in which [H3O+] = 1.9 10–9 M?

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Chem 1C General Chemis... Self Assessment Quiz 11

What is the [OH–] in an aqueous solution at 25 °C in which [H3O+] = 1.9 10–9 M?

查看解析

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类似问题

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.

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?

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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−] ___.