Calculate the pH and pOH of an aqueous solution with [H3O+] = 1.7 × 10–8 M.

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BlackTom AI · Accepted Answer

Question restatement: You are asked to calculate the pH and pOH for an aqueous solution with [H3O+] = 1.7 × 10^−8 M.

First, convert the hydronium concentration to pH. By definition, pH = −log10([H3O+]). Here, [H3O+] = 1.7 × 10^−8 M, so log10(1.7 × 10^−8) = log10(1.7) + log10(10^−8) = 0.2304 − 8 = −7.7696. Taking the negative gives pH ≈ 7.7696, which rounds to 7.77.

Next, determine pOH. The relationship between pH and pOH at 25 °C is pH + pOH = 14. Thus, pOH = 14 − pH ≈ 14 − 7.7696 = 6.2304, which rounds to 6.23.

An alternative check uses the water autoionization constant: Kw = [H3O+][OH−] = 1.0 × 10^−14 at 25 °C, so [OH−] = Kw / [H3O+] = (1.0 × 10^−14) / (1.7 × 10^−8) ≈ 5.88 × 10^−7 M. Then pOH = −log10([OH−]) ≈ −log10(5.88 × 10^−7) ≈ 6.230, consistent with the previous calculation.

Context note: A pH of 7 is neutral at 25 °C; since the given pH is slightly above 7, the solution is very mildly basic, which is consistent with [H3O+] being less than 1 × 10^−7 M. The pOH being slightly below 7 aligns with a small but nonzero concentration of hydroxide ions in solution.

Chem 1C General Chemis... Self Assessment Quiz 12

Calculate the pH and pOH of an aqueous solution with [H3O+] = 1.7 × 10–8 M.

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Chem 1C General Chemis... Self Assessment Quiz 12

Calculate the pH and pOH of an aqueous solution with [H3O+] = 1.7 × 10–8 M.

查看解析

登录即可查看完整答案

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−] ___.