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

Question

BlackTom AI · Accepted Answer

To analyze the question, we start from the given hydroxide concentration: [OH−] = 3.8 × 10−5 M.

First, convert this to pOH: pOH = −log10([OH−]) = −log10(3.8 × 10−5). Estimating log10(3.8) ≈ 0.58, and using −log10(10−5) = 5, we get pOH ≈ 5 − 0.58 ≈ 4.42.

Next, relate pH to pOH via the water dissociation constant at room temperature: pH + pOH = 14. Therefore, pH = 14 − pOH ≈ 14 − 4.42 ≈ 9.58.

A pH above 7 indicates a basic (alkaline) solution, so the solution is basic.

Note on the options: the provided data structure shows an empty list for answer_options, so there are no alternative choices to compare here. The computed result 9.58 aligns with the common assumption of 25 °C for Kw = 1.0 × 10−14, yielding a basic solution with pH ≈ 9.58. This corroborates the statement "9.58; basic" as the correct interpretation of the given [OH−].

CHM-1020-LD01.2025SU Exam 2

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

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CHM-1020-LD01.2025SU Exam 2

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

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?

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−] = _.