3.00×10−3 mol of HBr are dissolved in water to make 14.0 L of solution. What is the concentration of hydroxide ions, [OH−], in this solution?
回答 (2)
2016-07-27 5:59 pm
[HBr] = (3.00 × 10⁻³ mol) / (14.0 L) = 2.14 × 10⁻⁴ M
HBr is strong acid which completely dissociates in water to give H⁺ ions.
Hence, [H⁺] = 2.14 × 10⁻⁴ M
[H⁺] [OH⁻] = Kw
[OH⁻] = Kw / [H⁺] = (1.00 × 10⁻¹⁴) / (2.14 × 10⁻⁴) M = 4.67 × 10⁻¹¹ M
HBr is strong acid which completely dissociates in water to give H⁺ ions.
Hence, [H⁺] = 2.14 × 10⁻⁴ M
[H⁺] [OH⁻] = Kw
[OH⁻] = Kw / [H⁺] = (1.00 × 10⁻¹⁴) / (2.14 × 10⁻⁴) M = 4.67 × 10⁻¹¹ M
2016-09-19 1:47 am
This sounds weird
收錄日期: 2021-04-20 16:26:29
原文連結 [永久失效]:
https://hk.answers.yahoo.com/question/index?qid=20160727094543AAGeLef