3.00×10−3 mol of HBr are dissolved in water to make 16.0 L of solution.What is the concentration of hydroxide ions, [OH−] in this solution?
回答 (2)
2017-10-31 1:35 am
Concentration of HBr = (3.00 × 10⁻³ mol) / (16 L) = 1.875 × 10⁻⁴ M
HBr is a strong acid which completely dissociates to give H⁺ ions.
Hence, [H⁺] = 1.875 × 10⁻⁴ M
[OH⁻] = Kw / [H⁺] = (1.00 × 10⁻¹⁴) / (1.875 × 10⁻⁴) M = 5.33 × 10⁻¹¹ M
HBr is a strong acid which completely dissociates to give H⁺ ions.
Hence, [H⁺] = 1.875 × 10⁻⁴ M
[OH⁻] = Kw / [H⁺] = (1.00 × 10⁻¹⁴) / (1.875 × 10⁻⁴) M = 5.33 × 10⁻¹¹ M
2017-10-31 2:42 am
Just for a variety of methods:
pH = - log ((3.00 × 10^−3 mol) / (16.0 L)) = 3.727
pOH = 14 - pH = 10.273
10^-10.273 = 5.33 × 10^-11 M OH-
pH = - log ((3.00 × 10^−3 mol) / (16.0 L)) = 3.727
pOH = 14 - pH = 10.273
10^-10.273 = 5.33 × 10^-11 M OH-
收錄日期: 2021-04-18 17:53:31
原文連結 [永久失效]:
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