25℃时,0.01mol/L的HClO2溶液中,C(H+)为6.3X10-3mol/L,则25℃时HClO2的电离常数为

问题描述:

25℃时,0.01mol/L的HClO2溶液中,C(H+)为6.3X10-3mol/L,则25℃时HClO2的电离常数为
A1.07X10-2
B1.20X10-2
C1.30X10-2
D1.40X10-2

HClO2的电离方程式为HClO2==(双向箭头)H+ + ClO2-电离常数计算公式 K=[H+][ClO2-]/[HClO2]0.01mol/L的HClO2经过部分电离,剩下3.7x10-3mol/L,[H+]=6.3x10-3mol/L(水的电离太微弱,忽略),[ClO2-]=6.3x10-3mol/L,代入公...