Chemistry, 01.07.2019 00:00 kianofou853
Kw, the equilibrium constant for the ionization of water by the equation below, is 1.0 x 10-14. what does that mean when we are considering pure water?
Answers: 1
![[H^+]\&[OH^-]](/tpl/images/0036/7175/bc884.png)
are equal in pure water.
![K_{eq}=\frac{[H^+][OH^-]}{[H_2O]}](/tpl/images/0036/7175/59636.png)
![K_w=K_{eq}[H_2O]=[H^+][OH^-]=1.0\times 10^{-14}](/tpl/images/0036/7175/f0cd4.png)
![pH=7=-\log[H^+]](/tpl/images/0036/7175/ae186.png)
![[H^+]=1\times 10^{-7}mol/L](/tpl/images/0036/7175/f6d22.png)
of pure water is given![K_w=[H^+][OH^-]=1\times 10^{-7}\times[OH^-]= 1\times 10^{-14}](/tpl/images/0036/7175/db7b7.png)
![[OH^-]=1\times 10^{-7}mol/L](/tpl/images/0036/7175/b6b71.png)
![[H^+]\&[OH^-]](/tpl/images/0036/7175/72025.png)
are equal in pure water
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Kw, the equilibrium constant for the ionization of water by the equation below, is 1.0 x 10-14. what...
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