Calculate the [H3O+] and [OH?] for a solution with the following pH values:
1. pH=3.3
2. pH=5.64
3. pH=8.2
4. pH=10.9
5. pH=9.75
6.
1. pH=3.3
[H3O+]= 10^-pH = 10^-3.3 = 5.01*10^-4
[OH-]= 1*10^-14/[H3O+]= 1*10^-14/(5.01*10^-4) = 1.996*10^-11 = 2.0*10^-11
2. pH=5.64
[H3O+]= 10^-pH = 10^-5.64 = 2.29*10^-6
[OH-]= 1*10^-14/[H3O+]= 1*10^-14/(2.29*10^-6) = 4.4*10^-9
3. pH=8.2
[H3O+]= 10^-pH = 10^-8.2 = 6.31*10^-9
[OH-]= 1*10^-14/[H3O+]= 1*10^-14/(6.31*10^-9) = 1.58*10^-6
4. pH=10.9
[H3O+]= 10^-pH = 10^-10.9 = 1.26*10^-11
[OH-]= 1*10^-14/[H3O+]= 1*10^-14/(1.26*10^-11) = 7.94*10^-4
5. pH=9.75
[H3O+]= 10^-pH = 10^-9.75 = 1.78*10^-10
[OH-]= 1*10^-14/[H3O+]= 1*10^-14/(1.78*10^-10) = 5.62*10^-5
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