Since all the aqueous solution contain both OH- and H+
May I ask if there is 0.1M of HCL ( contain 0.1M H+) , does it means that there are 0.9M of OH-?
If not , how many ?
A question on pH of solutions!?
2009-12-24 9:18 am
回答 (2)
2009-12-24 9:35 am
✔ 最佳答案
let us consider that 1L of HCl is takenthen moles of H+ = 0.1
=> [H+] = 0.1/1 = 0.1
So, pH = -log[H+] = -log(10^-1) = 1
now we know that at 25 deg C, pH + pOH = 14
=> pOH = 14 -1 = 13
=> -log[OH-] = 13
=> [OH-] = 10^-13 M
Alternative method,
[H+][OH-] = Kw = 10^-14 (at 25 deg C)
=> [OH-] = 10^-14/[H+] = 10^(-14)/0.1 = 10^-13 M
2009-12-24 9:32 am
No . Not at all
you have concentratoins of H+ are [H+] concentration and concentration of OH- are [OH-]
[H+]*[OH-]= 10^-14
so if [OH+] = 10^-14/^[H+}
in your case [H+]=10^-1
AND so[OH-]= 10^-14/10-1= 10^-13
you have concentratoins of H+ are [H+] concentration and concentration of OH- are [OH-]
[H+]*[OH-]= 10^-14
so if [OH+] = 10^-14/^[H+}
in your case [H+]=10^-1
AND so[OH-]= 10^-14/10-1= 10^-13
收錄日期: 2021-04-25 13:54:51
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