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```
2.5mL of2/5M weak monoacidic base (Kb)=(1)(10)^-12 at 25*C.The concentration of H^+ at equivale points is(Kw=1(10^-14)at25*C (1)(3.7)(10^-13)M (2)(3.2)(10^-7)M (3)(3.2)(10^-2)M (4)(3.2)(10^-2)M

```
9 years ago

509 Points
```							BOH + H2O  <====>  B+ + OH-

1000 ml solution have molarity = 2/5
1ml = 2/5 *10-3
2.5ml = (2/5)*(2.5)*10-3 = 10-3M
now , concentration (OH-) = (kC)1/2
k = 10-12 , C = 10-3 so
[OH-] = [3.33*10-8]
[H+] = 10-14/[OH-] = 3.2*10-7

approve if u like my ans
```
9 years ago
610 Points
```							Dear student,The reaction can be written asBOH + H2O →  B+ + OH-1000 ml solution have molarity = 2/51ml = 2/5 *10-32.5ml = (2/5)*(2.5)*10-3 = 10-3MNow , concentration of (OH-) = (kC)1/2k = 10-12 , C = 10-3So,[OH-] = [3.33*10-8][H+] = 10-14/[OH-] = 3.2*10-7Hope it helps.Thanks and regards,Kushagra
```
6 months ago
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