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In: Chemistry

The pH of an aqueous solution of 7.96×10-2 M ammonium nitrate, NH4NO3 (aq), is . This...

The pH of an aqueous solution of 7.96×10^-2 M ammonium nitrate, NH₄NO₃ (aq), is .

This solution is

Expert Solution

NH4NO3(aq) --------------> NH4^+ (aq) + NO3^- (aq)

7.96*10^-2M 7.96*10^-2 M(0.0796M)

NH4^+ (aq) + H2O -------------> NH3(aq) + H3O^+ (aq)

I 0.0796 0 0

C -x +x +x

E 0.0796-x +x +x

Kb = 1.8*10^-5

ka = Kw/Kb

= 1*10^-14/1.8*10^-5 = 5.6*10^-10

Ka = [NH3][H3O^+]/[NH4^+]

5.6*10^-10 = x*x/0.0796-x

5.6*10^-10*(0.0796-x) = x^2

x = 6.67*10^-6

[H3O+] = x = 6.67*10^-6M

PH = -log[H3O^+]

= -log6.67*10^-6

= 5.1758 >>>>answer

queen_honey_blossom answered 2 years ago

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