A 0.100 M solution of nitrous acid has a PH ==2.10 . Determine the value of...

A 0.100 M solution of nitrous acid has a PH ==2.10 . Determine the value of the ionization constant for nitrous acid . Determine the present ionization for this acid.

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Expert Solution

PH = 2.1

-log[H^+] = 2.1

[H^+] = 10^-2.1 = 0.00794M

at equilibrium [H^+] = [NO2^-] = 0.00794M

HNO2(aq) -------------------> H^+ (aq) + NO2^- (aq)

Ka = [H^+][NO2^-]/[HNO2]

= 0.00794*0.00794/0.1

= 0.00063 = 6.3*10^-4

percent ionization of acid = final conc of H^+ *1000/initial conc of acid

= 0.00794*100/0.1 = 7.94% >>>>answer

queen_honey_blossom answered 1 year ago

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