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Which of the following would cause a decrease in the percent ionization of a solution of nitrous acid (HNO2) at equilibrium?
The options are
(a) NaNO2
(b) H2O
(c) Ca(NO3)2
(d) HNO3
(e) NaNO3
i was thinking that answer would be a, d because NaNO2 has common ion NO2^- with HNO2 and HNO3 has common ion H^+ with HNO2 (not sure how H2O would affect)
But given answer is a, c, d
Why should c i.e. Ca(NO3)2 be an answer? This has no ion in common with HNO2.
2 Answers
- pisgahchemistLv 73 years ago
HNO2.....
The study of nitrous acid is not for the newbie. There are a complex set of reactions which surround both gaseous and aqueous nitrous acid. It is not a straightforward weak acid like, for instance, acetic acid (CH3COOH) which partially ionizes to give H+ and CH3COO^- ions.
HNO2 easily decomposes to form the compounds NO, NO2 and water. Little molecular HNO2 exists in aqueous solution. NO2 hydrolyzes to produce HNO3 and HNO2.
2HNO2 <==> NO + NO2 + H2O
2NO2 + H2O <==> HNO2 + HNO3
This gives rise to:
3HNO2 <==> NO + HNO3 + H2O
or
HNO2 + NO2 <==> NO + HNO3
This is why an increase in nitrate ion shifts the equilibrium to the left, toward HNO2.
