The equilibrium constant for the reaction
HNO₂(aq)+ H₂O(l) $\rightarrow$ NO₂-(aq)+ H₃O⁺(aq)
is 4.3 * 10^-⁴ at 25^$\omicron$C.Will nitrous acid spontaneously dissociate when
[HNO₂(aq)] = 1.0 M and [NO₂-(aq)] = [H₃O⁺(aq)] = 1.0 * 10^-⁵ M?
Show your calculations.

Question

The equilibrium constant for the reaction
HNO₂(aq)+ H₂O(l)

\rightarrow

NO₂-(aq)+ H₃O⁺(aq)
is 4.3 * 10^-⁴ at 25^$\omicron$C.Will nitrous acid spontaneously dissociate when
[HNO₂(aq)] = 1.0 M and [NO₂-(aq)] = [H₃O⁺(aq)] = 1.0 * 10^-⁵ M?
Show your calculations.

Quizplus · Accepted Answer

The Answer of The equilibrium constant for the reaction HNO₂(aq)+ H₂O(l) $\rightarrow$ NO₂ - (aq)+ H₃O⁺(aq) is 4.3 * 10 ^- ⁴ at 25^$\omicron$C.Will nitrous acid spontaneously dissociate when [HNO₂(aq)] = 1.0 M and [NO₂ - (aq)] = [H₃O⁺(aq)] = 1.0 * 10 ^- ⁵ M? Show your calculations.

The Equilibrium Constant for the Reaction HNO2(aq)+ H2O(l) →\rightarrow→ NO2-(aq)+ H3O+(aq) Is 4

The Equilibrium Constant for the Reaction
HNO₂(aq)+ H₂O(l) $\rightarrow$ NO₂-(aq)+ H₃O⁺(aq)
Is 4