Answer : When [tex]KNO_2[/tex] dissolved into the solution then the equilibrium will shift in the left direction.
Explanation :
Le-Chatelier's principle : This principle states that if any change in the variables of the reaction, the equilibrium will shift in the direction to minimize the effect.
The dissociation reaction of [tex]HNO_2[/tex] is:
[tex]HNO_2\rightleftharpoons H^++NO_2^-[/tex]
As we are adding [tex]KNO_2[/tex] that means increase the concentration of [tex]NO_2^-[/tex] then the equilibrium will shift in the left direction.
If the concentration of [tex]NO_2^-[/tex] is increased on product side then the equilibrium will shift in the direction where decrease of concentration of
Hence, when [tex]KNO_2[/tex] dissolved into the solution then the equilibrium will shift in the left direction.
Explanation:
The reaction can be written as
HNO_2 ⇔H+ + NO2-
Now, adding KNO2 will further increase the conc. of NO2-.
Now, As per Le Chatelier's principle the equilibrium will shift reactant side as its conc. is decreased.
This reduces the extent of ionization of HNO2. Hence, Concentration H+ ion decreases.
And also, pH= -log[H+]
hence, pH increases.
