Answer : The equilibrium concentration of
at
is,
.
Solution : Given,
Equilibrium constant, ![K_c=1.8\times 10^{-5}](https://tex.z-dn.net/?f=K_c%3D1.8%5Ctimes%2010%5E%7B-5%7D)
Initial concentration of
= 0.260 m
Let, the 'x' mol/L of
are formed and at same time 'x' mol/L of
are also formed.
The equilibrium reaction is,
![HC_2H_3O_2(aq)+H_2O(l)\rightleftharpoons H_3O^+(aq)+C_2H_3O_2^-(aq)](https://tex.z-dn.net/?f=HC_2H_3O_2%28aq%29%2BH_2O%28l%29%5Crightleftharpoons%20H_3O%5E%2B%28aq%29%2BC_2H_3O_2%5E-%28aq%29)
Initially 0.260 m 0 0
At equilibrium (0.260 - x) x x
The expression for equilibrium constant for a given reaction is,
![K_c=\frac{[H_3O^+][C_2H_3O_2^-]}{[HC_2H_3O_2]}](https://tex.z-dn.net/?f=K_c%3D%5Cfrac%7B%5BH_3O%5E%2B%5D%5BC_2H_3O_2%5E-%5D%7D%7B%5BHC_2H_3O_2%5D%7D)
Now put all the given values in this expression, we get
![1.8\times 10^{-5}=\frac{(x)(x)}{(0.260-x)}](https://tex.z-dn.net/?f=1.8%5Ctimes%2010%5E%7B-5%7D%3D%5Cfrac%7B%28x%29%28x%29%7D%7B%280.260-x%29%7D)
By rearranging the terms, we get the value of 'x'.
![x=2.154\times 10^{-3}m](https://tex.z-dn.net/?f=x%3D2.154%5Ctimes%2010%5E%7B-3%7Dm)
Therefore, the equilibrium concentration of
at
is,
.