Calculate pH of 0.1 M acetic acid having K_(a)=1.8xx10^(-5)
The pH of 0.05 M acetic acid is (K_(a) = 2 xx 10^(-5))
What [NH_4^(+) ] in a solution that contains 0.02M NH_3 (K_b =1.8 xx 10^(-5) ) and 0.01 M KOH ?
The additions of sodium acetate to 0.1 M acetic acid will cause :
P^(H) of a solution of the mixture of 0.1 HCl and 0.1N CH_3 COOH is ( K_a =2xx10 ^(-5))
A one litre solution contains 0.08 mole of acetic acid ( K_(a) = 1.75 xx 10^(-5) ) . To this solution , 0.02 mole of NaOH is added . Then the pH of resulting solution is[log 1.75 =0.243 ]
The concentration of acetic acid required to get 3.5 xx 10^(-4) mole/lit of H^(+) ion is [K_(a) = 1.8 xx 10^(-5) ]
NARENDRA AWASTHI-IONIC EEQUILIBRIUM-Assertin-Reason Type Questions