Home
Class 12
CHEMISTRY
Calculate the pH and degree of hydrolsi...

Calculate the pH and degree of hydrolsis of `0.01` M solution of KCN , `K_(s)` for HCN is ` 6.2 xx 10^(-19)` .

Text Solution

AI Generated Solution

To calculate the pH and degree of hydrolysis of a 0.01 M solution of KCN, we will follow these steps: ### Step 1: Determine the \( K_a \) of HCN Given that \( K_s \) for HCN is \( 6.2 \times 10^{-19} \), we can find the \( K_a \) using the relationship: \[ K_w = K_a \times K_b \] Where \( K_w \) (the ion product of water) is \( 1.0 \times 10^{-14} \) at 25°C. ...
Promotional Banner

Similar Questions

Explore conceptually related problems

Calculate the degree of hydrolysis and pH of 0.2M solution of NH_(4)C1 Given K_(b) for NH_(4)OH is 1.8 xx 10^(-5) .

a. Calculate the percentage hydrolysis of 0.003M aqueous solution of NaOH. K_(a) for HOCN = 3.3 xx 10^(-4) . b. What is the pH and [overset(Theta)OH] of 0.02M aqueous solution of sodium butyrate. (K_(a) = 2.0 xx 10^(-5)) .

Calculate the degree of hydrolysis of 0.1 M solution of sodium acetate at 298 K : K_(a) = 1.8 xx 10^(-5) .

Calculate the degree of hydrolysis of the 0.01 M solution of salt (KF)(Ka(HF)=6.6xx10^(-4)) :-

Calculate the degree of hydrolysis of 0.1 M solution of acetate at 298 k. Given : K_a=1.8xx10^(-5)

Calculate the hydrolysis constant and degree of hydrolysis of NH_(4) Cl" in " 0.1 M solution . K_(b) = 1.8 xx 10^(-5) . Calculate the concentration of H^(+) ions in the solution .

Calculate the pH of a 0.01 M of HCl solution.

Calculate the pH of a 0.01 M of NaOH solution.

Calculate the hydrolysis constant. Degree of hydrolysis and pH of 0.5 M solution of NH_4Cl. ( Given : K_a = 1.78 xx 10 ^(-5) ,K_b= 1.8 xx 10 ^(-5) and K_w = 1.8 xx 10 ^(-14) )

Calculate the pH of 0.01 M solution of NH_(4)CN. The dissociation constants K_(a) for HCN=6.2xx10^(-10)and K_(b) for NH_(3)=1.6xx10^(-5).