In a buffer solution,the ratio of NH_4Cl to N | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(B) For a basic buffer,the $pOH$ is given by the Henderson-Hasselbalch equation: $pOH = pK_b + \log \frac{[Salt]}{[Base]}$.Initially,the ratio $\frac{

Vedclass · Accepted Answer

Decrease

Vedclass · Answer

(B) For a basic buffer,the $pOH$ is given by the Henderson-Hasselbalch equation: $pOH = pK_b + \log \frac{[Salt]}{[Base]}$.Initially,the ratio $\frac{[Salt]}{[Base]} = \frac{1}{1} = 1$,so $pOH = pK_b + \log(1) = pK_b$.Since $pH + pOH = 14$,the initial $pH = 14 - pK_b$.When the ratio becomes $\frac{2}{1} = 2$,the new $pOH' = pK_b + \log(2)$.Since $\log(2) \approx 0.301$,the $pOH$ increases.As $pH = 14 - pOH$,an increase in $pOH$ results in a decrease in the $pH$ value.

In a buffer solution,the ratio of $NH_4Cl$ to $NH_4OH$ is $1:1$. If this ratio is changed to $2:1$,the $pH$ value of the buffer will ...

Similar Questions

In a mixture of acetic acid and sodium acetate,the ratio of the concentration of the salt to the acid is increased ten times. Then the $pH$ of the solution:

For a $10 \, mL$ solution containing $0.1 \, M \, NH_4Cl$ and $0.01 \, M \, NH_4OH$,which of the following additions will not change the $pH$ of the solution?

In a buffer solution containing equal concentration of $B^{-}$ and $HB,$ the $K_b$ for $B^{-}$ is $10^{-10}.$ The $pH$ of the buffer solution is:

Which of the following solutions can act as a buffer?

$A$ solution contains $0.1 \ mol$ of acetic acid and $0.1 \ mol$ of sodium acetate in $500 \ mL$ of solution. If the $pH$ of the solution is $4.74$,find the ionization constant $(K_a)$ of acetic acid.

Vedclass Test Series

Exam Paper Generator

Online Exam Module