Calculate the $pH$ of a buffer solution containing $0.01 \ M$ salt and $0.004 \ M$ weak acid. $(pK_{a} = 4.762)$

When a person breathes rapidly during fear or excitement,the concentration of $CO_2$ in the blood decreases. What happens to the $pH$ of the blood?

The $pH$ of a sodium acetate buffer solution is given by the Henderson-Hasselbalch equation: $pH = pK_a + \log \frac{[Salt]}{[Acid]}$. For acetic acid,if $[Salt] = [Acid] = 0.1 \ M$,then the $pH$ of the solution is: $[K_a = 1.8 \times 10^{-5}]$

Which of the following mixtures in water acts as a basic buffer?

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 ...

The $pH$ of blood does not appreciably change by a small addition of acid or a base because blood