List of top Chemistry Questions on Buffer Solutions asked in JEE Main

Given below are two statements:
Statement I: The Henry’s law constant \( K_H \) is constant with respect to variations in solution concentration over the range for which the solution is ideally dilute.
Statement II: \( K_H \) does not differ for the same solute in different solvents.
In the light of the above statements, choose the correct answer from the options given below.
At 298 K, the mole percentage of N$_2$(g) in air is 80%. Water is in equilibrium with air at a pressure of 10 atm. What is the mole fraction of N$_2$(g) in water at 298 K? ($K_H$ for N$_2$ = $6.5 \times 10^7$ mm Hg)

Consider a solution of CO$_2$(g) dissolved in water in a closed container. Which one of the following plots correctly represents variation of $\log$ (partial pressure of CO$_2$ in vapour phase above water) [y-axis] with $\log$ (mole fraction of CO$_2$ in water) [x-axis] at
 $25^\circ$C? 

Only litre buffer solution was prepared by adding 0.10 mol each of $ NH_3 $ and $ NH_4Cl $ in deionised water. The change in pH on addition of 0.05 mol of HCl to the above solution is _____ $ \times 10^{-2} $, (Nearest integer) (Given : $ pK_b $ of $ NH_3 = 4.745 $ and $ \log_{10}3 = 0.477 $)
Given below are two statements:
Statement (I) : A Buffer solution is the mixture of a salt and an acid or a base mixed in any particular quantities.
Statement (II) : Blood is naturally occurring buffer solution whose pH is maintained by $H_2CO_3/HCO_3^-$ concentrations.
In the light of the above statements, choose the correct answer from the options given below.

If the pKa of lactic acid is 5, then the pH of 0.005 M calcium lactate solution at \(25^\circ \text{C}\) is \(\_\_\_\_\_\_ \times 10^{-1}\) (Nearest integer).
Lactic Acid
Strcuture

A litre of buffer solution contains $01$ mole of each of $NH _3$ and $NH _4 CL$ On the addition of $002$ mole of $HCl$ by dissolving gaseous $HCl$, the $pH$ of the solution is found to be ____ $\times 10^{-3}$ (Nearest integer) [Given : $pK _5\left( NH _3\right)=4745$ $ \log 2=0301$ $\log 3=0477$ $T =298 K ]$
S-I: Blood is a buffer solution, whose pH is maintained at 7.4 by an acidic buffer. 
S-II: pH is maintained by HCO3-  and   H2CO3