Ionic Equilibrium

The molar conductivity of a solution of a weak acid HX (0.01 M) is 10 times smaller than the molar conductivity of a solution of a weak acid HY (0.10 M). If $\lambda^0_{\ce{X-}}\approx\lambda^0_{\ce{Y-}}$, the difference in their $\mathrm pK_a$ values, $\mathrm pK_a(\ce{HX})-\mathrm pK_a(\ce{HY})$, is (consider degree of ionization of both acids to be $\ll1$)

The pH of the solution after Expt. 2 is

The correct statement(s) for orthoboric acid is/are

Assuming that the degree of hydrolysis is small, the pH of 0.1 M solution of sodium acetate ($K_a=1.0\times10^{-5}$) will be :

In some solutions, the concentration of $\ce{H3O+}$ remains constant even when small amounts of strong acid or strong base are added to them. These solutions are known as :

The conjugate base of hydrazoic acid is :

Zirconium phosphate $\ce{[Zr3(PO4)4]}$ dissociates into three zirconium cations of charge +4 and four phosphate anions of charge −3. If molar solubility of zirconium phosphate is denoted by S and its solubility product by $K_{sp}$ then which of the following relationship between S and $K_{sp}$ is correct ?

The initial rate of hydrolysis of methyl acetate (1 M) by a weak acid (HA, 1 M) is 1/100$^\text{th}$ of that of a strong acid (HX, 1 M), at 25 °C. The $K_a$ of HA is

The $K_{sp}$ of $\ce{Ag2CrO4}$ is $1.1\times10^{-12}$ at 298 K. The solubility (in mol/L) of $\ce{Ag2CrO4}$ in a 0.1 M $\ce{AgNO3}$ solution is

An aqueous solution of X is added slowly to an aqueous solution of Y as shown in List I. The variation in conductivity of these reactions is given in List II. Match List I with List II and select the correct answer using the code given below the lists:

The solubility product ($K_{sp}$; mol³ dm⁻⁹) of $\ce{MX2}$ at 298 K based on the information available for the given concentration cell is (take $2.303\times R\times298/F=0.059$ V)

In 1 L saturated solution of AgCl [$K_{sp}$(AgCl) $=1.6\times10^{-10}$], 0.1 mol of CuCl [$K_{sp}$(CuCl) $=1.0\times10^{-6}$] is added. The resultant concentration of $\ce{Ag+}$ in the solution is $1.6\times10^{-x}$. The value of "$x$" is

Aqueous solutions of $\ce{HNO3}$, KOH, $\ce{CH3COOH}$, and $\ce{CH3COONa}$ of identical concentrations are provided. The pair(s) of solutions which form a buffer upon mixing is(are)

Amongst the following, the total number of compounds whose aqueous solution turns red litmus paper blue is

KCN, $\ce{K2SO4}$, $\ce{(NH4)2C2O4}$, NaCl, $\ce{Zn(NO3)2}$, $\ce{FeCl3}$, $\ce{K2CO3}$, $\ce{NH4NO3}$, LiCN

The total number of diprotic acids among the following is

$\ce{H3PO4}$, $\ce{H2SO4}$, $\ce{H3PO3}$, $\ce{H2CO3}$, $\ce{H2S2O7}$, $\ce{H3BO3}$, $\ce{H3PO2}$, $\ce{H2CrO4}$, $\ce{H2SO3}$

The dissociation constant of a substituted benzoic acid at 25°C is $1.0\times10^{-4}$. The pH of a 0.01 M solution of its sodium salt is

2.5 mL of $\frac25$ M weak monoacidic base ($K_b=1\times10^{-12}$ at 25 °C) is titrated with $\frac2{15}$ M HCl in water at 25 °C. The concentration of H⁺ at equivalence point is ($K_w=1\times10^{-14}$ at 25 °C)

Solubility product constants ($K_{sp}$) of salts of types MX, MX₂ and M₃X at temperature 'T' are $4.0\times10^{-8}$, $3.2\times10^{-14}$ and $2.7\times10^{-15}$, respectively. Solubilities (mol dm⁻³) of the salts at temperature 'T' are in the order

STATEMENT-1: In water, orthoboric acid behaves as a weak monobasic acid.

because

STATEMENT-2: In water, orthoboric acid acts as a proton donor.