Question Bank Directory

Aqueous solution of which of the following compounds is the best conductor of electric current?

What is the molarity of the saturated solution if the solubility product for a salt of type AB is $4 \times 10^{-8}$?

In qualitative analysis, the metals of Group I can be separated from other ions by precipitating them as chloride salts. A solution initially contains $\text{Ag}^+$ and $\text{Pb}^{2+}$ at a concentration of $0.10 \text{ M}$. Aqueous $\text{HCl}$ is added to this solution until the $\text{Cl}^-$ concentration is $0.10 \text{ M}$. What will the concentration of $\text{Ag}^+$ and $\text{Pb}^{2+}$ at equilibrium? ($K_{sp}$ for $\text{AgCl} = 1.8 \times 10^{-10}$, $K_{sp}$ for $\text{PbCl}_2 = 1.7 \times 10^{-5}$)

The correct expression that represents the equivalent conductance at infinite dilution of $Al_2(SO_4)_3$ is: (Given that $\Lambda^{\circ}_{Al^{3+}}$ and $\Lambda^{\circ}_{SO_4^{2-}}$ are the equivalent conductances at infinite dilution of the respective ions)

The value of equilibrium constant of the reaction $HI(g) \rightleftharpoons \frac{1}{2} H_2(g) + \frac{1}{2} I_2(g)$ is $8.0$. The equilibrium constant of the reaction $H_2(g) + I_2(g) \rightleftharpoons 2HI(g)$ will be:

For the reaction $2\text{A} \rightleftharpoons \text{B} + \text{C}$; $K_c = 4 \times 10^{-3}$. At a given time, the composition of the reaction mixture is: $[\text{A}] = [\text{B}] = [\text{C}] = 2 \times 10^{-3}\text{ M}$. In light of the above facts, which of the following is correct?

Given below is a reaction sequence: $\text{CH}_3\text{CH}_2\text{Cl} \xrightarrow{\text{NaCN}} X \xrightarrow{\text{H}_2/\text{Ni}} Y \xrightarrow{\text{Acetic Anhydride}} Z$ The product '$Z$' in the above reaction is:

Match the redox conversions in List-I with the corresponding number of Faradays required in List-II. **List-I (Redox Conversion)** A. $1\text{ mol}$ of $\text{H}_2\text{O}$ to $\text{O}_2$ B. $1\text{ mol}$ of $\text{MnO}_4^-$ to $\text{Mn}^{2+}$ C. $1.5\text{ mol}$ of $\text{Ca}$ from molten $\text{CaCl}_2$ D. $1\text{ mol}$ of $\text{FeO}$ to $\text{Fe}_2\text{O}_3$ **List-II (Number of Faraday required)** I. $3\text{F}$ II. $2\text{F}$ III. $1\text{F}$ IV. $5\text{F}$

The molar solubility of $\text{CaF}_2$ ($K_{sp} = 5.3 \times 10^{-11}$) in $0.1\text{ M}$ solution of NaF will be:

Which of the following statements is correct for a reversible process in a state of equilibrium?

A compound, among the following, that cannot be classified as a protonic acid is:

At $25^\circ\text{C}$, molar conductance of $0.1 \text{ molar}$ aqueous solution of ammonium hydroxide is $9.54 \text{ ohm}^{-1}\text{cm}^2\text{mol}^{-1}$ and at infinite dilution, its molar conductance is $238 \text{ ohm}^{-1}\text{cm}^2 \text{mol}^{-1}$. The degree of ionization of ammonium hydroxide at the same concentration and temperature is:

Given that the equilibrium constant for the reaction $2\text{SO}_2(g) + \text{O}_2(g) \rightleftharpoons 2\text{SO}_3(g)$ has a value of $278$ at a particular temperature, the value of the equilibrium constant for the following reaction at the same temperature will be: $\text{SO}_3(g) \rightleftharpoons \text{SO}_2(g) + \frac{1}{2} \text{O}_2(g)$

The $\text{-OH}$ group of an alcohol or the carboxylic acid can be replaced by $\text{-Cl}$ using:

Based on electrode potentials in the table below: $\text{Cu}^{2+}(aq) + e^- \rightarrow \text{Cu}^+(aq) \quad E^\circ = 0.15 \text{ V}$ $\text{Cu}^+(aq) + e^- \rightarrow \text{Cu}(s) \quad E^\circ = 0.50 \text{ V}$ The value of $E^\circ_{\text{Cu}^{2+}/\text{Cu}}$ will be:

For the reversible reaction: $N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g) + \text{heat}$. The equilibrium shifts in a forward direction:

The correct order of increasing C-X bond reactivity toward nucleophiles among the following is: I. [Missing] II. [Missing] III. $(\text{CH}_3)_3\text{C-X}$ IV. $(\text{CH}_3)_2\text{CH-X}$

Consider the nitration of benzene using mixed conc. $H_2SO_4$ and $HNO_3$. If a large amount of $KHSO_4$ is added to the mixture, the rate of nitration will be:

The pH of the solution containing $50\text{ mL}$ each of $0.10\text{ M}$ sodium acetate and $0.01\text{ M}$ acetic acid is: [Given $\text{p}K_a$ of $\text{CH}_3\text{COOH} = 4.57$]

For the cell reaction $2Fe^{3+} (aq) + 2I^- (aq) \rightarrow 2Fe^{2+} (aq) + I_2 (aq)$, $E^{\ominus}_{cell} = 0.24 \text{ V}$ at 298 K. The standard Gibbs energy ($\Delta_r G^{\ominus}$) of the cell reaction is : [Given that Faraday constant $F = 96500 \text{ C mol}^{-1}$]