Assertion : It is difficult to distinguish the strengths of the strong acids such as

                  $\mathrm{HCl}, {\mathrm{H}}_2{\mathrm{SO}}_4, {\mathrm{HNO}}_3, \mathrm{HBr}, \mathrm{Hl} \mathrm{or} {\mathrm{HClO}}_4$ in dilute aqueous solutions.

Reason : In dilute aqueous solution all strong acids donate a proton to water and are essentially.

               100% ionised to produce a solution containing ${\mathrm{H}}_3{\mathrm{O}}^{+}$ ions plus the anions of strong acid.

1. If both the assertion and the reason are true and the reason is a correct explanation of the assertion
2. If both the assertion and reason are true but the reason is not a correct explanation of the assertion
3. If the assertion is true but the reason is false
4. If both the assertion and reason are false

Assertion : 0.20 M solution of $\mathrm{NaCN}$is more basic than 0.20 M solution of $\mathrm{NaF}$.

Reason : 0.20 M solution of $\mathrm{NaCN}$ is more basic than 0.20 M solution of ${\mathrm{CH}}_3\mathrm{COONa}.$

Assertion: A substance that can either act as an acid or a base is called ampholyte.

Reason: Bisulphide ion $\left({\mathrm{HS}}^{-}\right)$ and bicarbonate ion $\left({{\mathrm{HCO}}_3}^{-}\right)$ are ampholytes.

Which of the following statement is true if the reaction quotient, Q is equal to 1 ?

1. $∆G=0$

2. $∆G^{\circ }=0$

3. $∆S^{\circ }=0$

4. $∆G=∆G^{\circ }$

The concentration of Ag⁺ ions in a saturated solution of Ag₂C₂O₄ is 2.2 × 10^–4 mol L^–1.
The solubility product of Ag₂C₂O₄ is:

The solubility of AgCl (s) with solubility product 1.6×10^–10 in 0.1 M NaCl solution would be?

The following solutions were prepared by mixing different volumes of NaOH and HCl of different concentrations :

A)  $60$ $mL$ $\frac{M}{10}HCI$ $$ $+$ $40$ $mL$ $\frac{M}{10}NaOH$
B)   $55$ $mL$ $\frac{M}{10}HCI$ $$ $+$ $45$ $mL$ $\frac{M}{10}NaOH$
C)  $75$ $mL$ $\frac{M}{5}HCI$ $$ $+$ $25$ $mL$ $\frac{M}{5}NaOH$
D)  $100$ $mL$ $\frac{M}{10}HCI$ $$ $+$ $100$ $mL$ $\frac{M}{10}NaOH$

pH of which one of them will be equal to 1?

1. B
2. A
3. D
4. C

The solubility of BaSO₄ in water is $2.42$ $\times$ ${10}^{-3}$ g/ litre at 298 K. The value of the solubility product will be: (Molar mass of BaSO₄ = 233 gmol^–1)

Mark the conditions that favour the maximum product formation in the given reaction.
 $A_2$ $\left(g\right)$ $$ $+$ $B_2$ $\left(g\right)$ $$ $\leftrightharpoons$ $X_2$ $(g),$ ${∆}_{r}H$ $=$ $-X$ $k$ $J$ $$ 

1. Low temperature and High pressure
2. Low temperature and Low pressure
3. High temperature and High pressure
4. High temperature and Low pressure

Among the following, the correct order of acidity is:

1. HClO < HClO₂ < HClO₃ < HClO₄
2. HClO₂ < HClO < HClO₃ < HClO₄
3. HClO₄ < HClO₂ < HClO  < HClO₃
4. HClO₃ < HClO₄ < HClO₂ < HClO