Consider the following Assertion and Reason:

Assertion: It is difficult to distinguish the strengths of strong acids such as HCl, H₂SO₄, HNO₃, HBr, HI, and HClO₄ in dilute aqueous solutions.

Reason: In dilute aqueous solutions, all strong acids donate protons to water and are almost 100% ionised, producing H₃O⁺ ions and the corresponding anions of the acids.
 

Options:

1. Both Assertion and Reason are true, and Reason is the correct explanation of Assertion.
2. Both Assertion and Reason are true, but Reason is not the correct explanation of Assertion.
3. Assertion is true, but Reason is false.
4. Assertion is false, but Reason is true.

Assertion : 0.20 M solution of $\mathrm{NaCN}<mspace\; width="1em"></mspace>$is more basic than 0.20 M solution of $\mathrm{NaF}$.

Reason : 0.20 M solution of $\mathrm{NaCN}<mspace\; width="1em"></mspace>$ 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)  $60$ $mL$ $\frac{M}{10}HCl$ $$ $+$ $40$ $mL$ $\frac{M}{10}NaOH$

B)   $55$ $mL$ $\frac{M}{10}HCl$ $$ $+$ $45$ $mL$ $\frac{M}{10}NaOH$

C)  $75$ $mL$ $\frac{M}{5}HCl$ $$ $+$ $25$ $mL$ $\frac{M}{5}NaOH$

D)  $100$ $mL$ $\frac{M}{10}HCl$ $$ $+$ $100$ $mL$ $\frac{M}{10}NaOH$

Which of them will have a pH 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