What substance could be added to one liter of water to serve as a buffer?

1. One mole of ${\mathrm{CH}}_3{\mathrm{CO}}_2\mathrm{H}$ and 0.5 moles of NaOH

2. One mole of NH₄Cl and one mole of HCl

3. One mole of NH₄OH and one mole of NaOH

4. One mole of ${\mathrm{CH}}_3{\mathrm{CO}}_2\mathrm{H}$ and one mole of HCl

Acoording to Bronsted-Lowry concept, the correct order of relative strength of bases follows the order

1. CH₃COO^- > Cl^- > OH^-

2. CH₃COO^- > OH^- > Cl^-

3. OH^- > CH₃COO^- > Cl^-

4. OH^- > Cl^-> CH₃COO^-

pOH of H₂O is 7.0 at 298K. If water is heated at 350K, which of the following statement should be true ?

(1) pOH will decrease

(2) pOH will increase

(3) pOH will remain 7.0

(4) Concentration of H⁺ ions will increase but that of OH^- will decrease.

In which case following equilibrium can't be established:

CaCO₃(s) $\rightleftharpoons$CaO(s) + CO₂(g)

1. Some CaO & pressure of CO₂ was greater than Kp

2. Pure CaCO₃

3. Some CaCO₃ & pressure of CO₂ gas greater than K_p

4. Some CaCO₃ & pressure of CO₂ gas less than K_p.

An aqueous solution of NaHSO₃ is-

1. Acidic                 
2. Slightly alkaline
3. Alkaline             
4. Slightly Acidic

The solubility product constant (K_sp) of salts of types MX, MX₂ and M₃X at temperature T are 4.0 X 10^-8, 3.2 X 10^-14 and 2.7 X 10^-15 respectively. Solubilities(mol dm^-3) of the salts at temperature T are the order:

1. MX > MX₂ > M₃X

2. M₃X > MX₂ > MX

3. MX₂ > M₃X > MX

4. M₃X >MX > MX₂

Ostwald dilution law for weak electrolyte HA can be given as

$\left(1\right) {\mathrm{K}}_{\mathrm{a}}=\frac{{\mathrm{C\alpha }}^2}{(1-\mathrm{\alpha })}$
$\left(2\right) \mathrm{Ka} = {\mathrm{C\alpha }}^2 \mathrm{if} \mathrm{\alpha }\to 0$
$\left(3\right) {\mathrm{K}}_{\mathrm{a}} = \frac{{\mathrm{C\lambda }}^2}{{\mathrm{\lambda }}^2({\mathrm{\lambda }}^2-\mathrm{\lambda })}$
$\left(4\right) \mathrm{All} \mathrm{of} \mathrm{the} \mathrm{above}$

In the reaction, N₂O₄ $\rightleftharpoons$ 2NO₂, $\mathrm{\alpha }$ is that part of N₂O₄ which dissociates. The number of moles at equilibrium will be:

1. ${\left(1-\mathrm{\alpha }\right)}^2$

2. $3\mathrm{\alpha }$

3. $\mathrm{\alpha }$

4. $1+\mathrm{\alpha }$

In which solution, AgCl has minimum solubility ?

1. 0.05 M AgNO₃

2. 0.01 M NaCl

3. Pure Water

4. 0.01 M NH₄OH

50 ml of HCl (pH=1) is mixed with another 100 ml of HCl (pH=2) then pH of resulting solution will be approximately

1. 1.2

2. 1.4

3. 1.6

4. 1.8