Which one of the following pair shows Buffer's solution?

• NaCl + NaOH

• CH₃COONa + CH₃COOH

• CH₃COOH + CH₃COONH₄

• H₂SO₄ + CuSO₄

Which of the following chloride is water insoluble?

• HCl

• AgCl

• Both 'a' and 'b'

• None of these

0.005 M acid solution has 5 pH. The percentage ionisation of acid is :

• 0.8%

• 0.6%

• 0.4%

• 0.2%

CH₃COOH is weaker acid than H₂SO₄.It is due to:

• more ionization

• less ionization

• covalent bond

• electrovalent bond

705.

In the reaction $3\mathrm{A} + 2\mathrm{B} \to 2\mathrm{C}$, the equilibrium constant K_c is given by

• $\frac{\left[3\mathrm{A}\right] \mathrm{x}\left[2\mathrm{B}\right]}{\left[\mathrm{C}\right]}$

• $\frac{[\mathrm{A}{]}^3\times [\mathrm{B}]}{\left[\mathrm{C}\right]}$

• $\frac{[\mathrm{C}{]}^2}{[\mathrm{A}{]}^3\times [\mathrm{B}{]}^2}$

• $\frac{\left[\mathrm{C}\right]}{\left[3\mathrm{A}\right]\left[2\mathrm{B}\right]}$

The solubility of Sb₂S₃ in water is 1.0 × 10^-5 mol/L at 298K. What will be its solubility product?

• 108 × 10^-25

• 1.0 × 10^-25

• 144 × 10^-25

• 126 × 10^-24

What will be the pH value of 0.05 M Ba(OH)₂ solution?

• 12

• 13

• 1

• 12.96

N₂ and H₂ in 1 : 3 molar ratio are heated in a closed container having a catalyst. When the following equilibrium ${\mathrm{N}}_2\left(\mathrm{g}\right)+3{\mathrm{H}}_2\left(\mathrm{g}\right) \rightleftharpoons 2{\mathrm{NH}}_3\left(\mathrm{g}\right)$ is attained, the total pressure is 10 atm and mole fraction of NH₃ is 0.60. The equilibrium constant K_P for dissociation of NH₃ is

• 1.333 atm^-2

• 0.75 atm^-2

• 0.75 atm²

• 1.333 atm²

According to Le-Chatelier principle, adding heat a solid and liquid in equilibrium will cause the

• amount of solid to decrease

• amount of liquid to decrease

• temperature to rise

• temperature to fall

Solubility of AgCl at 20$°$C is 1.435 x 10^-3 g/L. The solubility product of AgCl is

• 1 x 10^-5

• 1 x 10^-10

• 1.435 x 10^-5

• 108 x10^-3