Concentration of the Ag⁺ ions in a saturated solution of Ag₂C₂O₄ is 2.24 ×10^-4mol L^-1 solubility product of Ag₂C₂O₄ is_______.

Which of the following fluro compounds is most likely to behave as a Lewis base?

The percentage of pyridine (C₅H₅N) that forms pyridinium ion (C₅H₅NH) in a 0.10M aqueous pyridine solution _______.(K_b for C₅H₅N = 1.7×10^-9) is 

MY and NY₃, are insoluble salts and have the same K_sp values of 6.2 × 10^-13 at room temperature. Which statement would be true with regard to MY and NY₃?

Pick the strongest conjugate base among the following

A lab assistant prepared a solution by adding a calculated quantity of HCl gas 25⁰C to get a solution with [H₃O⁺] = 4\(\times\)10^-5M. Is the solution neutral (or) acidic (or) basic.

Define solubility product.

Calculate the pH of 0.001M HCl solution

The K_W of a neutral solution is 10^-12 at a particular temperature. What are its pH and pOH values?

How is common ion effect related to the solubility of the electrolyte?

The K_a value for HCN is 10^-9. What is the pH of 0.4M HCN solution?

Calculate the extent of hydrolysis and the pH of 0.1 M ammonium acetate Given that \(K_{a}=K_{b}=1.8\times10^{-5}\)

 Find the pH of a buffer solution containing 0.20 mole per litre sodium acetate and 0.18 mole per litre acetic acid. K_a for acetic acid is \(1.8\times10^{-5}\).

What do you mean by auto ionisation of water?

For an aqueous solution of NH₄CI, prove that [H⁺] = \(\sqrt { { K }_{ n }.C } \)

What is the pH of an aqueous solution obtained by mixing 6 gram of acetic acid and 8.2 gram of sodium acetate and making the volume equal to 500 ml. (Given: K_a for acetic acid is  \(1.8\times10^{-5}\))

Calculate i) degree of hydrolysis, ii) the constant hydrolysis  and iii) pH of 0.1M CH₃COONa solution (pK_a for CH₃COOH is 4.74).

Calculate the pH of 0.1 M acetic acid if its ionisation constant Ka = 1.8 x 10^-5.

pH of a solution is 5.5 at 25°C. Calculate its [OH^-].