The concentration of hydroxide ion in a water sample is found to be 2.5 × 10^-6M. Identify the nature of the solution.

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.

Calculate the pH of 0.04 M HNO₃ Solution.

Define ionic product of water. Give its value at room temperature.

Explain common ion effect with an example.

Calculate the pH of 1.5\(\times\)10^-3 M solution of Ba(OH)₂

50ml of 0.05M HNO₃ is added to 50ml of 0.025M KOH. Calculate the pH of the resultant solution.

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 \(K_{a}=K_{b}=1.8\times10^{-5}\)

Derive an expression for the hydrolysis constant and degree of hydrolysis of salt of strong acid and weak base.

Solubility product of Ag₂CrO₄ is \(1\times10^{-12}\). What is the solubility of Ag₂CrO₄ in 0.01M AgNO₃ solution?

Write the expression for the solubility product of Ca₃(PO₄)₂

A saturated solution, prepared by dissolving CaF₂(s) in water, has \([Ca^{2+}]=3.3\times10^{-4}M\). What is the K_sp of CaF₂?

A particular saturated solution of silver chromate Ag₂CrO₄ has \([Ag^{+}]=5\times10^{-5}\) and \([CrO_{4}]^{2-}=4.4\times10^{-4}M\). What is the value of K_sp for Ag₂ CrO₄?

Write the expression for the solubility product of Hg₂Cl₂ .

K_sp of Ag₂CrO₄ is \(1.1\times10^{-12}\). What is solubility of Ag₂CrO₄ in 0.1M K₂CrO₄.

Will a precipitate be formed when 0.150 L of 0.1M Pb(NO₃)₂ and 0.100L of 0.2 M NaCl are mixed? \(K_{sp}\ (PbCl_{2})=1.2\times10^{-5}\).

K_sp of Al(OH)₃ is 1\(\times\)10^-15M. At what pH does 1.0×10^-3M Al³⁺ precipitate on the addition of buffer of NH₄Cl and NH₄OH solution?

Calculate pH of 10^-7 M HCl

 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 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).

Establish a relationship between the solubility product and molar solubility for the following
a) BaSO₄ 
b) Ag₂(CrO₄)

Indicate find out whether lead chloride gets precipitated or not when 1 mL of 0.1M lead nitrate and 0.5 mL of 0.2 M NaCl solution are mixed? K_sp of PbCl₂ is 1.2 x 10^-5 .