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

(a)

2.42 × 10^-8mol³L^-3

(b)

2.66 × 10^-12mol³L^-3

(c)

4.5 × 10^-11mol³L^-3

(d)

5.619 × 10^-12mol³L^-3

pH of a saturated solution of Ca(OH)₂ is 9. The Solubility product (K_sp) of Ca(OH)₂ _______.

(a)

0.5 × 10^-15

(b)

0.25 × 10^-10

(c)

0.125 × 10^-15

(d)

0.5 × 10^-10

Which will make basic buffer?

(a)

50 mL of 0.1M NaOH+25mL of 0.1M CH₃COOH

(b)

100 mL of 0.1M CH₃COOH+100 mL of 0.1M NH₄OH

(c)

100 mL of 0.1M HCl+200 mL of 0.1M NH₄OH

(d)

100 mL of 0.1M HCl+100 mL of 0.1M NaOH

Which of these is not likely to act as Lewis base?

(a)

BF₃

(b)

PF₃

(c)

CO

(d)

F^–

The aqueous solutions of sodium formate, anilinium chloride and potassium cyanide are respectively _______.

(a)

acidic, acidic, basic

(b)

basic, acidic, basic

(c)

basic, neutral, basic

(d)

none of these

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 

(a)

0.006%

(b)

0.013%

(c)

0.77%

(d)

1.6%

Equal volumes of three acid solutions of pH 1,2 and 3 are mixed in a vessel. What will be the H⁺ ion concentration in the mixture?

(a)

3.7 × 10^-2

(b)

10^-6

(c)

0.111

(d)

none of these

Using Gibb’s free energy change, ∆G^o=57.34 kJ mol^-1, for the reaction, X₂Y_(s)⇌2X⁺+Y^2- (aq), calculate the solubility product of X₂Y in water at 300 K_______. (R = 8.3 J K^-1Mol^-1)

(a)

10^-10

(b)

10^-12

(c)

10^-14

(d)

can not be calculated from the given dat

What is the pH of the resulting solution when equal volumes of 0.1M NaOH and 0.01M HCl are mixed?

(a)

2.0

(b)

3

(c)

7.0

(d)

12.65

The pH of 10^-5M KOH solution will be _______.

(a)

9

(b)

5

(c)

19

(d)

none of these

The pH of an aqueous solution is Zero. The solution is _______.

(a)

slightly acidic

(b)

strongly acidic

(c)

neutral

(d)

basic

Dissociation constant of NH₄OH is 1.8 x 10^-5  the hydrolysis constant of NH₄Cl would be _______.

(a)

1.8 × 10^-19

(b)

5.55 × 10^-10

(c)

5.55 × 10^-5

(d)

1.80 × 10^-5

What are Lewis acids and bases? Give two example for each.

Discuss the Lowry – Bronsted concept of acids and bases.

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

Define solubility product.

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

Derive an expression for Ostwald’s dilution law.

Define pH.

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

A solution of 0.10M of a weak electrolyte is found to be dissociated to the extent of 1.20% at 25^oC. Find the dissociation constant of the acid.

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

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?

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  \(1.8\times10^{-5}\))