Equilibrium · Question 35

The solubility of AgCl(s) with solubility product 1.6 10-10 in 0.1 M NaCl solution would be

1. 1.25 10-5 M
2. 1.6 10-9 M
3. 1.6 10-11 M
4. zero

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

1. BF3
2. PF3
3. CF4
4. SiF4

If the equilibrium constant for N2(g) + O2(g) 2NO(g) is K, the equilibrium constant for 12 N2(g) + 12 O2(g) NO(g) will be

1. 12K
2. K
3. K2
4. K1/2

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

1. 2.0
2. 7.0
3. 1.04
4. 12.65

Which one of the following pairs of solution is not an acidic buffer ?

1. CH3COOH and CH3COONa
2. H2CO3 and Na2CO3
3. H3PO4 and Na3PO4
4. HClO4 and NaClO4

The Ksp of Ag2CrO4, AgCl, AgBr and AgI are respectively, 1.1 10-12, 1.8 10-10, 5.0 10-13, 8.3 10-17. Which one of the following salts will precipitate last if AgNO3 solution is added to the solution containing equal moles of NaCl, NaBr, NaI and Na2CrO4?

1. AgBr
2. Ag2CrO4
3. AgI
4. AgCl

If the value of equilibrium constant for a particular reaction is 1.6 1012, then at equilibrium the system will contain

1. mostly products
2. similar amounts of reactants and products
3. all reactants
4. mostly reactants.

Which of the following salts will give highest pH in water?

1. KCl
2. NaCl
3. Na2CO3
4. CuSO4

Using the Gibbs energy change, G = +63.3 kJ, for the following reaction, Ag2CO3(s) 2Ag+(aq) + CO32-(aq) the Ksp of Ag2CO3(s) in water at 25 C is ( R = 8.314 J K-1 mol-1)

1. 3.2 10-26
2. 8.0 10-12
3. 2.9 10-3
4. 7.9 10-2

For the reversible reaction, N2(g) + 3H2(g) 2NH3(g) + heat The equilibrium shifts in forward direction

1. by increasing the concentration of NH3(g)
2. by decreasing the pressure
3. by decreasing the concentrations of N2(g) and H2(g)
4. by increasing pressure and decreasing temperature.