Given that the ionic product of is 2 × .
The solubility of in 0.1 M NaOH is ;
1. 2 × M
2. 1 × M
3. 1 × M
4. 2 × M
The salt solution that is basic in nature is:
1. Ammonium chloride.
2. Ammonium sulphate.
3. Ammonium nitrate.
4. Sodium acetate.
The molar solubility of in 0.1 M solution of NaF will be:
1.
2.
3.
4.
Which of the following cannot act both as a Bronsted acid and as a Bronsted base?
1. \(\mathrm{H C O_{3}^{-}}\)
2. \(\mathrm{NH_3}\)
3. HCl
4. \(\mathrm{H S O_{4}^{-}}\)
The pH of a 0.01 M NaOH (aq) solution will be:
1. 7.01
2. 2
3. 12
4. 9
Given that the equilibrium constant for the reaction
has a value of 278 at a particular temperature, the value of the equilibrium constant for the following reaction at the same temperature will be:
1.
2.
3.
4.
Given reaction: A2(g) + B2(g) ⇋ 2AB(g)
At equilibrium, the concentrations of A2 = 3.0×10–3 M; B2 = 4.2×10–3 M and AB = 2.8×10–3M. If the reaction takes place in a sealed vessel at 527 °C, then the value of KC will be:
1. | 3.9 | 2. | 0.6 |
3. | 4.5 | 4. | 2.0 |
In qualitative analysis, the metals of Group I can be separated from other ions by precipitating them as chloride salts. A solution initially contains Ag+ and Pb2+ at a concentration of 0.10 M. Aqueous HCl is added to this solution until the Cl– concentration is 0.10 M. What will the concentration of Ag+ and Pb2+ at equilibrium?
(Ksp for AgCl = 1.8 × 10-10)
(Ksp for PbCl2 = 1.7 × 10-5)
1. |
|
2. |
|
3. |
|
4. |
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The reaction-
begins with the concentrations of A and B both at an initial value of 1.00 M. When equilibrium is reached, the concentration of D is measured and found to be 0.25 M. The value for the equilibrium constant for this reaction is given by the expression:
1.
2.
3.
4.
The equilibrium constant Kp for the following reaction is:
1.
2.
3.
4.