Equilibrium constants K1 and K2 for the following equilibria
are related as:
1.
2.
3.
4.
Conjugate acid of NH2– is:
1. NH4OH
2. NH4+
3. \(NH_{2}^{-}\)
4. NH3
Incorrect statement about pH and H+ is:
1. | pH of neutral water is not zero. |
2. | Adding 1M solution of CH3COOH and 1M solution of NaOH, the pH will be 7. |
3. | H+ of dilute and hot H2SO4 is more than concentrate and cold H2SO4 |
4. | Mixing solution of CH3COOH and HCl, pH will be less than 7 |
At 25 ºC, the dissociation constant of a base, BOH, is 1.0 × 10–12. The concentration of hydroxyl ions in 0.01M aqueous solution of the base would be:
1. | 1.0 × 10–6 mole L–1 | 2. | 1.0 × 10–7 mole L–1 |
3. | 2.0 × 10–6 mole L–1 | 4. | 1.0 × 10–5 mole L–1 |
then C + D + E + F ⇒ product. The constant of reaction will be:
1.
2.
3.
4. None of these
The fertilizer which makes the soil acidic is:
1.
2. Super phosphate of lime .
3.
4.
Among the following examples, the species that behave(s) as a Lewis acid is/are:
1. Stannous chloride, stannic chloride
2. , stannous chloride
3. Only
4. , stannous chloride , stannic chloride
4 gm of NaOH is dissolved in 1000 ml of water. The ion concentration will be:
1. | 10-1 M | 2. | 10-13 M |
3. | 10-4 M | 4. | 10-10 M |
The solubility product of a sparingly soluble salt AX2 is 3.2 ×10–11. Its solubility (in moles/litre) is:
1. 3.1×10–4
2. 2 × 10–4
3. 4 × 10–4
4. 5.6 × 10–6
A compound BA2 has \(K_{sp} = 4\times 10^{-12}\)Solubility of this compound will be:
1. | 10-3 | 2. | 10-4 |
3. | 10-5 | 4. | 10-6 |