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 solubility product for a salt of type AB is . The molarity of its standard solution will be:
1.
2.
3.
4.
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
The pKb of dimethylamine and pka of acetic acid are 3.27 and 4.77 respectively at T (K).
The correct option for the pH of dimethylammonium acetate solution is:
1. | 7.75 | 2. | 6.25 |
3. | 8.50 | 4. | 5.50 |
The conjugate bases of Bronsted acids H2O and HF are respectively:
1. H3O+ and H2F+, respectively.
2. OH– and H2F+, respectively.
3. H3O+ and F–, respectively.
4. OH– and F–, respectively.
pH of a saturated solution of is 9. The solubility product of is:
1.
2.
3.
4.
Which composition will make the basic buffer?
1. | 100 mL of 0.1 M HCl+100 mL of 0.1 M NaOH |
2. | 50 mL of 0.1 M NaOH+25 mL of 0.1 M CH3COOH |
3. | 100 mL of 0.1 M CH3COOH+100 mL of 0.1 M NaOH |
4. | 100 mL of 0.1 M HCl+200 mL of 0.1 M NH4OH |