1. | 7.01 | 2. | 2 |
3. | 12 | 4. | 9 |
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. \(\mathrm{HCl}\)
4. \(\mathrm{H S O_{4}^{-}}\)
The molar solubility of in 0.1 M solution of NaF will be:
1. | 2. | ||
3. | 4. |
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 |
The hydrogen ion concentration of a 10-8 M HCl aqueous solution at 298 K (Kw = 10-14) is:
1.
2.
3.
4.
The following pair constitutes a buffer is:
1.
2.
3.
4.
For the reaction,
CH4(g) + 2O2(g) CO2(g) + 2H2O(l)
ΔrH = -170.8 kJ mol-1
Which of the following statements is not true?
1. | At equilibrium, the concentration of \(\mathrm{CO}_2 \mathrm{~g}\) and water (l) are not equal. |
2. | The equilibrium constant for the reaction is given by \(K_p=\frac{\left[\mathrm{CO}_2\right]}{\left[\mathrm{CH}_4\right]\left[\mathrm{O}_2\right]}\) |
3. | The addition of \(\mathrm{CH}_4 \mathrm{~g} \) or \(\mathrm{O}_2 \mathrm{~g}\) at equilibrium will cause a shift to the right |
4. | The reaction is exothermic |
Which one of the following orders correctly represents the increasing acid strengths of the given acids?
1.
2.
3.
4.