- 1(current)
Q. No.Given: \(\mathrm{K}_{\mathrm{sp}}\left[\mathrm{~A}(\mathrm{OH})_2\right]=9 \times 10^{-10} \text {}\)
\(\mathrm{K}_{\mathrm{sp}}\left[\mathrm{~B}(\mathrm{OH})_3\right]=27 \times 10^{-18} \text { at } 298 \mathrm{~K} .\)
| 1. | B(OH)3 will precipitate before A(OH)2 |
| 2. | A(OH)2 and B(OH)3 will precipitate together |
| 3. | A(OH)2 will precipitate before B(OH)3 |
| 4. | Both A(OH)2 and B(OH)3 do not show precipitation with NH4OH |
1. To decrease \(OH^-\) ion concentration
2. To increase \(Cl^-\)ion concentration
3. To increase \(NH^+_4\) ion concentration
4. To decrease \(H^+\) ion concentration
40% HI undergoes decomposition to form H₂ and I₂ at 300 K. Find the value of ΔG° for this decomposition reaction at 1 atm pressure in J mol⁻¹ (nearest integer).
(R = 8.31 J K⁻¹ mol⁻¹)
1. 2720
2. 2740
3. 2640
4. 2520
An aqueous solution contains an unknown concentration of Ba2+. When 50 mL of a 1 M solution of Na2SO4 is added, BaSO4 just begins to precipitate. The final volume is 500 mL. The solubility product of BaSO4 is 1 × 10–10. What is the original concentration of Ba2+ ?
1. 5 × 10–9 M
2. 2 × 10–9 M
3. 1 × 10–9 M
4. 1.0 × 10–10 M
In aqueous solution, the ionization constants for carbonic acid are
\(K_{1} = 4.2 \times 10^{- 7}\) and \(K_{2} = 4.8 \times 10^{- 11}\)
The correct statement for a saturated 0.034 M solution of the carbonic acid is:
| 1. | The concentration of H+ is double that of |
| 2. | The concentration of is 0.034 M. |
| 3. | The concentration of is greater than that of |
| 4. | The concentration of H+ and are approximately equal. |
- 1(current)
Q. No.
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