The strongest acid among the following compounds is:
1. | HClO3 | 2. | HClO4 |
3. | H2SO3 | 4. | H2SO4 |
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For the reaction the equilibrium constant is K1. The equilibrium constant is K2 for the reaction
The value of K for the reaction given below will be:
1.
2.
3.
4.
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A saturated solution of Ba(OH)2 has a pH of 12. The value of its Ksp will be:
1.
2.
3.
4.
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The equilibrium reaction that doesn't have equal values for Kc and Kp is:
1. \(2NO(g) \rightleftharpoons N_2(g) + O_2(g)\)
2. \(SO_2(g) + NO_2(g) \rightleftharpoons SO_3(g) + NO(g)\)
3. \(H_2(g) + I_2(g) \rightleftharpoons 2HI (g)\)
4. \(2C(s) + O_2(g) \rightleftharpoons 2CO_2(g)\)
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In a buffer solution containing an equal concentration of B- and HB, the Kb for B- is 10-10. pH of the buffer solution is:
1. | 10 | 2. | 7 |
3. | 6 | 4. | 4 |
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The value of the equilibrium constant of the reaction
is 8.0.
The equilibrium constant of the reaction
will be-
1. | \(1 \over 16\) | 2. | \(1 \over 64\) |
3. | 16 | 4. | \(1 \over 8\) |
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The pOH of a solution at 25 °C that contains 1×10-10 M of hydronium ions is:
1. | 7.00 | 2. | 4.00 |
3. | 9.00 | 4. | 1.00 |
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The ionic species that has the greatest proton affinity to form stable compound is:
1.
2.
3.
4.
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The following pair constitutes a buffer is:
1.
2.
3.
4.
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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.
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