The first ionization constant of H2S is 9.1 × 10–8. The concentration of HS– ion in its 0.1 M solution will be:
1. | 12.3 x 10-7 M | 2. | 11.4 x 10-6 M |
3. | 3.5 x 10-4 M | 4. | 9.54 x 10-5 M |
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The ionization constant of acetic acid is 1.74 × 10–5. The pH of acetic acid in its 0.05 M solution will be:
1. | 7.81
|
2. | 3.03
|
3. | 8.54
|
4. | 1.45 |
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The ionization constant of propanoic acid is 1.32 × 10–5. The degree of ionization of 0.05M acid solution will be:
1. = 0.63 x 10-2
2. = 1.63 x 10-4
3. = 1.63 x 10-2
4. = 0.05 x 10-2
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The salt that gives a neutral solution in water is:
1. KBr
2. NH4NO3
3. NaCN
4. Rb2(CO3)
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The equilibrium constant Kc expression for the above mentioned reaction is:
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OH– , F– , H+ and BCl3
The species described above that contain Lewis acids are:
1. BCl3 and F-
2. OH– and F-
3. H+and BCl3
4. F- and BCl3
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The conjugate bases for Brönsted acids, H2SO4, and HCO3- will be, respectively:
1. ,
2. HSO4-, CO3-
3. SO4-2, CO32-
4. HS2O4-, CO32-
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For the given reaction:
PCl5 (g) PCl3 (g) + Cl2 (g), ∆rH° = 124.0 kJ mol–1 and Kc = 8.3 10-3 mol L-1 at 473 K
The effect on Kc if (i) pressure is increased and (ii) the temperature is increased will be, respectively-
1. (i) Will increase; (ii) will decrease
2. (i) Will decrease; (ii) will remain the same
3. (i) Will remain the same; (ii) will increase
4. (i) will remain the same; (ii) Will decrease
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(a) PCl5 (g) PCl3 (g) + Cl2 (g)
(b) CaO (s) + CO2 (g) CaCO3 (s)
(c) 3Fe (s) + 4H2O (g) Fe3O4 (s) + 4H2 (g)
The effect of an increase in the volume on the number of moles of products in the above-mentioned reactions would be, respectively:
1. a) Increase, b) decrease, c) same
2. a) Decrease, b) same, c) increase
3. a) Increase, b) increase, c) same
4. a) Increase, b) decrease, c) increase
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The solubility product for a salt of type AB is . The molarity of its standard solution will be:
1.
2.
3.
4.
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