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Class XI Chemistry Equilibrium 6: Important Questions
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Question 1
In the following reaction
HC2O4– + PO43–HPO42– + C2O42–
which are the two Bronsted bases ?
HC2O4– + PO43–HPO42– + C2O42–
which are the two Bronsted bases ?
Question 2
According to Le-Chatelier’s principle, adding heat to a solid and liquid in equilibrium will cause the
Question 3
Calculate the pH of a 0.1M K3PO4 solution. If the third dissociation constant of phosphoric acid is 10–12. (Given (0.41)1/2 = 0.64 & log3 = 0.48)
Question 4
At what minimum concentration of OH– will 10–3 mole of Zn(OH)2 go into solution as in 1L solution.
Given:
(aq.)Zn2+(aq.) + 4OH– (aq.)
K = 10–15
Zn(OH)2 (s) Zn2+ (aq.) + 2OH– (aq)
Ksp = 10–17
Given:
(aq.)Zn2+(aq.) + 4OH– (aq.)
K = 10–15
Zn(OH)2 (s) Zn2+ (aq.) + 2OH– (aq)
Ksp = 10–17
Question 5
At 25 °C, the solubility product of Mg(OH)2 is 1.0 × 10–11. At which pH, will Mg2+ ions start precipitating in the form of Mg(OH)2 from a solution of 0.001 M Mg2+ ions?
Question 6
For the decomposition reaction NH2COONH4 (s) 2NH3 (g) + CO2 (g) the KP = 2.9 × 10–5 atm3. The total pressure of gases at equilibrium when 1 mol of NH2COONH4(s) was taken initially could be -
Question 7
A 1 litre container contains 2 moles of PCl5 initially. If at equilibrium, KC is found to be 1, degree of dissociation of PCl5 is -
Question 8
For the reaction, A(g) + B(g) C(g) + D(g) at 298K, the values of ΔH º and ΔS º are –29.8 kcal and –0.1 kcal K–1 respectively. The values of ΔG º and equilibrium constant Kc are-
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Jun 12JEE & BITSAT