Explanation
High pressure favours forward reaction if np < nr .High temp. favours forward reaction if it is endothermic.
At eqm. ∆G = 0 i.e. G(ice) = G(H2O) ≠ 0.
np < nr and reaction is endothermic. Hence high pressure and high temp. will favour forward reaction
The first two are the step reactions of the required reaction.
Kp is constant at constant temperature. As volume is halved, pressure will be doubled. Hence equilibrium will shift in the backward direction i.e. degree of dissociation decreases.
The reaction proceeds from right to left when Q > Kc so that Q tends to decrease to become equal to Kc.
M H2SO4 produces maximum H+ ions.
H3O+ can give proton
HCl > CH3COOH > H2CO3.
Ionic product of water is same for water, neutral, acidic or basic solutions.
On adding NH3 to water, [OH−]will increase; As
Kw = [H3O+] [OH-], therefore [H3O+] will decrease.
0.01 M CaCl2 ≡ 0.02 M Cl−, 0.01 M NaCl ≡ 0.01 M Cl−, 0.05 M Ag NO3 ≡ 0.05 M Ag+ [Ag+] [CL-]= Ksp (const.). Hence S2 = Ksp/0.02=50 Ksp, S3 = Ksp / 0.01 = 100 Ksp S4 = K sp / 0.05 = 20 Ksp
(a) by Henderson eqn.
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