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At 90oC, pure water has H3O+ ion concentration of 10-6 mol/L. The Kw at 90oC is
The hydrogen ion concentration of a 10–8 M HCl aq. solution at 298K (Kw = 10–14) is (a) 1.0 10 M x (b) 1.10 10 M x (c) 9.525 10 M x (d) 1.0 10 M x
The concentration of water molecules in pure water at 298 K is
For a pure water,
A monoprotic acid in 1.00 M solution is 0.01% ionized. The dissociation constant of this acid is (a) 1 10 x (b) 1 10 x (c) 1 10 x (d) 1 10 x
At infinite dilution, the percentage ionisation for both strong and weak electrolytes is
Concentration CN – in 0.1 M HCN is [Ka = 4 × 10 –10]
For a weak acid HA, Ostwald’s dilution law is represented by the equation (a) a c K 2 (b) a c K (c) a K c c (d) a c K
The a K of an acid is 3.2 10 x . The degree of dissociation of the acid at concentration of 0.2M is (a) 6.0 10 x (b) –2 1.26 10 x (c) –4 x (d) 0.04 10 x
The conjugate acid of HPO4 2– is
Conjugate base of NH3 is (a) NH (b) NH (c) NH
The correct order of acid strength is
Cl – is the conjugate base of
The conjugate base of NH2 – is
A weak acid, HA has a Ka of 1.00 10 x . If 0.100 mole of this acid is dissolved in 1 L of water, the percentage of acid dissociated at equilibrium is closest to
The correct order of acid strength is
The solubility of CaCO3 is 7 mg/L. Calculate the solubility product of BaCO3 from this information and from the fact that when Na2CO3 is added slowly to a solution containing equimolar concentration …
The solubility of AgCl is maximum in
The solubility of LiOH in a solution with pH = 8 is (Ksp = 1.8 × 10–12)
Assertion (A): pH of HCl solution is less than that of acetic acid of the same concentration. Reason (R): In equimolar solutions, the number of titrable protons present in HCl in less than that present in acetic…
Assertion: If HA and HB are two weak non-basic acids with Ka(HA) < Kb(HB), then, the aqueous solution of NaA will have higher pH than pH of aqueous solution of NaB of same concentration. Reason: Conjugate base of a…
Assertion: When aqueous, solution of CH3COOAg is diluted, then its degree of hydrolysis increases. Reason: Silver acetate is the salt of weak acid and weak base; its degree of hydrolysis does not depend on th…
Assertion: When aqueous, solution of CH3COONH4 is diluted, then its degree of hydrolysis increases. Reason: Ammonium acetate is the salt of weak acid and weak base; its degree of hydrolysis does not de…
Assertion: Aqueous solution of ammonium carbonate is basic. Reason: Acidic or Basic nature of a salt solution of a salt of weak acid and weak base depends on Ka and Kb of the acid and base forming it.
Assertion: If a K of HA is 10–3 and a K of HB is 10 at 25ºC, pH of an aqueous solution of HB will be one unit greater than pH of equimolar solution of HA. Reason: For weak acids, both concentration and ionizat…