19,000+ solved questions for JEE Advanced, JEE Mains, NEET & IChO — with answers and expert explanations.
What is the equilibrium [OH–] in 0.1413 M H₂CO₃ ? H CO H O H O HCO (Ka = 4.30 ×10–7)
A mixture of weak acid is 0.1 M in HCOOH a K 1.8 10 x and 0.1 M in HOCN a K 3.1 10 x Hence, [H O ] is
The equilibrium constant for this reaction is approximately 10–3. HPO (aq.) HCO (aq.) H PO (aq.) CO (aq.) Which is the strongest conjugate base in this reaction? (a) HPO (aq.) (b) HCO (aq.) (c) H PO (aq.) (d) CO (aq.)
Consider the following reaction which proceeds predominantly forward HSO NH NH SO From the information given it is clear that (a) HSOis a stronger acid than NH.
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…
Assertion: pH of 10–8 M HCl lies between 6 and 7. Reason: For very dilute solutions of acids, H⁺ ion contribution from water is also taken into consideration.
A buffer is prepared by adding 0.30 mol CH₃COONa to 2.0 L of a 0.10 M CH₃COOH solution. Calculate the eq K /c (x y) eq K c/(xy) 1/(x y) x y 1 x y eq K /c x y eq K /xyc pH after 0.030 mol HCl are added t…
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…
Assertion: pH of 10–8 M HCl lies between 6 and 7. Reason: For very dilute solutions of acids, H⁺ ion contribution from water is also taken into consideration.
Assertion: pH of water increases with an increase in temperature. Reason: Kw of water increases with increase in temperature.
Assertion: Addition of HCl(aq.) to HCOOH(aq.) decreases the ionization of HCOOH. Reason: Common ion effect of H⁺ ion, reduces the ionization of HCOOH.
Assertion (A): H₂SO₄ acts as a base in the presence of HClO₄. Reason (R): Perchloric acid is stronger acid than H₂SO₄.
The solubility products of MA, MB, MC and MD are 1.8 × 10–10, 4 × 10–3, 4 × 10–8 and 6 × 10–5 respectively. If a 0.01 M solution of MX is added dropwise to a mixture containing A–, B–, C– and D– ions then t…
Ksp of Mg (OH)₂ is 1 × 10–12. 0.01 M Mg (OH)₂ will be precipitating at the limiting pH :
Calculate the concentration of H⁺ ion in mol/L of 0.010M solution of NH₄Cl? (Kb = 1.8 × 10–6)