19,000+ solved questions for JEE Advanced, JEE Mains, NEET & IChO — with answers and expert explanations.
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
What is the equilibrium [OH–] in 0.1413 M H2CO3 ? H CO H O H O HCO (Ka = 4.30 ×10–7)
For a “c molar” concentrated solution of a weak electrolyte AxBy, the degree of dissociation is given as (a) (b) (c) (d)
A student dissolved 0.100 mol of an unknown monoprotic acid, HA, in sufficient water to make 1.00 L of solution. She measured the pH of the solution as pH = 2.60. Of the following, the acid HA is
When one drop of a concentrated HCl is added to 1 L of pure water at 25ºC, the pH drops suddenly from 7 to 4. When the second drop of the same acid is added, the pH of the solution further drops to about
Calculate the concentration of H+ ion in mol/L of 0.010M solution of NH4Cl? (Kb = 1.8 × 10–6)
Ksp of Mg (OH)2 is 1 × 10–12. 0.01 M Mg (OH)2 will be precipitating at the limiting pH :
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…
Assertion (A): H2SO4 acts as a base in the presence of HClO4. Reason (R): Perchloric acid is stronger acid than H2SO4.
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: pH of water increases with an increase in temperature. Reason: Kw of water increases with increase in temperature.
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: 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: 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: 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: 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: 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 (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…
The solubility of LiOH in a solution with pH = 8 is (Ksp = 1.8 × 10–12)
The solubility of AgCl is maximum in
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 volume strength of 1.5 N H2O2 solution is (AIPMT 1997)
CH ,NH ,H O and HF are the example of
Metal hydrides may be ionic, covalent or molecular in nature. Among LiH,NaH,KH,RbH,CsH the correct order of increasing ionic character is
On reaction with water, which of the following does not produce any hydride? (a) CaH (b) Be C (c) Mg N (d) Ca P