19,000+ solved questions for JEE Advanced, JEE Mains, NEET & IChO — with answers and expert explanations.
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)
The correct order of increasing [H3O+] in the following aqueous solution is:
H S aq H aq HS aq ;K 9.5 10 x HS aq H aq S aq ;K 1.0 10 x Given the equilibrium constants provided what is the equilibrium constant for the reaction: S (aq) 2H (aq) H S(aq) K = ?
How many milliliters (mL) of a 0.0500 M NaOH (a strong base) solution should be added to 1.00 L of 0.100 M H3PO4, solution to produce a buffer of pH = 2.00 ? For H3PO4, a K = 6.67 × 10–3 Given: H P…
How many milliliters of 0.250 M NH4Cl would have to be added to 450 mL of 0.350 M KOH in order to produce a buffer solution with a pH of 9.10? (Kb(NH3) = 1.8 × 10–5)
Which pair of reagents, mixed in the appropriate proportion, could make a buffer in pH 3-4 range ?
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 …
The pH of 10–5 M HCl solution if 1 ml of it is diluted to 1000 ml 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
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
For a “c molar” concentrated solution of a weak electrolyte AxBy, the degree of dissociation is given as (a) (b) (c) (d)
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