19,000+ solved questions for JEE Advanced, JEE Mains, NEET & IChO — with answers and expert explanations.
The solubility of CaF2 is ‘s’ moles/litre. Then its solubility product is........
The solubility in water of a sparingly soluble salt AB2 is 1.0 × 10 –5moll –1. Its solubility product number will be
Let the solubility of an aqueous solution of Mg(OH)2 be x then its Ksp is
The solubility product of a salt having general formula MX2, in water is : 4 × 10 –12. The concentration of M 2+ ions in the aqueous solution of the salt is
0.1 M solution of which one of these substances will react basic ?
Which is the correct alternate for hydrolysis constant of NH4CN (a) w a K K (b) w a b K K K x (c) b K c (d) a b K K
The aqueous solution of FeCl3 is acidic due to
The dissociation constant of CH3COOH is 1.8 × 10–5. The hydrolysis constant for 0.1 M sodium acetate is
A white salt is readily soluble in water and gives a colourless solution with a pH of about 9. The salt would be
Aqueous solution of sodium acetate is
The pH of 0.1 M solution of the following salts increases in the order :
The aqueous solution of ammonium chloride is
An aqueous solution of sodium carbonate is alkaline because sodium carbonate is a salt of
An aqueous solution of aluminium sulphate would show
Which one of the following salts gives an acidic solution in water
The solution of strong acid and weak base (FeCl3) is
Aq. solution of sodium cyanide is
Ka for HF is 3.5 × 10–4. Calculate Kb for the fluoride ion.
HCN is a weak acid (Ka = 6.2 × 10–10). NH4OH is a weak base (Kb = 1.8 × 10–5). A 1M solution of NH4CN would be :
A physician wishes to prepare a buffer solution at pH = 3.58 that efficiently resists a change in pH yet contains only small conc. of the buffering agents. Which one of the following weak acid together with its sodium…
The pH of blood does not appreciably change by a small addition of acid or a base because blood
How many moles of HCOONa must be added to 1L of 0.1 M HCOOH to prepare a buffer solution with a pH of 3.4 ? (Given : Ka for HCOOH = 2 × 10 –4); (10-0.3 = 0.5)
The dissociation constant of HCN is 5 × 10 –10. The pH of the solution prepared by mixing 1.5 mole of HCN and 0.15 moles of KCN in water and making up the total volume to 0.5 dm 3 is
In a mixture of a weak acid and its salt, the ratio of concentration of acid to salt is increased ten-fold. The pH of the solution
The pKa value of NH3 is 5. Calculate the pH of the buffer solution, 1 L of which contains 0.01 M NH4Cl and 0.10 M NH4OH