The degree of dissociation of water at 25°C is 2 × 10-7 % and density is 1.0 g cm-3. The ionization constant for water is - [IIT-1995]
A buffer solution can be prepared from a mixture of -
The pH of 0.1 M solution of the following salts increases in the order [JEE 1999]
An aqueous soltion of 6.3 g oxalic acid dihydrate is made up to 250 mL. The volume of 0.1 N NaoH required to completely neutralise 10 mL of this solution is : [JEE 2001]
For sparingly soluble salt ApBq, the relationship of its solubility product (Ls) with its solubility (S) is [JEE 2001]
A solution which is 10-3 M each in Mn2+, Fe2+, Zn2+ and Hg2+ is treated with 10-16 M sulphide ion. If Ksp, MnS, FeS, ZnS and HgS are 10-15, 10-23, 10-20 and 10-54 respectively, which one will precipitate first ? [JEE 2003]
HX is a weak acid (Ka = 10-5). It forms a salt NaX (0.1 M) on reacting with caustic soda. The degree of hydrolysis of NaX is [JEE 2004]
CH3NH2 (0.1 mole, Kb = 5 × 10-4) is added to 0.08 moles of HCl and the solution is diluted to one litre, resulting hydrogen ion concentration is [JEE 2005]
Ag+ + NH3 [Ag(NH3)]+ ; k1 = 3.5 × 10-3
[Ag(NH3)]+ + NH3 [Ag(NH3)2]+ ;
k2 = 1.7 × 10-3
then the formation constant of [Ag(NH3)2]+ is [JEE 2006]
The species present in solution when CO2 is dissolved in water: [JEE 2006]
Solubility product constant (Ksp) of salts of types MX, MX2 and M3X at temperature 'T' are 4.0 × 10-8, 3.2 × 10-14 and 2.7 × 10-15, respectively. Solubilities (mol. dm-3) of the salts at temperature 'T' are in the order
2.5 mL of M weak monoacidic base (Kb = 1 × 10-12 at 25°C) is titrated with M HCl in water at 25°C. The concentration of H+ at equivalence point is (Kw = 1 × 10-4 at 25°C) [JEE 2008]
Aqueous solutions of HNO3, KOH, CH3COOH, and CH3COONa of identical cocentrations are provided. The pair(s) of solutions which form a buffer upon mixing is(are). [JEE 2010]
A buffer solution consists of weak acid and its salt with strong base or weak base and its salt with strong acid.
If we limit the amount of nitric acid, then it will partially convert sodium acetate to acetic acid.
Now the solution contains acetic acid (weak acid) and sodium acetate (salt with strong base NaOH). So, it will become a buffer solution.
Acetic acid (weak acid) and sodium acetate (salt with strong base NaOH) also form a buffer solution.
Hence both C and D are correct.
The Ksp of Ag2CrO4 is 1.1 × 10-12 at 298 K. The solubility (in mol/L) of Ag2CrO4 in a 0.1 M AgNO3 solution is [IIT-2013]
The initial rate of hydrolysis of methyl acetate (1M) by a weak acid (HA, 1M) is 1/100th of a strong acid (HX, 1M) at 25ºC. The Ka of HA is [IIT-2013]
The Ksp of Ag2CrO4 is 1.1 × 10-12 at 298 K. The solubility (in mol/L) of Ag2CrO4 in a 0.1 M AgNO3 solution is