19,000+ solved questions for JEE Advanced, JEE Mains, NEET & IChO — with answers and expert explanations.
Ksp for HgSO4 is 6.4 × 10–5, then solubility of the salt is
The solubility product of Ag2CrO4 is 32 × 10–12. What is the concentration of ions in that solution (in g ions L–1)
The least soluble compound (salt) of the following is
The Ksp of CuS, Ag2S and HgS are 10–31, 10–44 and 10–54 respectively. The solubility of these sulphides are in the order
Why only As+3 gets precipitated as As2S3 and not Zn+2 as ZnS when H2S is passed through an acidic solution containing As+3 and Zn+2 ?
The pH of an aqueous solution of Ba(OH)2 is 10. If the Ksp of Ba(OH)2 is 1 × 10–9, then the concentration of Ba2+ ions in the solution in mol L–1 is
Ksp of Mg(OH)2 is 4.0 × 10–6. At what minimum pH, Mg2+ ions start precipitating 0.01 MgCl
The solubility products of different sparingly soluble salts are : 1. XY = 4 × 10–20 2. X2Y = 3.2 × 10–11 3. XY3 = 2.7 × 10–31 The increasing order of solubility is :
A precipitate of AgCl is formed when equal volumes of the following are mixed. [Ksp for AgCl = 10 –10]
The Ksp of Mg(OH)2 is 1 10 x . 0.01 Mg(OH)2 will precipitate at the limited pH
The precipitation takes place only when the product of concentration of ions
If a saturated solution prepared by dissolving Ag2CO3 in water has Ag 2.56 x . What is the value of Ksp for Ag CO ? (a) 83.9 10 x (b) 8.39 10 x (c) 93.8 10 x (d) 9.38 10 x
Some chemists at ISRO wished to prepare a saturated solution of a silver compound and they wanted it to have the highest concentration of silver ion possible. Which of the following compounds, would th…
The solubility of AgI in NaI solution is less than that in pure water, because
What is the minimum concentration of required to precipitate BaSO4 in a solution containing 1.0 × 10–4 mole of Ba2+ ? Ksp for BaSO4 = 4 × 10–10
The solubility of BaSO4 in water is 2.33 × 10–3g L–1.Its solubility product will be (molecular weight of BaSO4 = 223)
How many grams of CaC2O4 will dissolve in distilled water to make one litre of saturated solution of it ? (Ksp for CaC2O4 = 2.5 × 10–9mol2 lit–2)
The solubility of AgCl at 20ºC is 1.435 × 10–3gm/lit. The solubility product of AgCl is
The solubility product of barium sulphate is 1.5 × 10–9 at 18ºC. Its solubility in water at 18ºC is
The concentration of Ag+ ion in a given saturated solution of AgCl at 25ºC is 1.06 × 10–5g ion per litre. Thus the solubility product of AgCl is
The solubility product of a sparingly soluble salt AB at room temperature is 1.21 × 10–6 M2. Its molar solubility is
If the maximum concentration of PbCl2 in water is 0.01 M at 25ºC, its maximum concentration in 0.1 M NaCl will be
What is the value of Ksp for PbCl2 ?
The solubility of PbCl2 is (a) sp K
Which of the following is most soluble ?