Advertisements
Advertisements
प्रश्न
Write the relationship between solubility and solubility product for PbI2.
उत्तर
Solubility equilibrium for PbI2, is given by,
\[\ce{PbI2_{(s)} ⇌ Pb^{2⊕}_{(aq)} + 2I^⊖_{(aq)}}\]
∴ x = 1, y = 2
∴ Ksp = (1)1 (2)2 S1+2
∴ Ksp = 4 S3
The above expression shows the relationship between solubility and solubility product for PbI2.
APPEARS IN
संबंधित प्रश्न
Choose the most correct answer :
The solubility product of a sparingly soluble salt AX is 5.2 × 10–13. Its solubility in mol dm–3 is ______.
Answer the following :
Explain the relation between ionic product and solubility product to predict whether a precipitate will form when two solutions are mixed?
If ‘IP’ is the ionic product and ‘Ksp’ is the solubility product, precipitation of the compound will occur under the condition when:
Write the solubility product of sparingly soluble salt Bi2S3.
Write the relationship between molar solubility (S) and solubility product (Ksp) for CaF2.
The solubility product of BaCl2 is 4.0 × 10-8. What will be its molar solubility in mol dm-3?
Define molar solubility. Write it’s unit.
Write solubility product of following sparingly soluble salt.
BaSO4
Concentration of the Ag+ ions in a saturated solution of Ag2C2O4 is 2.24 × 10−4 mol L−1 solubility product of Ag2C2O4 is ____________.
The solubility of AgCl(s) with solubility product 1.6 × 10−10 in 0.1 M NaCl solution would be ____________.
MY and NY3, are insoluble salts and have the same Ksp values of 6.2 × 10−13 at room temperature. Which statement would be true with regard to MY and NY?
Solubility product of Ag2CrO4 is 1 × 10−12. What is the solubility of Ag2CrO4 in 0.01 M AgNO3 solution?
A saturated solution, prepared by dissolving CaF2(s) in water, has [Ca2+] = 3.3 × 10−4 M What is the Ksp of CaF2?
Ksp of AgCl is 1.8 × 10−10. Calculate molar solubility in 1 M AgNO3.
A particular saturated solution of silver chromate Ag2CrO4 has [Ag+] = 5 × 10−5 and [CrO4]2− = 4.4 × 10−4 M. What is the value of Ksp for Ag2CrO4?
The solubility product of AgBr is 5.2 × 10−13 Calculate its solubility in mol dm−3 and g dm−3 (Molar mass of AgBr = 187.8g mol−1)
The solubility product of Agl is 1.56 x 10−16. What iodide ion concentration will be required to precipitate Agl from 0.01 M AgNO3 solution?
Define solubility. How is it expressed?
Calculate the current strength (I) and number of moles of electrons required to produce 2.369 × 10−3 kg of Cu from CuS04 in one hour. (Given: Molar mass of Cu = 63 .5 gm/mol).
The solubility of silver sulphate is 1.85 x 10-2 mol dm-3. Calculate solubility product of silver sulphate.
Derive the relationship between solubility and solubility product of AgBr.
