Advertisements
Advertisements
Question
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 ______.
Options
7.2 × 10–7
1.35 × 10–4
7.2 × 10–8
13.5 × 10–8
Solution
The solubility product of a sparingly soluble salt AX is 5.2 × 10–13. Its solubility in mol dm–3 is `bb(underline(7.2 xx 10^-7))`.
Explanation:
Ksp = 5.2 × 10–13
\[\ce{\underset{s}{AX} ⇌ \underset{s}{A}^{-} + \underset{s}{X}^{+}}\]
Ksp = [A–][X+]
= s × s
5.2 × 10–13 = s2
`sqrt(10^-13) = sqrt(10^-12)` = 10–6
0.52 × 10–12 = s2
`sqrt(0.52 xx 10^-12)` = s
0.7211 × 10–6 = s
s = 7.211 × 10–7
APPEARS IN
RELATED QUESTIONS
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 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
Write solubility product of following sparingly soluble salt.
CaF2
If ‘S’ is solubility in mol dm–3 and Ksp is the solubility product, then write the relation between them for CaF2 and BaSO4. Calculate the concentration of H3O+ ion in soft drink whose pH is 3.5.
Define Solubility product.
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 BaSO4 in water is 2.42 × 10−3 g L−1 at 298 K. The value of its solubility product (Ksp) will be:
(Given molar mass of BaSO4 = 233 g mol−1)
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?
Write the expression for the solubility product of Ca3(PO4)2.
A saturated solution, prepared by dissolving CaF2(s) in water, has [Ca2+] = 3.3 × 10−4 M What is the Ksp of CaF2?
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?
Write the expression for the solubility product of Hg2Cl2.
Ksp of Ag2CrO4 is 1.1 × 10−12. what is the solubility of Ag2CrO4 in 0.1 M K2CrO4?
Write the relationship between solubility and solubility product for PbI2.
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?
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).
