he solubility of CaF2 (Ksp = 3.4 × 10-11) in 0.1 M solution of NaF would be(a) 3.4 × 10-12 M(b) 3.4 × 10-10 M(c) 3.4 × 10-9 M(d) 3.4 × 103 MQ.Type:- MCQ Single, Ans:- cOstwald’s dilution law is applicable for:Q.Type:- MCQ Single, Ans:- bThe conjugate base of OH- is:Q.Type:- MCQ Single, Ans:- bSolution :-One of the following species acts as both Bronsted acid and base:Q.Type:- MCQ Single, Ans:- c

Calculate the molar solubility of CaF2. (Ksp = 3.9 x 10-11)6.24 x 10-6M2.69 x 10-4M2.14 x 10-4M1.33 x 10-5M

Will a precipitate form when 0.10 L of 0.1M Ca(NO3)2 is added to 0.5 L of 0.01M NaF? (Ksp of CaF2 = 3.9 x 10-11)Yes, because Q > Ksp.Yes, because Q < Ksp.Yes, because Q is equal to Ksp.No, because Q < Ksp.

What is the molar solubility ofAg2CO3 (Ksp = 4 × 10–13) in 0.1 M Na2CO3 solution ?10–610–72 × 10–62 × 10–7

Ksp of CaF2 is 1.7  10-10 and its mol. wt. is 78 g mole-1. What volume of the saturated solution will contain 0.078 g of CaF2?

0.200 mol of calcium fluoride, CaF2, is added to 250 cm3 of distilled water which is then made up to a total volume of 1.00 dm3. From this solution, 1.00 cm3 is removed. Calculate the amount (in mol) of fluoride ions, F–, removed from the solution.