The solubility product (Ksp) of a salt, having general formula MX2, is 4 x 10-12. A salt willdissolve in water to make ions. MX2 will form M2+ and X- in water. The concentration of M2+ions in the aqueous solution of the salt is

For a binary salt AB the Ksp is 4 × 10–10. The molar solubility of AB is :-2 × 10–5 M5 × 10–5 M2 × 10–10 M4 × 10–5 M

A specific metal ion, M2+, forms a relatively insoluble sulfide compound, MS, which dissolves to a very limited extent.MS(s)   ⇋  M2+(aq)  +  S2-(aq)The concentration of ions in a saturated solution was found:[M2+(aq)]  ≡  [S2-(aq)]  =  0.000142 mol L-1.Calculate Ksp for the compound MS.Give three significant figures.Enter your answer in exponential form, for example, enter 0.000000672  as 6.72e-7 with no gaps and the -ve e if power is -ve.

Ksp of Ag2S is 4  10-48 at 250C. Calculate its solubility in a pure water and 0.01 M aqueous solution of Ag2S.

What is the molar solubility of Mg(OH)2 in a basic solution with a pH of 12.00? Ksp for Mg(OH)2 is 5.6 × 10-12.Group of answer choices5.6 × 10-10 M5.6 × 10-8 M1.1 × 10-4 M2.4 × 10-6 M

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