Question

3. The Ksp for silver chloride is 1.8 x 10-10 at 25 °C. What is the solubility of silver chloride (in mol L"?) in 0.025 M tin(IV) chloride solution? a) 8.5 x 10-5 b) 6.7 x 108 c) 7.2 x 10-9 d) 1.8 x 10-9 e) 1.3 x 10-5 4. What is the concentration of Zn2+(aq) ions in the solution made by adding water to zinc nitrate (0.10 mol) and ammonia (3.0 mol) so that the final volume of solution is 1.5 L? The Kstab of [Zn(NH3)4]2+ is 7.8 x 108 a) 4.9 x 10-11 M b) 9.5 x 10-12 M c) 6.1 x 10-12 M d) 2.8 x 10-12 M e) 2.3 x 10-13 M

Answer 1

3)

SnCl4 here is Strong electrolyte

It will dissociate completely to give [Cl-] = 4*[SnCl4]

= 4*0.025 M

= 0.1 M

At equilibrium:

AgCl <----> Ag+ + Cl-

   s 0.1 + s

Ksp = [Ag+][Cl-]

1.8*10^-10=(s)*(0.1+ s)

Since Ksp is small, s can be ignored as compared to 0.1

Above expression thus becomes:

1.8*10^-10=(s)*(0.1)

s = 1.8*10^-9 M

Answer: d

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