Question

write the specific defenintion on Ksp found in your text boo

Question 3 2 pts Solid Mn(OH)2 is added to a solution of 0.100 M FeCl2. After reaction, what will be the molar concentration of Fe2+ ? Helpful formulas: Mn(OH)2(s) 6Mn2+ (aq) + 2OH (aq) Ksp = 1.6 x 10-13 FeCl2(s) Fe2+ (aq) + 2OH- (aq) Ksp = 4.9 x 10-17 O 1.1 x 10-1 M. O 6.8 x 10-2 M. O 0.07 M. O 0.100 M

Answer 1

Given [FeCl₂] = 0.1

We fixed Vol = 1L

So, Moles of FeCl₂ =0.1*1 = 0.1 moles

Ksp =[Mn²⁺] [OH^-]²

1.6*10^-13 = x * (2x)² = 4x³

x³ = 4*10^-14

x= 3.42*10^-5 M = [Mn²⁺]

Reaction ratio = 1:1

Mole of MnCl₂ = Fe(OH)₂= 3.42*10^-5 Moles

But [Mn²⁺] = 3.42*10-⁵ this value = 0.000342

therefore [Mn²⁺] =0

Moles of Fe²⁺ after the reaction is given value ie, 0.1 M Because of concentration of Mn does not affect the Fe²⁺

so correct answer is 0.100M