For the reaction: mgf2(s) ⇌ mg2+(aq) + 2f- (aq), ksp= 6.4 × 10-9, the addition of 0.10 m naf to the solution cause what effect on the solubility equilibrium? view available hint(s) for the reaction: mgf2(s) ⇌ mg2+(aq) + 2f- (aq), ksp= 6.4 × 10-9, the addition of 0.10 m naf to the solution cause what effect on the solubility equilibrium? shifts the equilibrium to the right, reduces solubility. shifts the equilibrium to the left, reduces solubility. shifts the equilibrium to the left, increases solubility. shifts the equilibrium to the right, increases solubility.

Shifts the equilibrium to the left. reduces solubility.

Explanation:

          S                   S              2S

∴ Ksp = 6.4 E-9 = [ Mg2+ ] * [ F- ]² = S * (2S)²

⇒ 4S² * S = 6.4 E-9

⇒ 4S³ = 6.4 E-9

⇒ S³ = 1.6 E-9

⇒ S = 1.1696 E-3 M

        0.10M     0.10M        0.10M

          S'                 S'              2S' + 0.10

⇒ Ksp = 6.4 E-9 = (S')*(2S' + 0.10)²

If we compare the concentration (0.10 M) of the ion with Ksp ( 6.4 E-9 ); thne we can neglect S' as adding:

⇒ 6.4 E-9 = (S')*(0.10)² = 0.01S'

⇒ S' = 6.4 E-7 M

∴ % S' = ( 6.4 E-7 / 0.1 )*100 = 6.4 E-4% <<< 5%, we can make the assumption

We can observe that S >> S' ( 1.1696 E-3 M >> 6.4 E-7 M ), which shows that the solubility  is reduced by the efect of the common ion from the salt, which causes the equilibrium to shift to the left, precipitating part of MgF2(s).

the answer is 1260

you spend 7 hours in school for 1 school day with 5 school days in 1 school week with 36 school weeks in a school year.

7*5*36= 1260 it's all about multiplying