Answered! Question: A) A saturated solution of lead(II) fluoride, , was prepared by dissolving solid in water. The c……

A) A saturated solution of lead(II) fluoride, $rm PbF_2$ , was prepared by dissolving solid $rm PbF_2$ in water. The concentration of $rm Pb^{2+}$ ion in the solution was found to be $2.08times 10^{-3}$ $;M$ . Calculate K_sp for $rm PbF_2$ .

B)The value of K_sp

for silver sulfate, $rm Ag_2SO_4$ , is $1.20times 10^{-5}$ . Calculate the solubility of $rm Ag_2SO_4$ in grams per liter.

C) If 500.0

of 0.10 $M~rm Ca^{2+}$ is mixed with 500.0

of 0.10 $M~rm {SO_4}^{2-}$ , what mass of calcium sulfate will precipitate?

K_sp for $rm CaSO_4$ is $2.40times 10^{-5}$ .

D) What is the pH of a buffer prepared by adding 0.809 mol of the weak acid $rm HA$ to 0.305 mol of $rm NaA$ in 2.00 $rm L$ of solution? The dissociation constant K_a of $rm HA$ is $5.66times 10^{-7}$ . What is the $rm pH$ after 0.150 mol of $rm HCl$ is added to the buffer from Part A? Assume no volume change on the addition of the acid. What is the $rm pH$ after 0.195 mol of $rm NaOH$ is added to the buffer from Part A? Assume no volume change on the addition of the base.

Expert Answer

A saturated solution of lead(II) fluoride, $rm PbF_2$ , was prepared by dissolving solid $rm PbF_2$ in water. The concentration of $rm Pb^{2+}$ ion in the solution was found to be $2.08times 10^{-3}$ $;M$ . Calculate K_sp

for $rm PbF_2$ .

[Pb2+] = 2.08 * 10^-3 M

One mole of Pb F2 gives two moles of fluoride ions

so [F-] = 2 * 2.08 * 10^-3 M

Ksp = ionic product of a saturated solution

= [Pb^2+] [ Cl -]^2

= (2.08 * 10^-3 M) * (2.08 * 10^-3 M)^2

= 9.00 * 10^-9

Solubility of silver sulfate can be calculated using the Ksp formula:

Ksp = [Ag2+] [SO4^2-]

Hope this helps

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