Question

Calculate the molar solubility of PbCl_{2} in 0.332M
CaCl_{2.} K_{sp}=1.72 x10^{-5}

Answer #1

Ksp of PbCl2 = 1.72 x 10^-5

concentration of CaCl2 = 0.332 M

concentration of Cl- = 2 x 0.332 = 0.664 M

PbCl2 ------------> Pb+2 + 2 Cl-

S 0.664

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

1.72 x 10^-5 = S x (0.664)^2

S = 3.90 x 10^-5 M

**Molar solubility of PbCl2 = 3.90 x 10^-5 M**

Calculate the molar solubility in (M) of PbCl2
(ksp=1.2x10-5 at 298K) in
a) pure H2O (l)
b) 0.50M NaCl (aq)

The molar solubility of PbCl2 at
298K is 1.4422×10-2. Determine the Ksp of
this salt.

Calculate the Ksp of a solution of PbCl2 in water. The
temperature is 293 K and the molar solubility is 0.0013 M.

The solubility product constant of lead(ii) chloride , PbCl2 is
1.7*10^-5 . calculate the molar solubility in pure water and in a
0.50 m solution of sodium chloride.

In an experiment to
determine the solubility of PbCl2 in water, it was found
that a maximum of 0.45 g of the salt would dissolve in 100 mL of
water at 25°C.
(A) Calculate the
solubility of PbCl2 in its saturated solution in moles
per litre. (Molar mass of PbCl2 = 278.10 g
mol-1)
(B) Calculate the
Ksp for PbCl2 in water at 25°C.
(C)Comment on the solubility of PbCl2 in a solution
of NaCl at 25°C.
Answers for A=...

The molar solubility of AgCl in 6.5 x10^-3 M AgNO3 is 2.5x10^-8
M. In deriving Ksp from these data, which of the following
assumptions is (are) reasonable
A. Ksp is the same as solubility
B. Ksp of AgCl is the same in 2.5x10^-8 M AgNO3 as in pure
water
C. Solubility of AgCl is independent of the concentration of
AgNO3
D. [Ag+] does not change significantly upon addition of AgCl to
6.5x10^-3 M AgNO3
E. [Ag+] after the addition of...

The Ksp for silver sulfate (Ag2SO4) is 1.2 × 10-5. Calculate the
molar solubility of silver sulfate in a solution of (4.5x10^-1) M
K2SO4 Please clearly show your work and explain steps

MX (Ksp = 5.67×10−36)
Use the Ksp values to calculate the molar solubility of
each of the following compounds in pure water.

Use the Ksp values to calculate the molar solubility of each of
the following compounds in pure water.
MX (Ksp = 1.47×10−38)
Ag2CrO4 (Ksp = 1.12×10−12)

calculate the molar solubility of Ag2SO4 in each solution below.
(the ksp of silver sulfate is 1.5x10^-5)
a.0.34M AgNO3
b.0.34M Na2SO4

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