Question

Calculate the solubility of Mercury (I) carbonate, Hg2CO3 if its solubility product constant, Ksp is 8.9 X 10^-17

Answer #1

Ksp = 8.9x10^-17

Hg2CO3 ---------------------- 2 Hg+ + CO3-2

2S S where S=molar solubility

Ksp = [Hg+]^2[CO3-2]

Ksp = (2s)^2 (S)

Ksp = 4S^3

S^3=Ksp/4

S^3 = 8.9x10^-17/4=2.225 x10^-17=22.25x10^-18

S=2.812x10^-6

Solubity of Hg2CO3= 2.81x10^-6 M

Calculate the Ksp (solubility product CONSTANT) value of AgI if
at equilibrium [I -] = 1.23 x 10 -6 M (Hint: write the balanced
chemical reaction and Ksp expression) Enter using 'e' notation:
.00555 would be entered 5.55e-3

The solubility product constant Ksp of
Mn(OH)2 is 2.1 x 10-13 at 25oC.
The molar mass of Mn(OH)2 is 88.96 g/mol.
a. Calculate its molar solubility
b. Calulate its solubility in g/L

The Ksp for silver carbonate (Ag2CO3) is 8.1???10?12. Calculate
the solubility of silver carbonate in each of the following.
(a) water mol/L
(b) 0.15 M AgClO3 mol/L
(c) 0.43 M Na2CO3 mol/L

Calculate the molar solubility of silver phosphate in a 0.030M
Na3PO4 solution. Ksp for silver
phosphate is 8.9×10-17.

The solubility-product constants, Ksp, at 25 ∘C for two
compounds [iron(II) carbonate, FeCO3, and cadmium(II) carbonate,
CdCO3] are given: FeCO3=2.10×10−11, CdCO3=1.80×10−14.
[CO3^-2]= 1.22x10^-12M
What will the concentration of CO32− be at the moment before
Fe2+ begins to precipitate?
Express your answer with the appropriate units.

calculate the molar solubility of the following salts
under specific conditions:
Calcium carbonate(CaCO3) in water [Ksp= 4.5*10^-9]
Calcium fluoride (CaF2) in water [Ksp= 3.2*10^-11]
Zinc (11) hydroxide (Zn(OH)2) in a solution of pH=
7.50 [Ksp=3.0*10^-16]

What is the molar solubility of Silver Carbonate in pure water
if its Ksp = 8.1x10^-12? What is its molar solubility in a 0.1 M
KNO3 solution? (An activity problem) . Explain how and why
solubility changed.

the solubility-product constant (ksp) for MgCO3 at 25 degrees
celcius is 6.8 x 10^-6. what is the molar solubility of this
substance in 0.22M MgCl2 at 25 degrees C?

Calculate Kc of the following reaction: CuBr(s)+Br-(aq)---->
CuBr2-(aq) The solubility product constant, Ksp, for CuBr is 6.27×
10–9 and the overall formation constant, Kf (β2), for CuBr2– is
8.0× 105.

The solubility-product constants, Ksp, at 25 ∘C for two
compounds [iron(II) carbonate, FeCO3, and cadmium(II) carbonate,
CdCO3] are given by the table
Part A
A solution of Na2CO3 is added dropwise to a solution that
contains 1.04×10−2M Fe2+ and
1.50×10−2M Cd2+. What concentration of CO32− is
need to initiate precipitation? Neglect any volume changes during
the addition.
Express the molar concentration numerically.
Part B
In the solution from Part A, what will the concentration of
CO32− be when Fe2+ begins...

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