Question

A) The K_{sp} of BaCO_{3} is 5.0 x
10^{-9}. What is the soliubility of barium carbonate in a
solution that contains 1.56 M of Na_{2}CO_{3}?

B) At a ceratin temperature ths solubility of
Ca_{3}(PO_{4})_{2} is 1.43 x
10^{-6}M. What is the K_{sp} at this
temperature?

Express your answer in scientific notation.

Answer #1

A )

[CO3-2] = 1.56 M

BaCO3 ----------------------> Ba+2 + CO3-2

S S ------------> in absence common ion

S S + 1.56------------> in absence common ion

S 1.56

Ksp = [Ba+2][CO3-2]

5.0 x 10^-9 = (S) x 1.56

S = 3.20 x 10^-9 M

**solubility = 3.20 x 10^-9 M**

B)

Solubility = S = 1.43 x 10^-6

Ca3(PO4)2 --------------------> 3 Ca+2 + 2 PO4-3

3S 2S

Ksp = [Ca+2]^3 [PO4-3]^2

Ksp = (3S)^2 (2S)^3

Ksp = 108 S^5

Ksp = 108 x (1.43 x 10^-6)^5

**Ksp = 6.46 x 10^-28**

The Ksp for BaCO3 is 1.6 x 10-9 .
A)Write a chemical equation for the equilibrium of
BaCO3 (s) with its ions.
B) When 20.0 mL of a 0.10 M Ba(NO3)2 is
added to 50.0 mL of a 0.10 M Na2CO3 calculate
the reaction quotient and determine if a precipitate will form?
C) For the same reaction, predict the direction the system once
it gets to equilibrium will shift when acid is added to the
system.

The Ksp for BaCO3 is 1.6 x 10-9 .
A)Write a chemical equation for the equilibrium of
BaCO3 (s) with its ions.
B) When 20.0 mL of a 0.10 M Ba(NO3)2 is
added to 50.0 mL of a 0.10 M Na2CO3 calculate
the reaction quotient and determine if a precipitate will form?
C) For the same reaction, predict the direction the system once
it gets to equilibrium will shift when acid is added to the
system.

What is the molar solubility BaCO3 in pure water?
(Ksp = 5.1*10-9)
Answer = 7.1 * 10-5M

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...

a. The Ksp for Ag2SO3 = 1.50 X
10-14. What is the molar solubility of
Ag2SO3 in a 5 M solution of lithium
sulfite?
b.The Ksp for
Mg3(PO4)2 = 1.04 X
10-24. What is the molar solubility of
Mg3(PO4)2 in a 1.40 M solution of
sodium phosphate?
c.If the Ksp for Y(OH)3 = 1.00 X 10-22,
what is the molar solubility of Y(OH)3 in a buffer
solution composed of 1.60M trimethylamine (=
(CH3)3N) (Kb = 6.5 X
10-5) and 1.40M...

Which of the following has the greatest molar solubility?
Ca3(PO4)2 Ksp = 1.0 x 10-26
CaF2 Ksp = 3.4 x 10-11
CaCO3 Ksp = 3.9 x 10-9
CaC2O4 Ksp = 2.3 x 10-9
CaSO4 Ksp = 2.4 x 10-5

1)At 25 oC the solubility of silver iodide is 8.94 x
10-9 mol/L. Calculate the value of Ksp at
this temperature. Give your answer in scientific notation to 2
SIGNIFICANT FIGURES (even though this is strictly incorrect)
2)The Ksp of Al(OH)3 is 1.0 x
10-33. What is the solubility of Al(OH)3 in
0.0000010 M Al(NO3)3? Give your answer using
scientific notation and to 2 significant figures (i.e., one decimal
place).

The Ksp of barium fluoride is 1.00 x 10–6.
The Ksp of calcium fluoride is 3.90 x 10–11.
An aqueous solution of sodium fluoride is slowly added to a
water sample that contains barium ion (4.50×10-2M ) and
calcium ion (3.75×10-2M ). What is the remaining
concentration of the first ion to precipitate when the second ion
begins to precipitate?

The Ksp of barium fluoride is 1.00 x 10^–6. The Ksp of calcium
fluoride is 3.90 x 10^–11. An aqueous solution of sodium fluoride
is slowly added to a water sample that contains barium ion
(3.95×10^-2M ) and calcium ion (4.65×10^-2M ). What is the
remaining concentration of the first ion to precipitate when the
second ion begins to precipitate?_____M

The Ksp of barium fluoride is 1.00 x 10–6. The Ksp of calcium
fluoride is 3.90 x 10–11.
An aqueous solution of sodium fluoride is slowly added to a
water sample that contains barium ion (4.45×10-2M ) and
calcium ion (5.50×10-2M ). What is the remaining
concentration of the first ion to precipitate when the second ion
begins to precipitate?

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