Question
In: Chemistry
The solubility of magnesium carbonate is highest in a buffer solution with a pH of :...
The solubility of magnesium carbonate is highest in a buffer solution with a pH of :
a)3.5 b)8.5 c)6.5 d)10.5
Please explain how you come to the conclusion.
Solutions
queen_honey_blossom answered 2 years agoRelated Solutions
Calculate molar solubility of ZnCO3 in a buffer solution of pH = 7
Calculate molar solubility of ZnCO3 in a buffer
solution of pH = 7
a) The molar solubility of barium carbonate in a 0.249 M potassium carbonate solution is _________M....
a) The molar solubility of barium carbonate in
a 0.249 M potassium carbonate
solution is _________M.
b) The solubility of Co(OH)2 is
measured and found to be 3.61×10-4 g/L.
Use this information to calculate a Ksp value for
cobalt(II) hydroxide.
Ksp = ______
c) The solubility of
Ag2SO4 is measured and found
to be 5.17 g/L. Use this information to calculate
a Ksp value for silver
sulfate.
Ksp =_________
The Determination of Magnesium by Direct Titration Preparation of Solutions: Buffer solution, pH 10: Diluted 57mL...
The Determination of Magnesium by Direct Titration
Preparation of Solutions:
Buffer solution, pH 10: Diluted 57mL of NH3 and 7g
NH4Cl totaling 100mL solution
Eriochrome Black T: Dissolved 102.4mg in 15mL ethanolamine and
5mL of absolute ethanol
EDTA: 3.8008g of purified dihydrate Na2H2Y
2H2O, mixed with distilled water to total volume of
1L
I received a Magnesium Sulfate unknown, and diluted it to 500mL
with distilled water then transferred 3 50mL aliquots to separate
conical flasks and added 2mL of...
Calculate the molar solubility of Fe(OH)2 in a buffer solution where the pH has been fixed...
Calculate the molar solubility of Fe(OH)2 in a buffer
solution where the pH has been fixed at the indicated values.
Ksp = 7.9 x 10-16.
(a) pH 8.0
___ M
(b) pH 10.7
___ M
(c) pH 13.6
___ M
HopHelpCh17N6
Calculate the molar solubility of Fe(OH)2 in a buffer solution where the pH has been fixed...
Calculate the molar solubility of Fe(OH)2 in a buffer
solution where the pH has been fixed at the indicated values.
Ksp = 7.9 x 10-16.
(a) pH 7.6
_________M
(b) pH 10.2
__________M
(c) pH 12.0
___________M
A carbonic acid/carbonate buffer is used. Explain the action of said buffer in resisting pH changes...
A
carbonic acid/carbonate buffer is used. Explain the action of said
buffer in resisting pH changes after the addition of NaOH using
relevant chemical equations and Le Chateliers Principle.
Thank you.
13. A. The molar solubility of calcium carbonate in a water solution is _____M. B. The...
13. A. The molar solubility of calcium
carbonate in a water solution is _____M.
B. The equilibrium concentration of cyanide ion
in a saturated zinc cyanidesolution is _____M.
C. The equilibrium concentration of copper(II)
ion in a saturated copper(II) hydroxide solution
is _____M.
Calculate the solubility (in grams per 1.00×102mL of solution) of magnesium hydroxide in a solution buffered...
Calculate the solubility (in grams per 1.00×102mL of solution)
of magnesium hydroxide in a solution buffered at pH = 12. Express
your answer using two significant figures. I got S1 = 1.2×10^-8
which is correct but for this part i did not get it "How does this
compare to the solubility of Mg(OH)2 in pure water? "Express your
answer using two significant figures. please solve it i could not
get the answer.
#16.98 Calculate the solubility (in grams per 1.00×102mL of solution) of magnesium hydroxide in a solution...
#16.98 Calculate the solubility (in grams per 1.00×102mL of
solution) of magnesium hydroxide in a solution buffered at pH = 12.
g/(1.00×102mL)
B) How does this compare to the solubility of Mg(OH)2 in pure
water?
a) Calculate the solubility (in grams per 1.00×10^2mL of solution) of magnesium hydroxide in a solution...
a) Calculate the solubility (in grams per
1.00×10^2mL of solution) of magnesium hydroxide in a
solution buffered at pH = 12.
S1 = _________________ g/(1.00×10^2mL)
b) Calculate the solubility (in grams per
1.00×10^2mL of solution) of magnesium hydroxide in
pure water.
S = __________________ g/(1.00×10^2mL)
c) How does the solubility of Mg(OH)2 in a buffered solution
compare to the solubility of Mg(OH)2 in pure water?
S1/S = ________________
TIA.
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