Question
In: Chemistry
1.What is the solubility of CoCO3(s) in solution that is well-buffered at pH 4.0? (CoCO3: Ksp=1X1010,...
1.What is the solubility of CoCO3(s) in solution that is well-buffered at pH 4.0?
(CoCO3: Ksp=1X1010, H2CO3: Ka1 = 4.45 x 10-7; Ka2= 4.69 X 10-11)
Solutions
queen_honey_blossom answered 1 month agoRelated Solutions
Determine the molar solubility (S) of Ag2CO3 in a buffered solution with a pH of 3.573...
Determine the molar solubility (S) of Ag2CO3 in a buffered
solution with a pH of 3.573 using the systematic treatment of
equilibrium. Ksp(Ag2CO3) = 8.46 × 10–12; Ka1(H2CO3) = 4.45 × 10–7;
Ka2(H2CO3) = 4.69 × 10–11. Please show step as to how you got the
answer, i would really appreciate it.
Determine the molar solubility (S) of Ag2CO3 in a buffered solution with a pH of 3.573...
Determine the molar solubility (S) of Ag2CO3 in a buffered
solution with a pH of 3.573 using the systematic treatment of
equilibrium. Ksp(Ag2CO3) = 8.46 × 10–12; Ka1(H2CO3) = 4.45 × 10–7;
Ka2(H2CO3) = 4.69 × 10–11. Please show step as to how you got the
answer, i would really appreciate it.
Determine the molar solubility (S) of Ag2CO3 in a buffered solution with a pH of 3.566...
Determine the molar solubility (S) of Ag2CO3 in a buffered
solution with a pH of 3.566 using the systematic treatment of
equilibrium. Ksp(Ag2CO3) = 8.46 × 10–12; Ka1(H2CO3) = 4.45 × 10–7;
Ka2(H2CO3) = 4.69 × 10–11.
Determine the molar solubility (S) of Ag2CO3 in a buffered solution with a pH of 3.167...
Determine the molar solubility (S) of Ag2CO3 in a buffered
solution with a pH of 3.167 using the systematic treatment of
equilibrium. Ksp(Ag2CO3) = 8.46 × 10–12; Ka1(H2CO3) = 4.45 × 10–7;
Ka2(H2CO3) = 4.69 × 10–11.
Determine the molar solubility (S) of Ag2CO3 in a buffered solution with a pH of 3.255...
Determine the molar solubility (S) of Ag2CO3 in a buffered
solution with a pH of 3.255 using the systematic treatment of
equilibrium. Ksp(Ag2CO3) = 8.46 × 10–12; Ka1(H2CO3) = 4.45 × 10–7;
Ka2(H2CO3) = 4.69 × 10–11.
Show all the work please. And if you're not sure, please just
don't do it.
thank you
Determine the molar solubility (S) of Ag2CO3 in a buffered solution with a pH of 3.255...
Determine the molar solubility (S) of Ag2CO3 in a buffered
solution with a pH of 3.255 using the systematic treatment of
equilibrium. Ksp(Ag2CO3) = 8.46 × 10–12; Ka1(H2CO3) = 4.45 × 10–7;
Ka2(H2CO3) = 4.69 × 10–11. Show all the work please. And if you're
not sure, please just don't do it. thank you
What is the solubility of Mg(OH)2 in an aqueous solution buffered to a pH of 13.13?...
What is the solubility of Mg(OH)2 in an aqueous solution
buffered to a pH of 13.13? The Ksp of Mg(OH)2 is 1.8 x 10-11. Hint:
Determine the [OH-] from the pH then deal with solubility with
common ion.
Determine if adding each of the following to a saturated
Ca3(PO4)2 solution will increase,
decrease, or have little to no effect on it ssolubility.
- A.
B. C.
HCl
- ...
Compare the molar solubility of Mg(OH)2 in water and in a solution buffered at a pH...
Compare the molar solubility of Mg(OH)2 in water and in a
solution buffered at a pH of 9.3.
water M
buffered solution M
What is the solubility of AgCN(s) (Ksp = 2.2 × 10⁻¹⁶) in a solution containing 0.57...
What is the solubility of AgCN(s) (Ksp = 2.2 × 10⁻¹⁶) in a
solution containing 0.57 M H⁺? (Ka for HCN is 6.2 × 10⁻¹⁰.)
What is the solubility of MnS, in g/L, in a buffered solution that is 0.216 M...
What is the solubility of MnS, in g/L, in a buffered solution
that is 0.216 M HC2H3O2 and 0.331 M NaC2H3O2. (Hint what is the
function of the buffer solution?) Ksp = 3.0 x 10–14 for MnS.
Please clearly show your work and explain steps
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