Question

In: Chemistry

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

Solutions

Expert Solution


Related 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
calculate the molar solubility of of Ag2CO3 in a solution that is buffered to a phone...
calculate the molar solubility of of Ag2CO3 in a solution that is buffered to a phone of 7.50
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
Ignoring activities, determine the molar solubility (S) of Zn(CN)2 in a solution with a pH =...
Ignoring activities, determine the molar solubility (S) of Zn(CN)2 in a solution with a pH = 1.34. Ksp (Zn(CN)2) = 3.0 × 10-16; Ka (HCN) = 6.2 × 10-10.
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)
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       -   ...
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT