The chief compound in marble is CaCO3. Marble has been widely used for statues and ornamental work on buildings, including such structures as the Taj Mahal. However, marble is readily attacked by acids via the following reaction.
CaCO3(s)+H+(aq)⇌Ca2+(aq)+HCO3−(aq)
Equilibrium constants at 25 ∘C are listed in the table below.
| Substance | Kc | Value of Kc |
| CaCO3 | Ksp | 4.5×10−9 |
| H2CO3 | Ka1 | 4.3×10−7 |
| Ka2 | 5.6×10−11 |
What is the molar solubility of marble (i.e., [Ca2+] in a saturated solution) in normal rainwater, for which pH=4.20?
In: Chemistry
This problem is a long one, but fairly conceptual in
nature.
a. For each of the following salts, write the reaction that occurs
when it dissociates in water: NaCl(s), NaCN(s), KClO2(s),
NH4NO3(s), KBr(aq), NaF(s).
b. Consider each of the reactions that you wrote above, and
identify the aqueous ions that *could* be proton donors (acids) or
proton acceptors (bases). Briefly *explain how you decided which
ions to choose*.
c. For each of the acids and bases that you identified in part b, write the chemical reaction it can undergo in aqueous solution (its reaction with water).
d. Are there any reactions that you have written above that you anticipate will occur to such an extent that the pH of the solution will be affected? As part of your answer, be sure to explain how you decided.
e. Assume that in each case, above, 0.01 mol of the salt was dissolved in enough water at 25 deg Celsius to make 1.0L of solution. In each case, what additional information would you need in order to calculate the pH? If there are cases where no additional information is required, be sure to state that as well.
f. Say you take 0.01 mol of NH4CN and dissolve it in enough water at 25 deg Celsius to make 1.0L of solution. Using chemical reactions and words, explain how you would go about determining what effect this salt will have the pH of the solution. Be sure to list any additional information you would need to arrive at an answer.
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