In which of the following solution would CaC2O4 have the highest molar solubility? Please help.
A) 0.01 M NaCl
B) 0.01 M H2C2O4
C) 0.01 M Na2C2O4
D) 0.01 M NaHC2O4
E) 0.01 M HCl
I think it is E because it is a strong acid and will completely dissociate
You're right.
To determine the solution in which CaC2O4 (calcium oxalate) would have the highest molar solubility, we need to consider the common ion effect.
The molar solubility of a substance is generally higher in a solution that does not contain a common ion. A common ion is an ion that is already present in the solution due to another compound.
Let's analyze each option:
A) 0.01 M NaCl: This solution contains Na+ ions, which are not common with CaC2O4.
B) 0.01 M H2C2O4: This solution contains C2O4^2- ions, which are common with CaC2O4. The common ion effect will reduce the molar solubility of CaC2O4.
C) 0.01 M Na2C2O4: This solution contains C2O4^2- ions, which are common with CaC2O4. The molar solubility of CaC2O4 will be reduced due to the common ion effect.
D) 0.01 M NaHC2O4: This solution contains HC2O4^- ions, which are common with CaC2O4. The molar solubility of CaC2O4 will be reduced due to the common ion effect.
E) 0.01 M HCl: This solution contains Cl- ions, which are not common with CaC2O4. The molar solubility of CaC2O4 will not be affected by the presence of Cl- ions.
Based on this analysis, the solution in which CaC2O4 would have the highest molar solubility is option E) 0.01 M HCl.
To determine which solution would have the highest molar solubility of CaC2O4, we need to consider the solubility rules and the effect of different ions on the solubility of the compound.
CaC2O4 is a sparingly soluble salt, which means it does not dissolve easily in water. To increase the solubility of CaC2O4, we want to minimize the concentration of ions that can form insoluble compounds with Ca or C2O4 ions.
Let's analyze the options:
A) 0.01 M NaCl: This solution contains Na+ and Cl- ions. Neither of these ions will react with Ca or C2O4 ions to form an insoluble compound, so they will not affect the solubility of CaC2O4.
B) 0.01 M H2C2O4: This solution contains H+ and C2O4 ions. H2C2O4 is a weak acid, which means it partially dissociates into H+ and H2C2O4- ions. However, neither H+ nor H2C2O4- ions can form insoluble compounds with Ca or C2O4 ions. Therefore, their presence will not significantly affect the solubility of CaC2O4.
C) 0.01 M Na2C2O4: This solution contains Na+ and C2O4 ions. Na+ ions will not react with Ca or C2O4 ions to form insoluble compounds. However, C2O4 ions can react with Ca2+ ions to form CaC2O4, which is insoluble. Therefore, the presence of C2O4 ions will decrease the solubility of CaC2O4.
D) 0.01 M NaHC2O4: This solution contains Na+, H+, and HC2O4 ions. Na+ ions will not affect the solubility of CaC2O4. However, H+ ions from the weak acid NaHC2O4 can react with C2O4 ions to form H2C2O4, which is weakly soluble. The increase in H2C2O4 concentration will shift the equilibrium of H2C2O4 dissociation, causing more HC2O4 ions to form. As a result, more C2O4 ions will react with Ca2+ ions, decreasing the solubility of CaC2O4.
E) 0.01 M HCl: This solution contains H+ and Cl- ions. HCl is a strong acid, which means it completely dissociates into H+ and Cl- ions. Like in solution B, neither H+ nor Cl- ions will form insoluble compounds with Ca or C2O4 ions. Therefore, their presence will not significantly affect the solubility of CaC2O4.
Based on the analysis, solution E (0.01 M HCl) would indeed have the highest molar solubility of CaC2O4 because it does not contain any ions that can react with Ca or C2O4 ions to form insoluble compounds.