Final answer:
d. The concentration of solute species in solutions of salts in contact with a solution containing a common ion can be calculated by considering the common ion effect. This effect occurs when a salt is dissolved in a solution that already contains one of the ions from the salt. The concentrations of the solute species can be determined by the solubility of the salt and the concentration of the common ion. In some cases, changes in the initial concentrations of the common ions can be neglected.
Step-by-step explanation:
To calculate the concentration of solute species in solutions of salts in contact with a solution containing a common ion, we need to consider the common ion effect. The common ion effect occurs when a salt is dissolved in a solution that already contains one of the ions from the salt. This affects the solubility of the salt and the concentrations of the solute species. Let's calculate the concentration of solute species for each of the given solutions:
a) NaCl in contact with a Na+ common ion solution:
When NaCl is dissolved in a solution that already contains Na+, the sodium ion concentration increases. The chloride ion concentration is determined by the solubility of NaCl. Since NaCl is a strong electrolyte, it completely dissociates into Na+ and Cl- ions:
[Na+] = [NaCl] = 1.250 M
[Cl-] = [NaCl] = 1.250 M
The concentration of Na+ is 1.250 M, and the concentration of Cl- is also 1.250 M.
b) Ba(NO3)2 in contact with a NO3− common ion solution:
When Ba(NO3)2 is dissolved in a solution that already contains NO3−, the nitrate ion concentration increases. The barium ion concentration is determined by the solubility of Ba(NO3)2. Since Ba(NO3)2 is a strong electrolyte, it completely dissociates into Ba2+ and 2NO3- ions:
[Ba2+] = [Ba(NO3)2] = 0.0355 M
[NO3-] = 2[Ba(NO3)2] = 2 * 0.0355 M = 0.071 M
The concentration of Ba2+ is 0.0355 M, and the concentration of NO3- is 0.071 M.
c) K2CO3 in contact with a K+ common ion solution:
When K2CO3 is dissolved in a solution that already contains K+, the potassium ion concentration increases. The carbonate ion concentration is determined by the solubility of K2CO3. Since K2CO3 is a strong electrolyte, it completely dissociates into 2K+ and CO3^2- ions:
[K+] = [K2CO3] = 0.856 g / (molar mass of K2CO3) * (1 mol / 0.225 L)
[CO3^2-] = [K2CO3] = 0.856 g / (molar mass of K2CO3) * (1 mol / 0.225 L)
The concentration of K+ is determined by the given mass of K2CO3, and the concentration of CO3^2- is also determined by the given mass of K2CO3.
d) FeCl3 in contact with a Fe3+ common ion solution:
When FeCl3 is dissolved in a solution that already contains Fe3+, the iron(III) ion concentration increases. The chloride ion concentration is determined by the solubility of FeCl3. Since FeCl3 is a strong electrolyte, it completely dissociates into Fe3+ and 3Cl- ions:
[Fe3+] = [FeCl3] = ???
[Cl-] = 3[FeCl3] = ???
d. The concentration of Fe3+ is determined by the given concentration of FeCl3, and the concentration of Cl- is also determined by the given concentration of FeCl3.