Before tackling fractional precipitation problems, ensure proficiency with:
Can the two ions be effectively separated? Explain.
Determine the minimum concentration of the added reagent needed to start precipitating each individual ion. Use the Kspcap K sub s p end-sub expression for each potential compound.
Fractional precipitation occurs when two or more ions in a homogeneous solution are separated by adding a single reagent that forms a precipitate with both ions. Because different compounds have different solubility product constants ( Kspcap K sub s p end-sub
compounds precipitate first because they require a lower concentration of the common ion to exceed their solubility limit. High Kspcap K sub s p end-sub
Fraction of Ag⁺ remaining = (3.20 × 10⁻¹³) / 0.10 = 3.2 × 10⁻¹² (essentially all precipitated).
The principles of fractional precipitation are based on the solubility product constant (Ksp) of the ions involved. Ksp is a measure of the solubility of a salt in water. When the concentration of ions in a solution exceeds the Ksp, precipitation occurs. By controlling the concentration of ions and the conditions of the solution, it is possible to selectively precipitate certain ions while keeping others in solution.
The climax of the POGIL exercise asks students to evaluate the efficiency of the separation. When the second precipitate ( ) just begins to form, the concentration of
Before tackling fractional precipitation problems, ensure proficiency with:
Can the two ions be effectively separated? Explain.
Determine the minimum concentration of the added reagent needed to start precipitating each individual ion. Use the Kspcap K sub s p end-sub expression for each potential compound. fractional precipitation pogil answer key 2021
Fractional precipitation occurs when two or more ions in a homogeneous solution are separated by adding a single reagent that forms a precipitate with both ions. Because different compounds have different solubility product constants ( Kspcap K sub s p end-sub
compounds precipitate first because they require a lower concentration of the common ion to exceed their solubility limit. High Kspcap K sub s p end-sub Use the Kspcap K sub s p end-sub
Fraction of Ag⁺ remaining = (3.20 × 10⁻¹³) / 0.10 = 3.2 × 10⁻¹² (essentially all precipitated).
The principles of fractional precipitation are based on the solubility product constant (Ksp) of the ions involved. Ksp is a measure of the solubility of a salt in water. When the concentration of ions in a solution exceeds the Ksp, precipitation occurs. By controlling the concentration of ions and the conditions of the solution, it is possible to selectively precipitate certain ions while keeping others in solution. High Kspcap K sub s p end-sub Fraction
The climax of the POGIL exercise asks students to evaluate the efficiency of the separation. When the second precipitate ( ) just begins to form, the concentration of