will a precipitate form when 650 ml of 0.008 K2So4 is added to 175 ml of AgNo3 Ksp of Ag2So4=1.5*10^-5
Can any one tell me how to do it >? please
If Qsp > Ksp, a ppt will form. So what is Qsp?
You are mixing two solutions. That changes the concentrations of both. To what? You are diluting 0.008 M K2SO4 from 650 mL to (650+ 175) = 825 mL.
So final (K2SO4) = (SO4) = 0.008 x (650/825) = ?
(Ag2SO4) = ? You don't know since you don't know how much AgNO3 is in the initial solution.
To determine if a precipitate will form when 650 mL of 0.008 M K2SO4 is added to 175 mL of AgNO3, we need to compare the ion concentrations with the solubility product constant (Ksp) of Ag2SO4. Here's how you can calculate it step by step:
1. Start by writing the balanced equation for the reaction:
2AgNO3 + K2SO4 -> Ag2SO4 + 2KNO3
2. Determine the initial concentrations of the ions in the solution:
- For K2SO4:
- The concentration of K+ ion is twice the molar concentration of the K2SO4 because there are 2 K+ ions in each K2SO4 molecule.
- Therefore, the initial concentration of K+ is 0.008 M x 2 = 0.016 M
- The concentration of SO4²- ion is equal to the molar concentration of the K2SO4.
- Therefore, the initial concentration of SO4²- is 0.008 M.
- For AgNO3:
- The concentration of Ag+ ion is equal to the molar concentration of AgNO3 because there is 1 Ag+ ion in each AgNO3 molecule.
- Therefore, the initial concentration of Ag+ is 175 mL (given) converted to liters = 0.175 L, multiplied by the molarity of AgNO3 (which is usually not given in the question).
3. Calculate the final concentration of the ions once the reaction occurs:
- Since AgNO3 is a soluble ionic compound, it dissociates completely in water. So the final concentration of Ag+ is the same as the initial concentration of Ag+.
- Since K2SO4 is also a soluble ionic compound, it dissociates completely in water. So the final concentrations of K+ and SO4²- are the same as their initial concentrations.
4. Calculate the ion product (IP), which is the product of the ion concentrations in the solution:
- IP = [Ag+]^2 * [SO4²-]
5. Compare the ion product (IP) with the solubility product constant (Ksp). If IP > Ksp, a precipitate will form. If IP < Ksp, no precipitate will form.
So, to answer your question, you need to calculate the ion concentrations and then compare the ion product with the solubility product constant (Ksp) of Ag2SO4 to determine if a precipitate will form.