For which of the following mixtures will Ag2SO4(s) precipitate?
150.0 mL of 0.10 M Na2SO4(aq) and 5.0 mL of 0.20 M AgNO3(aq)
150.0 mL of 0.10 M Na2SO4(aq) and 5.0 mL of 0.30 M AgNO3(aq)
150.0 mL of 0.10 M Na2SO4(aq) and 5.0 mL of 0.40 M AgNO3(aq)
150.0 mL of 0.10 M Na2SO4(aq) and 5.0 mL of 0.50 M AgNO3(aq)
Help?? I know I have to use Qsp equation, but I feel like I'm stil not getting the correct answer
To determine if Ag2SO4(s) will precipitate in each of the mixtures, you need to compare the reaction quotient (Qsp) to the solubility product constant (Ksp) for Ag2SO4.
Step 1: Write the balanced equation for the reaction:
AgNO3(aq) + Na2SO4(aq) → Ag2SO4(s) + 2NaNO3(aq)
Step 2: Determine the concentration of Ag+ and SO4^2- ions in each mixture.
For the first mixture (150.0 mL of 0.10 M Na2SO4(aq) and 5.0 mL of 0.20 M AgNO3(aq)):
Ag+ concentration = (5.0 mL / 155.0 mL) x 0.20 M = 0.00645 M
SO4^2- concentration = 0.10 M
For the second mixture (150.0 mL of 0.10 M Na2SO4(aq) and 5.0 mL of 0.30 M AgNO3(aq)):
Ag+ concentration = (5.0 mL / 155.0 mL) x 0.30 M = 0.00968 M
SO4^2- concentration = 0.10 M
For the third mixture (150.0 mL of 0.10 M Na2SO4(aq) and 5.0 mL of 0.40 M AgNO3(aq)):
Ag+ concentration = (5.0 mL / 155.0 mL) x 0.40 M = 0.0123 M
SO4^2- concentration = 0.10 M
For the fourth mixture (150.0 mL of 0.10 M Na2SO4(aq) and 5.0 mL of 0.50 M AgNO3(aq)):
Ag+ concentration = (5.0 mL / 155.0 mL) x 0.50 M = 0.0161 M
SO4^2- concentration = 0.10 M
Step 3: Calculate Qsp for each mixture.
Qsp = [Ag+]^2 × [SO4^2-]
For each mixture, substitute the Ag+ and SO4^2- concentrations into the Qsp equation and calculate Qsp.
Step 4: Compare Qsp with Ksp.
The Ksp value for Ag2SO4 is 1.4 × 10^-5.
If Qsp < Ksp, then Ag2SO4 will not precipitate.
If Qsp > Ksp, then Ag2SO4 will precipitate.
By comparing the calculated Qsp values for each mixture with the Ksp value, you can determine whether Ag2SO4 will precipitate or not in each case.
To determine if Ag2SO4(s) will precipitate in each mixture, you need to compare the reaction quotient (Qsp) with the solubility product constant (Ksp) for Ag2SO4.
The solubility product constant (Ksp) expresses the equilibrium constant for the dissociation of a sparingly soluble compound (in this case, Ag2SO4) into its ions in a solution.
The reaction quotient (Qsp) is similar to the equilibrium constant, but it is determined using the initial concentrations of the reactants rather than the equilibrium concentrations.
The Qsp equation for the dissociation of Ag2SO4 is:
Qsp = [Ag+]^2 * [SO4^2-]
If Qsp > Ksp, then Ag2SO4 will precipitate. If Qsp < Ksp, then Ag2SO4 will not precipitate.
Using the given mixtures, let's calculate Qsp and compare it with Ksp:
Mixture 1: 150.0 mL of 0.10 M Na2SO4(aq) and 5.0 mL of 0.20 M AgNO3(aq)
[Ag+] = (5.0 mL * 0.20 M) / (150.0 mL + 5.0 mL) = 0.00667 M
[SO4^2-] = 0.10 M
Qsp = (0.00667 M)^2 * 0.10 M = 4.45 x 10^-6
Mixture 2: 150.0 mL of 0.10 M Na2SO4(aq) and 5.0 mL of 0.30 M AgNO3(aq)
[Ag+] = (5.0 mL * 0.30 M) / (150.0 mL + 5.0 mL) = 0.010 M
[SO4^2-] = 0.10 M
Qsp = (0.010 M)^2 * 0.10 M = 1.0 x 10^-5
Mixture 3: 150.0 mL of 0.10 M Na2SO4(aq) and 5.0 mL of 0.40 M AgNO3(aq)
[Ag+] = (5.0 mL * 0.40 M) / (150.0 mL + 5.0 mL) = 0.0133 M
[SO4^2-] = 0.10 M
Qsp = (0.0133 M)^2 * 0.10 M = 1.77 x 10^-5
Mixture 4: 150.0 mL of 0.10 M Na2SO4(aq) and 5.0 mL of 0.50 M AgNO3(aq)
[Ag+] = (5.0 mL * 0.50 M) / (150.0 mL + 5.0 mL) = 0.0167 M
[SO4^2-] = 0.10 M
Qsp = (0.0167 M)^2 * 0.10 M = 2.79 x 10^-5
Now, compare the calculated Qsp values with the Ksp value for Ag2SO4. If Qsp > Ksp, Ag2SO4 will precipitate.
The Ksp value for Ag2SO4 is typically given as 1.2 x 10^-5.
Comparing the Qsp values with Ksp:
Qsp (mixture 1) < Ksp --> Ag2SO4 will not precipitate.
Qsp (mixture 2) > Ksp --> Ag2SO4 will precipitate.
Qsp (mixture 3) > Ksp --> Ag2SO4 will precipitate.
Qsp (mixture 4) > Ksp --> Ag2SO4 will precipitate.
Therefore, Ag2SO4 will precipitate in mixtures 2, 3, and 4, but not in mixture 1.
Calculate (Ag^+) and (SO4^2-), substitute into Ksp expression. That is Qsp.
If Qsp > Ksp a ppt will occur. If Qsp < Ksp, no ppt will occur.
For example, a)
(SO4^2-) = 150.0 x 0.10/155.0)= 0.0968M
(Ag^+) = 5.0 x 0.2/155.0 = 0.00645M
(0.00645)^2(0.0968) = 4.03E-6 which is smaller than Ksp = 1.20E-5; therefore, no ppt of Ag2SO4 will occur.