In: Chemistry
1. Using your determined value of Ksp, calculate how many milligrams of Ag2CrO4 will dissolve in 10.0 mL of H2O.
Ksp=8.26*10-11.
2. Use your Ksp and show, by calculation, that Ag2CrO4 should precipitate when 5mL of 0.004M AgNO3 are added to 5mL of 0.0024M K2CrO4.
Ksp=8.26*10-11
Please show work on both.
Q1 Using your determined value of Ksp, calculate how many milligrams of Ag2CrO4 will dissolve in 10.0 mL of H2O. Ksp=8.26*10-11
Solution :-
Dissociation equation for the Ag2CrO4 is as follows
Ag2CrO4 ----- > 2 Ag^+ + CrO4^2-
2x x
Ksp euation is as follows
Ksp = [Ag^+]2[CrO4^2-]
Now lets calculate the molar solubility of the Ag2CrO4 using the ksp value.
8.26*10-11 = [2x]2[x]
8.26*10-11 = 4x3
8.26*10-11/4 =x3
2.07*10-11 = x3
By taking cube root of both sides we get
2.74*10-4 =x
Therefore the molar solubility if the Ag2CrO4 is 2.74*10-4 mol per liter
We have to find mass of the Ag2CrO4 in 10 ml water sample
10 ml * 1 L / 1000 ml = 0.010 L
Now lets calculate the moles of the Ag2CrO4 that are soluble in 10 ml water
Moles = molarity * volume in liter
Moles if Ag2CrO4 = 2.74*10-4 mol per L * 0.010 L
= 2.74*10-6 mol
Now lets convert the moles of Ag2CrO4 to its mass
(2.74*10-6 mol * 331.7301 g / 1 mol Ag2CrO4)* (1kg / 1000 g) =9.1*10-7 kg
Therefore mass of the Ag2CrO4 that can be soluble in 10 ml water is =9.1*10-7 kg
Q2 Use your Ksp and show, by calculation, that Ag2CrO4 should precipitate when 5mL of 0.004M AgNO3 are added to 5mL of 0.0024M K2CrO4. Ksp=8.26*10-11
Solution :-
Lets find the final concentration of the each AgNO3 and K2CrO4 after mixing the solutions
The final volume of the solution after mixing = 5 ml + 5ml = 10 ml
Final concentration of the AgNO3 = 0.004 M * 5 ml / 10 ml = 0.002 M
Final concentration of the K2CrO4 =0.0024 M * 5 ml / 10 ml = 0.0012 M
Now lets calculate the reaction quotient (Qc) and compare it with Kc
Qc= [Ag^+]2[CrO4^2-]
Lets put the concentration values in the formula.
Qc =[0.002]2[0.0012]
Qc = 4.8*10-9
Qc > Kc therefore Ag2CrO4 will precipitate out.