If a solution of 20mL of 0.050M K+ is added to 80mL of 0.50M ClO4- will a precipitate form and what is the value of Qsp? For KClO4, Ksp = 1.07 x 10-2. Thank you for any help! I don't know what I am doing in this problem!

Answer 1

KClO4 --------->. K^+ + ClO4^-

Qsp=[K^+][ClO4^-]

moles=Molarity*volume (L)

Solve for moles of each

If Qsp>Ksp, precipitate forms, if less, no precipitate forms.

Answer 2

I agree with Qsp but I disagree with the calculation to determine if a ppt will form or not. It isn't mols one wants; it is molarity.
M K^+ = 0.05 x (20/100) = ?
M ClO4^- = 0.5 x (80/100) = ?
Plug those concentrations into Qsp to determine if Qsp > Ksp.

Answer 3

Forgot a step : Solve for moles AND TAKE THE TOTAL VOLUME WHICH IS 0.1L AND CALCULATE MOLARITY. Caps is just to emphasize the part I forgot, not to yell.

Answer 4

you forgor 💀