Hi DrBob thank tou for your help so far its really inspiring I must say:)

I have another question though:P

Use the table to predict wheter a precipiatate forms if:
25.0 mL of 0.010 mol/L silver nitrate is mixed with 25.0 mL of 0.0050 mol/L potassium chloride

My teacher says the precipitate does form but I cant figure out how to arrive at this answer:

The table is a table of Ksp Values which I cannot send since it is in Microsoft Word

Has your teacher talked about the solubility quotient? That's how this is done.

AgCl ==> Ag+ + Cl^-
Ksp = (Ag^+)(Cl^-)

Summary: Calculate the concentrations of the AgNO3 and KCl after they are mixed and see if the (Ag^+)*Cl^-) equals, is less than, or is greater than Ksp. If it is less than Ksp, no ppt forms. If it is greater than Ksp, a ppt forms. If it is the same as Ksp (exactly equal to Ksp), the solution is saturated and the addition of one more Ag or Cl ion would ppt.

What you do is calculate mols AgNO3 from M x L = 0.01 M x 0.025 L = 0.00025 mols.
Then calculate mols KCl from M x L = 0.005 M x 0.025 L = 0.000125
After mixing the two solutions, the new concentration is (just before they react, if they will react)
(AgNO3) = 0.00025 mols/0.05 L (that's 25 mL + 25 mL = 50 mL = 0.05 L
) = 0.005 M.
(KCl) = 0.000125 M/0.05 L = 0.0025 M.

Now you have the concentrations of the two solutions just before they react but after they are mixed. Just multiply and see what the quotient is and compare with Ksp.
KQ = (At^+)(Cl^-) = 0.005*0.0025 = 1.25 x 10^-5. Now compare that with Ksp. I think your table will give you something like 1.7 x 10^-10 for Ksp of AgCl; therefore, the quotient is MUCH larger than Ksp. Since Ksp can't be exceeded, then a ppt MUST form.

No problem, I can still help you without the table. To determine whether a precipitate will form when two solutions are mixed, we need to compare the product of the ion concentrations, which is given by the solubility product constant (Ksp), to the actual ion product of the solutions.

The balanced chemical equation for the reaction between silver nitrate (AgNO3) and potassium chloride (KCl) is:

AgNO3(aq) + KCl(aq) → AgCl(s) + KNO3(aq)

From this equation, we can see that the products of the reaction are silver chloride (AgCl) and potassium nitrate (KNO3).

To determine if AgCl will precipitate, we compare the Ksp of AgCl to the ion product (Q) formed by the concentrations of the reacting ions.

The Ksp expression for AgCl is: Ksp = [Ag+][Cl-]

For this reaction, we have 0.010 mol/L silver nitrate and 0.0050 mol/L potassium chloride. Since both solutions have equal volumes (25.0 mL), when they are mixed, the final volume will be 50.0 mL.

To find the concentrations of Ag+ and Cl- ions, we need to use the dilution formula:

C1V1 = C2V2

Where:
C1 is the initial concentration of the silver nitrate solution
V1 is its initial volume
C2 is the final concentration after mixing
V2 is the final volume after mixing

Applying the formula:
0.010 mol/L * 25.0 mL = C2 * 50.0 mL
C2 = (0.010 mol/L * 25.0 mL) / 50.0 mL
C2 = 0.0050 mol/L

So, the final concentration of both Ag+ and Cl- ions will be 0.0050 mol/L.

Now, substitute the concentrations into the Ksp expression for AgCl:

Ksp = [Ag+][Cl-] = (0.0050 mol/L)(0.0050 mol/L) = 2.5 x 10^-5

Since the ion product (Q) is equal to the Ksp value, AgCl will precipitate from the solution.

Therefore, the teacher is correct, and a precipitate does form when 25.0 mL of 0.010 mol/L silver nitrate is mixed with 25.0 mL of 0.0050 mol/L potassium chloride.