56 197
Assignments Done
99,1%
Successfully Done
In January 2018
Your physics homework can be a real challenge, and the due date can be really close — feel free to use our assistance and get the desired result.
Be sure that math assignments completed by our experts will be error-free and done according to your instructions specified in the submitted order form.
Our experts will gladly share their knowledge and help you with programming homework. Keep up with the world’s newest programming trends.

Answer on Other Chemistry Question for sam

Question #27035
will a precipitate occur if 250 ml of 1.5 x 10^.3 M NaCl is mixed with 250 mL of 2.0 x 10^.7 M AgNO3? Ksp of AgCl = 1.6 x 10^-10
Expert's answer
The equation for the chemical reaction is

NaCl(aq) + AgNO3(aq) = AgCl(s) + NaNO3(aq)

Ksp = [Ag+] x [Cl-] = 1.6 x 10^-10
From the equation for Ksp:
[Ag+] = [Cl-] = (1.6 x 10^-10) ^0.5 = 1.3 x 10^-5 M

The amount of NaCl is
n(NaCl) = C(NaCl) x V(L) = 1.5 x 10^-3 x 0.25 = 3.75 x 10^-4 mol

The amount of AgNO3 is
n(AgNO3) = C(AgNO3) x V(L) = 2.0 x 10^-7 x 0.25 = 5.0 x 10^-8 mol

The precipitate will occur if the product of [Ag+] and [Cl-] will be more or equal to Ksp:
[Ag+] = n(Ag+) / V(of new solution) = 5.0 x 10^-8 / (0.25 + 0.25) = 1.0 x 10^-7 M
[Cl-] = n(Cl-)/V(of new solution) = 3.75 x 10^-4 / (0.25 + 0.25) = 7.5 x 10^-4 M
[Ag+] x [Cl-] = 1.0 x 10^-7 x 7.5 x 10^-4 = 7.5 x 10^-11 it is less than Ksp, that's why the precipitate will not occur

Answer: The precipitate won't occur.

Need a fast expert's response?

Submit order

and get a quick answer at the best price

for any assignment or question with DETAILED EXPLANATIONS!

Comments

No comments. Be first!

Leave a comment

Ask Your question