# Chemistry

Given the two reactions

1.PbCl2 <--->Pb^2+ + 2 Cl^-,
K1= 1.82×10^−10

2. AgCl <----> Ag^+ + Cl^-,
K2 = 1.15×10−4

what is the equilibrium constant Kfinal for the following reaction?

PbCl2+ 2 Ag^+ <---> 2AgCl+ Pb^2+

This is what i have soo far:

PbCl2<--->Pb2+ + 2Cl- K1= 1.82×10^−10
AgCl <---> Ag+ + Cl- K2= 1/1.15×10^−4

(AgCl)^2(Pb)/(PbCl2)(Ag)2=
(Pb2+)(Cl)^2/(PbCl2)* (Ag)(Cl-)/(AgCl)

I dunt know what to do next because, i did :

= 1.82×10^−10 * 1/1.15×10^−4

It says When the stoichiometry of a reaction changes, the new equilibrium constant is raised to the same power. Thus, if a reaction is multiplied by 2, the equilibrium constant K is squared.

1. 👍 0
2. 👎 0
3. 👁 2,174
1. Right. First, however, check your numbers for the k values. I think they are reversed because Ksp for AgCl is about 10^-10 and Ksp for PbCl2 is about 10^-4. But if the Ks were put in the problem on purpose, then
K1 = 1.82 x 10^-10
and K2 for the reverse direction is 1/1.15 x 10^-4 and you square that [that is (1/K2)^2].
Since you added the equations to get the final equation, now you multiply the new Ks. So K for the reaction requested is K1/K2^2. Check me out on that.

1. 👍 0
2. 👎 0
2. The Values are correct i doubled checked:

But when do

1.82 x 10^-10/ (1/1.15×10^−4)^2
= 2.47*10^-18

But it says this answer is wrong

1. 👍 1
2. 👎 0
3. No.
K1 = 1.82 x 10^-10
K2 = (1/1.15 x 10^-4)^2
Then Keq for the reaction is
K1*(1/K2)^2 =
1.82 x 10^-10*(1/1.15 x 10^-4)^2 =
1.82 x 10^-10*(7.56 x 10^7) =
0.01376. Check it for math. Check it for significant figures.

1. 👍 0
2. 👎 0
4. I would round it ti 0.014 = Keq.

1. 👍 0
2. 👎 0
5. Here is the error
So K for the reaction requested is K1/K2^2. Check me out on that.
It's K1*(1/K2)^2
1.82 x 10^-10*(1/1.15 x 10^-4)^2 = 0.014

1. 👍 0
2. 👎 0
6. That's right thank you

1. 👍 0
2. 👎 0

## Similar Questions

1. ### Chemistry

When solutions of KCl and Pb(NO3)2 are mixed, a precipitate forms. Which of the following is the balanced equation for the double replacement reaction that occurs? a. KCl(aq) + Pb(NO3)2 (aq) ¨ KNO3 (aq) + PbCl2 (s) b. KNO3 (aq)

2. ### general chemistry

a 5.95 g sample of AgNO3 is reacted with excess BaCl2 according to the equation 2AgNO3 + BaCl2 yields 2AgCl + Ba(NO3)2 to give 3.17 g of AgCl. What is the percent yield of AgCl?

3. ### chemistry

Complete the two reduction half reactions for the cell shown at the right, and show the line notation for the cell by dragging labels to the correct position. (The electrode on the left is the anode, and the one on the right is

4. ### Chemistry

Classify the following reactions as precipitation reactions, oxidation-reduction reactions, or acid-base reactions. 1)2NaCl(aq)+K2H2Sb2O7(aq)==Na2H2SbO7(s)+2KCl(aq) 2)(CH3COO)2Cu(aq)+(NH4)2C2O4(aq)==CuC2O4(s)+2CH3COONH4(aq)

1. ### Chemistry

Explain why the solubility of PbF2 is pH dependent, but the solubility of PbCl2 is not. I know the solubility of PbF2 is pH dependent because the solubility would increase as the solution becomes more acidic because the F^- ion is

2. ### chemistry

Assuming that the total volume does not change after 0.200 g of KCl is added to 1.0 L of a saturated aqueous solution of AgCl, calculate the number of moles of Ag+ ion in the solution after equilibrium has been reestablished. For

3. ### Chemistry

A solution contains 0.022 M Ag and 0.033 M Pb2 . If you add Cl–, AgCl and PbCl2 will begin to precipitate. What is the concentration of Cl– required, in molarity, when A. AgCl precipitation begins? B. AgCl precipitation is

4. ### chemistry

Use the appropriate values of Ksp and Kf to find the equilibrium constant for the following reaction: PbCl2(s)+ 3OH(aq) >> Pb(OH)3 (aq) + 2Cl(aq). ksp for PbCl2 is 1.17*10^-5 kf for complex ion is 8*10^13. anyways...I know that

1. ### Chemistry

We performed a lab in class about a month ago concerning different types of equilibrium. One particular portion of the lab adding 5 mL of .3M HCl to 5 mL of .3 M Pb(NO3)2. After a precipitate finally formed, 8 mL of water was

2. ### Chemistry

What is the maximum mass(g) of KCL that can be added to 1.00L of a 0.0100 M lead(ii) chloride solution without causing any precipitation of PbCl2? Assume the additional KCl does not affect the volume of the solution. For, PbCl2,

3. ### Chemistry

Combine the Ksp and Kf equilibria for AgCl and Ag(NH3)2+ respectively and demonstrate Hess's law to determine the equilibrium constant for the dissolution of AgCl in NH3. AgCl + 2NH3 --> Ag(NH3)2 + Cl- K= (Ksp)(Kf) If there is

4. ### Chemistry

What is the molar solubility of AgCl in 1.0 M K2S2O3 if the complex ion Ag(S2O3)2^3-forms? The Ksp for AgCl is 1.8 × 10^-10 and the Kf for Ag(S2O3)2^3- is 2.9 × 10^13.