Question

For PbCl3−, Kform = 2.5 × 101. Use this information plus the Ksp for PbCl2 to...

For PbCl3−, Kform = 2.5 × 101. Use this information plus the Ksp for PbCl2 to calculate Kc for the following reaction: PbCl2(s) + Cl-(aq) <---> PbCl3-(aq)

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

The Kform PbCl3- = 2.5 × 101

Pb+2 + 3Cl- --> PbCl3-

Kform = [PbCl3-] / [Pb+2][Cl-]^3 ..........(1)

Pb+2 + 2Cl- = PbCl2

Ksp = [Pb+2] [Cl-]^2 .....(2)

We have to calculate

PbCl2(s) + Cl-(aq) <---> PbCl3-(aq)

Kc = [PbCl3-] / [Cl-] ..........(3)

So we have to equate expression (3) with expression 1 and 2.

Let us multiply the two

Kform X Ksp = [PbCl3-] / [Pb+2][Cl-]^3 X [Pb+2] [Cl-]^2 = [PbCl3-] / [Cl-] = Kc

Ksp = 1.6 x 10^-5

Kc = 2.5 × 101 X 1.6 x 10^-5 = 4 X 10^-4

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Write the equilibrium expression (Kc) for the following reacCon. PbCl2(s) ? Pb2+(aq) + 2Cl–(aq) Kc =...
Write the equilibrium expression (Kc) for the following reacCon. PbCl2(s) ? Pb2+(aq) + 2Cl–(aq) Kc = ______________________ b. (6 pts) At 25˚C, a certain mass of PbCl2 was dissolved in water and the equilibrium concentraCon of dissolved Pb2+ was measured to be 1.62 x 10–2 M. Calculate Kc for this process. (Hint: If 1 mole of Pb2+ dissolves, how much Cl– dissolves with it?) c. (4 pts) In ques@on 2b, the mass of solid PbCl2 added to water was not...
Calculate the molar solubility in (M) of PbCl2 (ksp=1.2x10-5 at 298K) in a) pure H2O (l)...
Calculate the molar solubility in (M) of PbCl2 (ksp=1.2x10-5 at 298K) in a) pure H2O (l) b) 0.50M NaCl (aq)
PbCl2 (s) ==== Pb2+ (aq) + 2 Cl- (aq) Record your observations for the following changes...
PbCl2 (s) ==== Pb2+ (aq) + 2 Cl- (aq) Record your observations for the following changes and explain each in term of Le Chatelier’s principle. Write net ionic equations for the reactions which occur. 1. Heating the PbCl2 mixture. 2. Addition 1.0 M Na2CO3 to the clear liquid. 3. Reaction with 1.0 M HNO3. 4. Reaction with Na2S.
At 25 C the Ksp for PbCl2 is 1.6 × 10^–5. 1.) Calculate Q for the...
At 25 C the Ksp for PbCl2 is 1.6 × 10^–5. 1.) Calculate Q for the following: 125.0 mL of 0.0300 M Pb(NO3)2 is mixed with 75.0 mL of 0.0200 M NaCl at 25 C 2.) Will a precipitate form from the above reaction?
Calculate Kc of the following reaction: CuBr(s)+Br-(aq)----> CuBr2-(aq) The solubility product constant, Ksp, for CuBr is...
Calculate Kc of the following reaction: CuBr(s)+Br-(aq)----> CuBr2-(aq) The solubility product constant, Ksp, for CuBr is 6.27× 10–9 and the overall formation constant, Kf (β2), for CuBr2– is 8.0× 105.
Reaction (i) Pb2+(aq) + 2 Cl-(aq) ⇌ PbCl2(s) If NaOH is added to reaction (i), a...
Reaction (i) Pb2+(aq) + 2 Cl-(aq) ⇌ PbCl2(s) If NaOH is added to reaction (i), a second precipitation reaction will occur: Reaction (ii) Pb2+(aq) + 2 OH-(aq) ⇌ Pb(OH)2(s) The important aspect of this is that the two reactions take place within the same container (just because we draw them separately on paper does not mean they are separate inside in the container). Thus, reaction (i) and (ii) are coupled at the molecular level by a common chemical species that...
For the reaction: PbCl2(s) ↔ Pb2+(aq)+2Cl1-(aq), what is Q* when 1.7 mL of 0.058 M lead...
For the reaction: PbCl2(s) ↔ Pb2+(aq)+2Cl1-(aq), what is Q* when 1.7 mL of 0.058 M lead nitrate is added to 16 mL of 0.025 M sodium chloride? Ksp of lead chloride is 1.6 x 10-5 M3.
If Kp=3.13x10-2 at 500 K for the reaction: Br2 (g) + Cl2 (g) <--> 2 BrCl...
If Kp=3.13x10-2 at 500 K for the reaction: Br2 (g) + Cl2 (g) <--> 2 BrCl (g) a) Calculate Kc at 500K b) What is the value of Kc for the reverse reaction at 500 K? c) Calculate the value of Kp for the following reaction at 500 K:    2Br2 (g) + 2Cl2 (g) <--> 4BrCl (g) d) Given the following two reactions and their equilibrium constants:    AgCl (s)<--> Ag+1 (aq) + Cl-1 (aq) Kc=1.8x10-10 M2    Ag+1...
At 25 degrees Celcius the Ksp for PbCl2 is 1.6 × 10–5. Calculate Q  for the following:...
At 25 degrees Celcius the Ksp for PbCl2 is 1.6 × 10–5. Calculate Q  for the following: 125.0 mL of 0.0100 M Pb(NO3)2 is mixed with 75.0 mL of 0.0200 M NaCl at 25 degrees Celcius
Calculate the value of the equilibrium constant, Kc, for the following reaction. FeS(s) + 6CN-(aq) <----->...
Calculate the value of the equilibrium constant, Kc, for the following reaction. FeS(s) + 6CN-(aq) <-----> [Fe(CN)6]4-(aq) + S2-(aq) Kc=______? The solubility product constant, Ksp, for FeS is 1.6 × 10^–19, and the formation constant, Kf, for [Fe(CN)6]^4– is 1.5 × 10^35 Kc=______
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT