ZuoTi.Pro
Question

Thermo Chemistry

If a constant [Cl−]= 0.120 M is maintained in a solution in which the initial [Pb2+]= 7.0×10−2 M , what percentage of the Pb2+ will remain in solution after PbCl2(s) precipitates?

-Thermochem   
0 0
Add a comment Improve this question Transcribed image text
Next > < Previous
Sort answers by oldest

Homework Answers

Request Professional Answer

Request Answer!

We need at least 10 more requests to produce the answer.

0 / 10 have requested this problem solution

The more requests, the faster the answer.

Request! (Login Required)

All students who have requested the answer will be notified once they are available.
Know the answer?
Add Answer to:
Thermo Chemistry
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

Similar Homework Help Questions

  • An aqueous solution contains 0.3 M Cl'and 0.4 MF: A chemist wishes to do a fractional...

    An aqueous solution contains 0.3 M Cl'and 0.4 MF: A chemist wishes to do a fractional precipitation experiment in which he slowly adds Pb2+, which can form ppts of PbCl2(s) [K sp = 1.6 x 10-6] and PbF, (s) [Ksp = 7.1 x 10-7]. Which of the following is entirely correct? Pb2+ 0.3 M cl- 0.4M F- Cl precipitates first when [Pb2+] = 1.8 x 10-4 M. OF precipitates first when [Pb2+] = 1.0 x 10-4M. Cl precipitates first when...

  • A26. What will be observed when 15.0 mL of 0.040 M lead(II) nitrate, Pb(NO3)2, is mixed...

    A26. What will be observed when 15.0 mL of 0.040 M lead(II) nitrate, Pb(NO3)2, is mixed with 15.0 mL of 0.040 M sodium chloride? (lead chloride Ksp = 1.7 × 10–5). (A) A clear solution with no precipitate will result. (B) Solid PbCl2 will precipitate and excess Pb2+ ions will remain in solution. (C) Solid PbCl2 will precipitate and excess Cl– ions will remain in solution. (D) Solid PbCl2 will precipitate and there will be no excess ions in solution....

  • 14. A student adds HCl to an unknown solution to make (Cl) = 0.15 M. Some...

    14. A student adds HCl to an unknown solution to make (Cl) = 0.15 M. Some PbCl2 precipitates. Calculate the concentration of Pb2+ remaining in solution. The value of Kap for lead (II) chloride is 2.4 x 10-4

  • Consider the dissolution equation of lead(II) chloride. PbCl2 (s) Pb2+ (aq) + 2 C1- (aq) Suppose...

    Consider the dissolution equation of lead(II) chloride. PbCl2 (s) Pb2+ (aq) + 2 C1- (aq) Suppose you add 0.2331 g of PbCl2(s) to 50.0 mL of water. In the resulting saturated solution, you find that the concentration of Pb2+ (aq) is 0.0159 M and the concentration of Cl - (aq) is 0.0318 M. What is the value of the equilibrium constant, Ksp, for the dissolution of PbCl2? Answer:

  • A.) Given the reaction 2A + B ⇋ 4 C (all gases) concentrations at equilibrium are...

    A.) Given the reaction 2A + B ⇋ 4 C (all gases) concentrations at equilibrium are A = 0.076 M B = 0.829 M If K = 3.32, find the concentration of C and report it in M units. B.) Cu (s) + 2 Ag+ ⇋ Cu2+ (aq+) + 2 Ag(s)    K = 7.88 x 104 PbCl2 (s) ⇋ Pb2+ (aq) + 2 Cl- (aq) K = 2.4 x 10-4 AgI (s) ⇋ Ag+ (aq) + I- (aq) K =...

  • In pairs; Let’s say you add 10.0 g PbCl2 (s) to 1.0 L of water. Even...

    In pairs; Let’s say you add 10.0 g PbCl2 (s) to 1.0 L of water. Even though PbCl2 is ‘insoluble’, a fraction of the solid will dissolve. Write out the chemical equilibrium for the dissolution of PbCl2 in water. The Ksp for PbCl2 is 1.7 x 10-4. Calculate how many grams of PbCl2 will dissolve in the solution. Your lab partner claims that by adding NaCl to the solution, thus increasing [Cl-] and forcing the equilibrium back toward PbCl2 (s),...

  • 8) Calculate the following for 2.0 L solution containing [Ag+] = 0.100 M and [Pb2+] =...

    8) Calculate the following for 2.0 L solution containing [Ag+] = 0.100 M and [Pb2+] = 0.100 M. Assume no volume changes. (AgCl Ksp = 1.8 x 10-10, PbCl2 Ksp = 1.8 x 10-5). a) At what [Cl-] will each salt precipitate? b) What percent of the Ag+ has precipitated before the Pb2+ begins to precipitate? c) How much sodium chloride must be added (in grams) to precipitate a maximum AgCl before before any PbCl2 begins to precipitate?

  • Suppose a chemist starts with an aqueous buffer that contains 0.05 mol of HCN and 0.07...

    Suppose a chemist starts with an aqueous buffer that contains 0.05 mol of HCN and 0.07 mol of NaCN in a total volume of 1.00 L. What is the pH after 0.03 mol of OH is added to the buffer? a. 2.01 b. 9.46 c. 10.92 d. 10.01 e. 8.61 Calculate Eºcell for the following balanced redox reaction in acidic solution: 35024+ 2Cr(s) + 12 H+ + 3 SO2 (g) + 2Cr+3 + 6 H2O (acidic) a. +1.945 V b....

  • A Calculate the molar solubility of PbCl2 in a 0.2340 M lead(II) perchlorate, Pb(ClO )2 solution...

    A Calculate the molar solubility of PbCl2 in a 0.2340 M lead(II) perchlorate, Pb(ClO )2 solution Solubility = B. Let's say we have a beaker where a saturated solution of lead(II) chloride is in equilibrium with solid lead(II) chloride in which of these cases will the molar solubility be lowest after equilibrium is reestablished? After the addition of solid NaNO3. After the addition of 0.120 moles of Clion. Not enough information given, After letting some of the solvent evaporate None...

  • Given the two reactions PbCl2(s)⇌Pb2+(aq)+2Cl−(aq), K3 = 1.87×10−10, and AgCl(s)⇌Ag+(aq)+Cl−(aq), K4 = 1.18×10−4, what is the...

    Given the two reactions PbCl2(s)⇌Pb2+(aq)+2Cl−(aq), K3 = 1.87×10−10, and AgCl(s)⇌Ag+(aq)+Cl−(aq), K4 = 1.18×10−4, what is the equilibrium constant Kfinal for the following reaction? PbCl2(s)+2Ag+(aq)⇌2AgCl(s)+Pb2+(aq)

ADVERTISEMENT
Free Homework Help App
Download From Google Play
Scan Your Homework
to Get Instant Free Answers
Need Online Homework Help?
Ask a Question
Get Answers For Free
Most questions answered within 3 hours.
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT