Question

What concentration of Ba2+ is necessary to begin precipitating BaSO4 if the sulfate concentration is 2.2...

What concentration of Ba2+ is necessary to begin precipitating BaSO4 if the sulfate concentration is 2.2 x 10-4 M? Ksp BaSO4 = 1.1 x 10-10

0 0
Add a comment Improve this question Transcribed image text
Answer #1

saj ionic Prrae τ 4.84xg2 -l0

Add a comment
Know the answer?
Add Answer to:
What concentration of Ba2+ is necessary to begin precipitating BaSO4 if the sulfate concentration is 2.2...
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for? Ask your own homework help question. Our experts will answer your question WITHIN MINUTES for Free.
Similar Homework Help Questions
  • A solution of Na2SO4 is added dropwise to a solution that is 1.1×10−2 M in Ba2+...

    A solution of Na2SO4 is added dropwise to a solution that is 1.1×10−2 M in Ba2+ and 1.1×10−2 M in Sr2+. 1. What concentration of SO2−4 is necessary to begin precipitation? (Neglect volume changes. BaSO4:Ksp=1.1×10−10; SrSO4:Ksp=3.2×10−7.) 2. What is the concentration of SO2−4 when the second cation begins to precipitate?

  • Barium sulfate,BaSO4 , is used in medical imaging of the gastrointestinal tract because it is opaque to X rays. A bariu...

    Barium sulfate,BaSO4 , is used in medical imaging of the gastrointestinal tract because it is opaque to X rays. A barium sulfate solution, sometimes called a cocktail, is ingested by the patient, whose stomach and intestines can then be visualized via X-ray imaging. If a patient ingests 400 mL of a saturated barium sulfate solution, how much toxic Ba2+ ion has the patient consumed? The solubility product Ksp of BaSO4 is 1.1*10^-10 .

  • 15a) The Ksp of BaSO4 is 1.1 x 10-10. What is the solubility of BaSO4? a....

    15a) The Ksp of BaSO4 is 1.1 x 10-10. What is the solubility of BaSO4? a. 1.0 x 10-5 b.2.0 x 10-5 c. 4.0 x 10-5 d. 8.0 x 10-5 o o 15b) The Ksp of BaSO4 is 1.1 x 10-10. What is the solubility of BaSO4 in 0.10 M Na2SO4? a. 2.8 x 10-10 b.5.5 x 10-10 c. 1.1 x 10-9 d. 2.2 x 10-9

  • A solution of Na2SO4 is added dropwise to a solution with 0.020 M Ba2+ and 0.020...

    A solution of Na2SO4 is added dropwise to a solution with 0.020 M Ba2+ and 0.020 M Sr2+. (for BaSO4, Ksp = 1.1x10–10 and for SrSO4, Ksp = 3.2x10–7) (a) What precipitate will form first? Why? (b) What concentration of SO4 2– in the solution is necessary to begin precipitation? (neglect any volume change)

  • Solid sodium sulfate, Na2SO4, is added slowly to a solution that is 1.0 x 10-4 in...

    Solid sodium sulfate, Na2SO4, is added slowly to a solution that is 1.0 x 10-4 in both Ba2+ and Pb2+ until [SO42-] reaches 1.0 x 10^-4 M. Would either BaSO4 (Ksp = 1.1 x 10^-10) or PbSO4 (Ksp = 1.7 x 10^-8) precipitate under these conditions?

  • A solution contains 0.040 M of Na2SO4 and 0.050 M of NaIO3. Another solution of Ba2+...

    A solution contains 0.040 M of Na2SO4 and 0.050 M of NaIO3. Another solution of Ba2+ is added to the first solution.( You must accept that the original solution does not include HSO-4). a) Which of the Baryum salts precipitate firstly? b) Calculate the Ba2+ concentration while the first precipitate is occuring. c) While the more dissolved precipitate is precipitating, what is the concentration of anion which forms the less dissolved Baryum salt ? Ba(IO3) Ksp= 1.57x10-9 BaSO4 Ksp= 1.1x10-10

  • Calculate the solubility of barium sulfate. BaSO4 in units of grams per liter. Ksp (BaSO4) =...

    Calculate the solubility of barium sulfate. BaSO4 in units of grams per liter. Ksp (BaSO4) = 1.1x10-10 solubility = AL The equilibrium concentration of chloride ion in a saturated lead chloride solution is M. In the presence of excess OH, the Ar+ (aq) ion forms a hydroxide complex ion. Al(OH)4 Calculate the concentration of free Ap+ ion when 1.56x10-mol Al(CH2C00)3(s) is added to 1.00 L of solution in which [OH-] is held constant (buffered at pH 12.10). For Al(OH)4, Ke=...

  • What is the concentration of barium ions in a saturated solution of barium sulfate? Ksp(BaSO4) =...

    What is the concentration of barium ions in a saturated solution of barium sulfate? Ksp(BaSO4) = (2.321x10^-8)

  • Barium sulfate, BaSO4, is used in medical imaging of the gastrointestinal tract because it is opaque...

    Barium sulfate, BaSO4, is used in medical imaging of the gastrointestinal tract because it is opaque to X rays. A barium sulfate solution, sometimes called a cocktail, is ingested by the patient, whose stomach and intestines can then be visualized via X-ray imaging. If a patient ingests 380 mL of a saturated barium sulfate solution, how much toxic Ba2+ ion has the patient consumed? The solubility product Ksp of BaSO4 is 1.10×10−10.

  • A solution of Na2SO4 is added dropwise to a solution that is 1.1×10−2 M in Ba2+...

    A solution of Na2SO4 is added dropwise to a solution that is 1.1×10−2 M in Ba2+ and 1.1×10−2 M in Sr2+. The solubility-product constants are as follows: BaSO4:SrSO4:KspKsp==1.1×10−103.2×10−7 You may want to reference(Pages 751 - 753) Section 17.6 while completing this problem. Which cation will precipitate first? Ba2+ precipitates first. Sr2+ precipitates first. What concentration of SO42− is necessary to begin precipitation? (Neglect volume changes.) Express the molarity to two significant digits. 1.0×10−8   M   ***Need help with this answer. 1.)...

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