Question

11. What is the maximum volume of 8.6 × 10–5 M K2CrO4 that, added to 40.4...

11. What is the maximum volume of 8.6 × 10–5 M K2CrO4 that, added to 40.4 mL of a solution that is 5.1 × 10–5 M Ba(NO3)2 and 1.5 × 10–6 M Pb(NO3)2, will precipitate PbCrO4 but not BaCrO4? For PbCrO4, Ksp = 1.8 × 10–14, and for BaCrO4, Ksp = 1.2 × 10–10.

Homework Answers

Know the answer?
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
Similar Questions
A solution is 0.10 M Pb(NO3)2 and 0.10 M AgNO3. If solid NaCl is added to...
A solution is 0.10 M Pb(NO3)2 and 0.10 M AgNO3. If solid NaCl is added to the solution, what is [Ag+] when PbCl2 begins to precipitate? (Ksp PbCl2 = 1.7 x 10-5; AgCl = 1.8 x 10-10) A solution is 0.10 M Pb(NO3)2 and 0.10 M AgNO3. If solid NaCl is added to the solution, what is [Ag+] when PbCl2 begins to precipitate? (Ksp PbCl2 = 1.7 x 10-5; AgCl = 1.8 x 10-10)
A solution is 0.10 M Pb(NO3)2 and 0.10 M AgNO3. If solid NaCl is added to...
A solution is 0.10 M Pb(NO3)2 and 0.10 M AgNO3. If solid NaCl is added to the solution, what is [Ag+] when PbCl2 begins to precipitate? (Ksp PbCl2 = 1.7 x 10-5; AgCl = 1.8 x 10-10)
The solubility-product constant (Ksp) for MnCO3 at 25°C is 2.2 ✕ 10−11. What is the molar...
The solubility-product constant (Ksp) for MnCO3 at 25°C is 2.2 ✕ 10−11. What is the molar solubility of this substance in 0.22 M MnCl2 at 25°C? AND Calculate the Qsp or Ksp, as indicated, and determine whether a precipitate will form when each of the following mixtures is prepared. (You may assume temperature is held constant, volumes are additive, and that the initial solutions, prior to mixing, are unsaturated.) (a) 25.12 mL 1.30 ✕ 10−4M CaCl2 is mixed with 25.19...
1A.If 14.0 mL of 0.10 M Ba(NO3)2 are added to 48.0 mL of 0.17 M Na2CO3,...
1A.If 14.0 mL of 0.10 M Ba(NO3)2 are added to 48.0 mL of 0.17 M Na2CO3, will BaCO3 precipitate? A.BaCO3 will precipitate. B. BaCO3 will not precipitate.      Calculate Q. ______________ 1B The molar solubility of MnCO3 is 4.2 ? 10-6M. What is Ksp for this compound?
If 550 mL of some Pb(NO3)2 solution is mixed with 400 mL of 6.70 x 10−2...
If 550 mL of some Pb(NO3)2 solution is mixed with 400 mL of 6.70 x 10−2 M NaCl solution, what is the maximum concentration of the Pb(NO3)2 solution added if no solid PbCl2 forms? (Assume Ksp = 2.00 x 10−5 M at this temperature.) Enter the concentration in M.
If 450 ml of some Pb(NO3)2 solution is mixed with 400 ml of 1.10 x 10-2...
If 450 ml of some Pb(NO3)2 solution is mixed with 400 ml of 1.10 x 10-2 M NaCl solution, what is the maximum concentration of the Pb(NO3)2 solution added if no solid PbCl2 forms? (Assume Ksp = 2.00 x 10-5 M at this temperature.) Enter the concentration in M.
A solution contains 7.61×10-3 M sodium chromate and 1.37×10-2 M sodium chloride. Solid silver nitrate is...
A solution contains 7.61×10-3 M sodium chromate and 1.37×10-2 M sodium chloride. Solid silver nitrate is added slowly to this mixture. What is the concentration of chloride ion when chromate ion begins to precipitate? [chloride] = --------------M Table of Solubility Product Constants (Ksp at 25 oC) Type Formula Ksp Bromides PbBr2 6.3 × 10-6 AgBr 3.3 × 10-13 Carbonates BaCO3 8.1 × 10-9 CaCO3 3.8 × 10-9 CoCO3 8.0 × 10-13 CuCO3 2.5 × 10-10 FeCO3 3.5 × 10-11 PbCO3...
Select the single best answer. If 18.00 mL of 0.10 M Ba(NO3)2 are added to 40.00...
Select the single best answer. If 18.00 mL of 0.10 M Ba(NO3)2 are added to 40.00 mL of 0.10 M Na2CO3 a precipitate of BaCO3 will form.    a precipitate of NaNO3 will form.    no precipitation occurs because both possible products are soluble.    no precipitate forms because Q < Ksp.
What is the equilibrium constant for the dissolution of lead(II) chromate in Na2S2O3? For PbCrO4, Ksp...
What is the equilibrium constant for the dissolution of lead(II) chromate in Na2S2O3? For PbCrO4, Ksp = 2.0 x 10–16; for Pb(S2O3)34–, Kf = 2.2 x 106. (Use E for the power of 10) Solid AgNO3 is slowly added to a solution that contains 0.24 M of Cl− and 0.10 M of Br− (assume volume does not change). What is [Br−] (in M) when AgCl(s) starts to precipitate? Ksp of AgCl is 1.8 x 10−10. Ksp for AgBr is 5.0...
Calculate the volume, in mL, of 0.230 M Pb(NO3)2 that must be added to completely react...
Calculate the volume, in mL, of 0.230 M Pb(NO3)2 that must be added to completely react with 34.8 mL of 0.417 M NaCl. Pb(NO3)2 (aq) + 2NaCl (aq) -> PbCl2 (s) + 2NaNO3 (aq)
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT