What happens when equal volumes of 4x10-4 M aqueous solutions of calcium nitrate, Ca(NO3)2, and sodium fluoride, NaF, are combined? The Ksp of calcium fluoride, CaF2, is 4.0×10-11. Periodic Table and Datasheet O Q < K; no precipitate forms O Q > K; no precipitate forms O Q < K; a precipitate forms O Q > K; a precipitate forms

What happens when equal volumes of 4x10-4 M aqueous solutions of calcium nitrate, Ca(NO3)2, and sodium fluoride, NaF, are combined? The Ksp of calcium fluoride, CaF2, is 4.0×10-11. Periodic Table and Datasheet O Q < K; no precipitate forms O Q > K; no precipitate forms O Q < K; a precipitate forms O Q > K; a precipitate forms

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

The Kgp of Ca3 (PO4), is 1.3 x 10-26. Estimate the solubility of this salt in units of g. L-1. You must show any reaction equation(s) that you may think are necessary. If a sample of solid Ca3 (PO4)2 is stirred into exactly one litre of a 0.550M solution of NazPO4, how will the solubility of the salt compare with the answer that you have obtained in question 2.1? Explain you answer in a short sentence.
What happens when equal volumes of 2x10-4 M aqueous solutions of calcium nitrate, Ca(NO3)2, and sodium fluoride, NaF2, are combined? The Kgp of calcium fluoride, CaF2, is 4.0x10-11. K; no precipitate forms K; a precipitate forms
Will a precipitate (ppt) form when 300.0 mL of 5.0 × 10-M AGNO, are added to 300.0 mL of 2.5 x 10- M NaBr? Answer yes or no, and identify the precipitate if there is one. Ken(AgBr) = 5.0 x-10-13 no, a precipitate will not form. O yes, the ppt is NaNO3(s). O yes, the ppt is AgBr(s). O yes, the ppt is NaBr(s). O yes, the ppt is AgNO3(s).
Calcium sulfate, CaSO4, has a Ksp value of 7.10 × 10-5. What happens when calcium and sulfate solutions are mixed to give 2.00 x 10-3 MCA²+ and 3.00 x 10–²MSO4?-? A precipitate forms because Q > Ksp . A precipitate forms because Q Ksp. O No precipitate forms because Q < Ksp.
Will a precipitate (ppt) form when 300.0 mL of 5.0 x 10 °M AgNO3 are added to 300.0 mL of 2.5 × 10-/M NaBr? Answer yes or no, and identify the precipitate if there is one. Ksp(AgBr) = 5.0 × 10-13 O no, a precipitate will not form. O yes, the ppt is NaNO3(s). O yes, the ppt is AgBr(s). O yes, the ppt is NaBr(s). O yes, the ppt is AgNO3(s).
The molar solubility of iron(III) sulfide, Fe2S3, is 1.05×10-18 mol/L. (1) Express the solubility in units of grams per liter. g/L (2) Calculate the concentration of iron(III) ion in a saturated solution of iron(III) sulfide. mol/L
A solution contains 8.73x10-³ M potassium iodide and 9.62x10-3 M ammonium bromide. Solid lead acetate is added slowly to this mixture. What is the concentration of iodide ion when bromide ion begins to precipitate? [iodide] = M
The solubility of iron(II) hydroxide, Fe(OH)2, is 1.43×10–3 gram per liter at 25 °C 1.) A 50.0 milliliter sample of 3.00×10–3 molar FeSO4 solution is added to 50.0 milliliters of 4.00×10-6 molar NaOH solution. Does a precipitate of Fe(OH)2 form? Explain and show calculations to support your answer.
solid P6CO3 is at equilibrium with its ions ? A) The concentration of CO ions in solution is is wrong for 500 mL of saturated solution in which 1.6 x 1015. Which one of the following statements 12. The solubility product for PbCO3 at 25°C is for 500 mL of saturated solution in which is wrong PbCO3 = 267 g/mol A) The concentration of CO3 ions in solution is %3D 4x10-8 M. B) The maximum mass of P6CO3 dissolved in solu- -3 tion is 5.34 x 10° mg. C) The solubility of P6CO3 at 25°C is 4 x 10-8 mol/L. D) The total number of ions in solution is 2.4x10-16. E) The concentration of each of Pb<+ and CO, ions at 50°C is 4 x 10-8 M.
35.0 mL of 6.7 x 10-4 M Ca(NO3)2 is mixed at 25˚C with 65.0 mL of 8.4 x 10–5 M Na2CO3.Compute the initial concentrations of [Ca2+]init and [CO32-]init after mixing.Assume volumes are additive. 3. Should a precipitate form when the solutions in prelab questions #2 above are mixed?Support your answer with a calculation
6. Suppose a solution is prepared with 5.0 x10-3 M manganese ion (Mn*2) and 1.0 x x10-4 M sulfide ion (S-2). Will the manganese sulfide precipitate? The Ksp of manganese sulfide is 2.5 x10-10, and its molecular weight is 87.0 g/mol. You can assume no other reactions occur.
A solution is 0.010 M in both Br- and SO42-. A 0.250 M solution of lead (II) nitrate is slowly added to it. What is the concentration in the solution of the first ion when the second one starts to precipitate at 25 degrees Celcius? The answer should be 1.34 x 10-4 M