Color of Solution Solution Solute A Na,CrO4 Yellow (NH4)2C2O4 Colorless B AgNO3 Colorless D CaCl2 Colorless Experiment Solutions Mixed Number Result A + B A + C No precipitate, yellow solution Red precipitate forms A + D Yellow precipitate forms B + C White precipitate forms B + D White precipitate forms C + D White precipitate forms 3.

Color of Solution Solution Solute A Na,CrO4 Yellow (NH4)2C2O4 Colorless B AgNO3 Colorless D CaCl2 Colorless Experiment Solutions Mixed Number Result A + B A + C No precipitate, yellow solution Red precipitate forms A + D Yellow precipitate forms B + C White precipitate forms B + D White precipitate forms C + D White precipitate forms 3.

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter15: Complex Ion And Precipitation Equilibria

Section: Chapter Questions

Problem 64QAP

See similar textbooks

Similar questions

Assuming that no equilibria other than dissolution are involved, calculate the concentration of all solute species in each of the following solutions of salts in contact with a solution containing a common ion. Show that it is not appropriate to neglect the changes in the initial concentrations of the common ions. (a) TICl(s) in 0.025 M TlNO3. (b) BaF2(s) in 0.0313 M KF. (c) MgC2O4 in 2.250 L of a solution containing 8.156 g of Mg(NO3)2. (d) Ca(OH)2(s) in an unbuffered solution initially with a pH of 12.700
A sample solution contains two unknown ions. A student did a series of tests on the solution, in the order listed below. If a precipitate formed at any stage, the mixture was filtered and further tests were done on the filtrate. The results are as follows. First test:Second test:Third test:Fourth test: solution is a pink colourNaIO3(aq) added and no precipitate formsflame colour is redNa2CO3(aq) is added and no precipitate forms Two possible ions that the solution contains are a.lithium and manganese(II) b. strontium and cobalt(II) c. strontium and manganese(II) d. lithium and cobalt(II)
The following graphs represent the behavior of BaCO3 underdifferent circumstances. In each case, the vertical axisindicates the solubility of the BaCO3 and the horizontalaxis represents the concentration of some other reagent.(a) Which graph represents what happens to the solubilityof BaCO3 as HNO3 is added? (b) Which graph representswhat happens to the BaCO3 solubility as Na2CO3 is added?(c) Which represents what happens to the BaCO3 solubilityas NaNO3 is added? [
A sample solution contains two unknown ions. A student did a series of tests on the solution, in the order listed below. If a precipitate formed at any stage, the mixture was filtered and further tests were done on the filtrate. The results are as follows. First test:Second test:Third test:Fourth test: solution is a blue-green colourNaBr(aq) is added and a precipitate formsflame colour is violetNaClO4(aq) is added and no precipitate forms Two possible ions that the solution contains are a.lead(II) and potassium b.copper(I) and cesium c.lead(II) and rubidium d.copper(I) and potassium
A solution is prepared by mixing 100.0 mL of 0.015 mol/L Mg(NO3)2 with 300 mL of 0.10 mol/L KF. Will a precipitate of MgF2 form? Ksp of MgF2 is 6.4 x 10—9 .
Give a chemical formula for the following.a) dissolves KCl but not AgClb) dissolves CuCO3 but not BaSO4c) which dissolves FeS and Ag2O at the same timed) Dissolving MgO and Ba (OH) 2 at the same time 5) Give a chemical formula for the following.a) Precipitating with both KCl and CuCl2b) Precipitating with both NaCl and Na2CO3c) Precipitating with AgNO3 but not with Cu (NO3) 2d) Precipitating with CuC12 but not with KCl What products are produced when they occur? Complete the reactions. a) MgCO3 (s) + HNO3 (aqueous) b) CuBr2 (aq) + Na2S (aq) c) Ba (s) + O2 (g) d) NaCl (aq) + Zn (NO3) 2 (aq) e) BaSO4 (s) + Na2CO3 (aqueous)
Calculate the molar solubility and solubility in g/L of lithium fluoride (LiF, 25.939 g/mol) in pure water. Ksp = 1.7 x 10-3 Calculate the molar solubility and solubility in g/L of gold(III) chloride (AuCl3, 303.33 g/mol) in pure water. Ksp = 3.2 x 10-25 Calculate the molar solubility and solubility in g/L of gold(III) chloride in a solution that is 0.010 M in MgCl2. Ksp = 3.2 x 10-25
A solution is prepared by combining 20.00ml of 0.150 molar Ba2+ and 25.00ml of 0.125 molar Cl- Using concentrations and volumes above, determine if a precipitate will form when these solutions are mixed at 25C. Provide a calculation to support your answer, keep in mind the system is not at standard state. Ba2+ (aq) -560.77 kJ/mol Delta Gfo Cl- (aq) -131.228 kJ/mol Delta Gfo BaCl2 -1296.32 kJ/mol Delta Gfo
The solubility of Ag2CrO4 (Ksp = 1.2 x 10-12) is several times greater than that of AgCl (Ksp = 1.82 x 10-10), so the red precipitate cannot form until all the chloride ions have effectively been removed from the solution. If a student uses 1 mg of K2CrO4 Aas an indicator for 100 mL of sample solution, what is the concnetrion of chloride ion in the solution when the red precipitate (Ag2CrO4) starts to form?
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
The Ksp for BaSO4 is (1.1 x 10-10) and that for BaSeO4 is (2.8 x 10-11), A 1 Molar solution of BaCl2 is added slowly to a solution that is 1.0 x 10¯4 Molar of sodium sulfate Na2SO4 and 1.0 x 10¯4 Molar of sodium selenate, Na2SeO4. What is the approximate percentage of one anion has precipitated at the point which the second anion just begins to precipitate? (Assume the addition of the BaCl2 solution does not change the overall solution volume to any significant degree.)
When 600 mL of 8.2 × 10− 6 M Ba(NO3)2 is added to 600 mL of 6.2 × 10− 7 M Na2CrO4, no precipitate is observed. Show why a precipitate does not form. You must include a calculation as part of your answer. [Ksp BaCrO4 = 1.2 × 10−10]