Complete the table below by deciding whether a precipitate forms when aqueous solutions A and B are mixed. If a precipitate will form, enter its empirical formula in the last column. Does a precipitate form when A and B empirical formula of solution A solution B precipitate are mixed? lead(II) nitrate potassium sulfate yes no potassium sulfide iron(II) chloride yes no potassium hydroxide iron(II) nitrate О yes no

Complete the table below by deciding whether a precipitate forms when aqueous solutions A and B are mixed. If a precipitate will form, enter its empirical formula in the last column. Does a precipitate form when A and B empirical formula of solution A solution B precipitate are mixed? lead(II) nitrate potassium sulfate yes no potassium sulfide iron(II) chloride yes no potassium hydroxide iron(II) nitrate О yes no

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter11: Solutions

Section: Chapter Questions

Problem 39P

See similar textbooks

Similar questions

The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each. (a) BaSiF6, 0.026 g/100 mL (contains SiF62- ions) (b) Ce(IO3)4, 1.5102 g/100 mL (c) Gd2(SO4)3, 3.98 g/100 mL (d) (NH4)2PtBr6, 0.59 g/100 mL (contains PtBr62- ions)
The ideal product of gravimetric analysis called precipitate should portray some specific properties. Which among the following is a property of a good precipitate and why?
You choose to investigate some of the solubility guidelinesfor two ions , the chromate ion(CrO4)-2 and the oxalate ion (C2O4) - 2. You are given 0.01 Msolutions (A, B, C, D) of four water-soluble salts: When these solutions are mixed, the following observationsare made as given in table: (a) Write a net ionic equation for the reaction that occurs ineach of the experiments. (b) Identify the precipitate formed,if any, in each of the experiments.
In the following table, predict the identity of any precipitates formed when aqueous solutions at theintersection of each row and column are mixed. If no precipitate occurs where indicated, write “NR.” NaI K2CO3 LiOH H2SO4 PbC2H3O2 Mg(NO3)2 AgClO4 CaCl2
If Sn3(PO4)2 solution is to be subjected to argentometric titration, a) Write the balanced titration reaction. (products are Ag3PO4(s),, other ions are spectator ions b) Write the stoichiometric relationship (fundamental eqn) between the titrant (AgNO3) and the titrand (Sn3(PO4)2. c) Is this a feasible titration technique? Why?
The purity of a pharmaceutical preparation of sulfanildamide (C6H4N2O2S), is prolonged oxidizing the sulfur in the sample to SO2 and bubbling this SO2 through a solution of H2O2 which converts it to H2SO4. The acid is titrated with a standard solution of NaOH (0.1251 M) until the end point with bromothymol blue, which changes color when both protons of the acid sulfuric have been neutralized. Calculate the purity of the preparation in % by weight given that a sample of 0.5136 g required 50.00 mL of the NaOH solution
A dietary iron supplement consist of tablets containing the metal in the form of ferrous ions (Fe2+). Themetal content of these tablets can be determined by dissolving a weighed amount of tablet(s) in dilutesulphuric acid solution and titrating an aliquot of this solution with a standard potassium permanganatesolution as follows: One of the tablets is finely ground and the resulting powder has a mass of 0.4500 g. Distilled water and some sulphuric acid is added until the sample is dissolved. This solution istransferred to a 250.00 mL volumetric flask and made up to the mark. A 25.00 mL portion of this solution is pipetted into a conical flask, and titrated with a 0.0200 M KMnO4solution. The endpoint of the titration is determined when the colourless solution in the conical flask turns abright pink due to the presence of excess permanganate ions. The average titration value is 6.23 mL of the KMnO4 solution. 2KMNO4+8H2SO4+10FeSO4= K2SO4 +2MnSO4 +8H20 +5Fe2(SO4)3 1.Determine the…
You are presented with a white solid and told that due tocareless labeling it is not clear if the substance is bariumchloride, lead chloride, or zinc chloride. When you transferthe solid to a beaker and add water, the solid dissolves to givea clear solution. Next a Na2SO4(aq) solution is added anda white precipitate forms. What is the identity of the unknownwhite solid?
Recommend a specific cation for the quantitative precipitation of carbonate ion andjustify your recommendations.
Gravimetric Analysis. Please include complete solution, thank you. In the gravimetric determination of sulfate in a 0.2841 g sample of pure Na2SO4, a BaSO4 precipitate weighing 0.4604 g was obtained. The weight of the precipitate was smaller than the theoretical one, since some BaSO4 was converted to BaS during the heating process. Calculate the percent of BaS in the precipitate and percent error of the analysis.
A 185 mL sample of 1.20 M Pb(NO₃)₂ is mixed with 61.5 mL of 1.50 M NaCl, and the PbCl₂ precipitate is filtered from the solution. Then 200 mL of 3.00 M NaBr is added to the remaining solution, and the PbBr₂ precipitate is also collected and dried. What is the mass of the PbBr₂ precipitate, assuming the yield in each precipitation step is 100%?
2KMnO4 (aq) +5H2C2O4 (aq) + 3H2SO4 (aq) > 10CO2 (g) + K2SO4 (aq) +2MnSO4 (aq) + 8H2O (l) 90ml of 0.0150 M KMnO4 solution is mixed with 30 ml of 0.095 M H2C2O4 solution in a medium where there is excess sulfuric acid. Assume 100% yield Calculate the concentration of the following ions or molecules in the final solution a) Mn2+ b) K+ c) MnO4- d)H2C2O4