For each of the four selected groups of cations listed below, design a separation scheme and write balanced ionic equation(s) for the predicted reactions. Assume these cations are in aqueous solution and that no other cations than the ones listed are present. a) Fe3+, Co2+ and K+ b) Al3+, Ni2+ and Ba2+ c) Pb2+, Zn2+ and Ca2+

For each of the four selected groups of cations listed below, design a separation scheme and write balanced ionic equation(s) for the predicted reactions. Assume these cations are in aqueous solution and that no other cations than the ones listed are present. a) Fe3+, Co2+ and K+ b) Al3+, Ni2+ and Ba2+ c) Pb2+, Zn2+ and Ca2+

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter3: Chemical Reactions

Section: Chapter Questions

Problem 87GQ: Gas evolution was observed when a solution of Na2S was treated with acid. The gas was bubbled into a...

See similar textbooks

Similar questions

In a titration experiment, H2O2(aq) reacts with aqueous MnO4^1- (aq) as represented by the equation below. The dark purple KMnO4 solution is added from a buret to a colorless, acidified solution of H2O2(aq) in an Erlenmeyer flask. (Note: At the endpoint of the titration, the solution is a pale pink color.) Which element is being oxidized during the titration, and what is the element’s change in oxidation number? a.) Oxygen, which changes from -1 to 0 b.) Oxygen, which changes from 0 to -2 c.) Manganese, which changes from -1 to+2 d.) Manganese, which changes from +7 to +2
A second analyst was attempting to determine the percent KHP in an unknown sample, similar to that in the CEM 262 laboratory experiment 1. The analyst found the molarity of the standardized NaOH solution to be 0.1016 mol/L. Three aliquots of the unknown sample having weights of 0.8181 g, 0.9393 g, and 0.8719 g were titrated with the NaOH solution requiring 20.00 mL, 22.39 mL, and 22.14 mL, respectively. From these data, determine the average percent KHP in the unknown sample.
1. Write the balanced formula, complete ionic, and net ionic equations for one of the reactions that produced a precipitate, including phase symbols. 2. Write the balanced formula, complete ionic, and net ionic equations for the dissolution of one of the precipitates with acetic acid, including phase symbols.
You have three solutions, A, B, and C, each of which are believed to be one of thefollowing: calcium hydroxide, potassium sulfate, and sodium chloride. Combining B andC results in the formation of a precipitate, but neither solution forms a precipitate with A.Adding iron(II) nitrate to each solution only produces a precipitate with C.1. Identity each unknown.A ________________________B ________________________C ________________________2. Write complete equations, balanced with phases, for each of the following reactionsa) A + Bb) A + Cc) B + Cd) A + Fe(NO3)2e) B + Fe(NO3)2f) C + Fe(NO3)2
A 1.2516 gram sample of a mixture of CaCO3 and Na2SO4 was analyzed by dissolving the sample and completely precipitating the Ca2+ as CaC2O4. The CaC2O4 was dissolved in sulfuric acid and the resulting H2C2O4 was titrated with a standard KMnO4 solution. (a) Write the balanced equation for the titration reaction, shown unbalanced below: MnO4- + H2C2O4 + H+ ® Mn2+ + CO2 + H2O (i) Indicate which substance is the oxidizing agent and which substance is the reducing agent. (b) The titration of the H2C2O4 obtained required 35.62 milliliters of 0.1092 molar MnO4- solution. Calculate the number of moles of H2C2O4 that reacted with the MnO4- (c) Calculate the number of moles of CaCO3 in the original sample. (d) Calculate the percentage by weight of CaCO3 in the original sample.
A sample of ore is treated with concentrated nitric acid and potassium chlorate to convert all of the sulfur to sulfate (SO42-). The nitrate and chlorate are removed by treating the solution with concentrated HCl. The sulfate is precipitated with barium (Ba2+) and weighed as BaSO4. Which is the main analyte in the sample? Ba2+ SO42- ClO3- NO3-
Calcium oxalate is a sparingly soluble ionic compound composed of calcium ions (Ca2+) and oxalate ions (C2O42–). It is a main culprit in kidney stone disease due to the formation of calcium oxalate crystals in the urine. A typical value for the concentration of calcium in urine is 0.3 grams per liter. Given a Ksp value for calcium oxalate of 1.3 × 10–8, calculate the minimum concentration of oxalate ion in urine that could lead to precipitation of calcium oxalate.
The following reactions poccur in aqueous solution. Complete and balance the molecular equations using phase labels. Then write the net iconic equations. a) CaS + HBr b) MgCO3 + HNO3 c) K2SO4 + H2SO4
I am not sure what the products of the reactions should be. 1) Get two test tubes and a wooden test tube rack. Into one test tube, add about 2 mL of 6 M HCl. Place a single piece of copper metal into the other test tube. Write the appearance of each below and then pour the acid over the copper. Observe what happens and write a balanced net ionic equation on your data sheet. need help with question 1-3
Write balanced net ionic equations for all reactions in which a precipitate formed. You must show sates and charges for all ions and compounds, (aq), (s) etc. please look at the chart attached. All the boxes with writing had precipate formed. Ex. Mg+2 + CO3-2 ..etc Please provide only typed answer solution no handwritten solution needed and please do it all for instant positive rating
Describe a process to individually remove ions Ag+, Ba2+, and Be2+ from a solution. Be sure to list the compounds that you add in order, and the method of removing the precipitate. You may wish to use a flow chart.
A 57.0 mLmL sample of a 0.108 MM potassium sulfate solution is mixed with 37.0 mLmL of a 0.106 MM lead(II)(II) acetate solution and the following precipitation reaction occurs: K2SO4(aq)+Pb(C2H3O2)2(aq)→2KC2H3O2(aq)+PbSO4(s). Find the theoretical yield and percent yield.