Question 1 Lithium carbonate Ksp= 8.15x10^-4 4.Discuss possible sources of error that would account for a discrepancy of greater than 10%.Questions:1.If the concentration of [Li*] were doubled (say, by adding a highly soluble Li salt such as Lil), whatwould be the new concentration of [CO3] in the saturated solution?2. If the concentration of [CO3²] were doubled (say, by adding a highly soluble carbonate salt such asCs₂CO3), what would be the new concentration of [Li*] in the saturated solution? Why is the effectless than in question 1?3. Strontium sulfate has the formula SrSO4. Write an expression for its Ksp in terms of [Sr²*] and

The solubility product constant, Ksp, is the equilibrium constant for a solid substance in aqueous…

ssible sources of error that would account for a discrepancy of greater than 10%. ntration of [Li*] were doubled (say, by adding a highly soluble Li salt such as Lil), what e new concentration of [CO32] in the saturated solution? tration of [CO3²] were doubled (say, by adding a highly soluble carbonate salt such as t would be the new concentration of [Li] in the saturated solution? Why is the effect uestion 1? fate has the formula SrSO4. Write an expression for its Ksp in terms of [Sr] anc

ssible sources of error that would account for a discrepancy of greater than 10%. ntration of [Li*] were doubled (say, by adding a highly soluble Li salt such as Lil), what e new concentration of [CO32] in the saturated solution? tration of [CO3²] were doubled (say, by adding a highly soluble carbonate salt such as t would be the new concentration of [Li] in the saturated solution? Why is the effect uestion 1? fate has the formula SrSO4. Write an expression for its Ksp in terms of [Sr] anc

General Chemistry - Standalone book (MindTap Course List)

11th Edition

ISBN:9781305580343

Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Chapter19: Electrochemistry

Section: Chapter Questions

Problem 19.25QP

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Find the pH value for a solution containing 0.5 mg/L of copper ion (Cu2+) dissociated from Cu(OH)2 at equilibrium. If the pH of this solution is adjusted to 6 and 10, what would be the concentrations of copper ion in mg/L at equilibrium, respectively?
What mass in grams of Na2S2O3 is needed to dissolve 6.3 g of AgBr in a 1.0 L solution if Ksp for AgBr is 3.3×10−13 and Kf for [Ag(S2O3)2]3− is 4.7×1013? Report your answer with the correct number of significant figures.
Given two possible formulas: K[Fe(C2O4)2(H2O)2] or K3[Fe(C2O4)3], a titration of 1.356g of the compound (one of the two formulas above requires 34.5 mL of 0.108 M KMnO4. Which formula matches the compound being titrated?
2) A three gram sample containing an unknown amount of Sn2* is titrated with 37.5 mL of a 0.015 M dichromate solution. Use the results from problem one to determine the percentage of tin in the sample.
1. Calculate the molarity of a solution prepared by dissolving 11.5 g of solid NaOH in enogh water to make 1.50 L solution. 2. Give the concentration of each type of ion in the following solutions: a) 0.50 M Co(NO3)2 b) 1 M Fe(ClO4)3
。 A 0.140 mol quantity of CoCl₂ is added to a liter of 1.20 M NH3 solution. What is the concentration of Co²+ ions at equilibrium? Assume the formation constant* of Co(NH3)² + is 5.0 × 10³¹ M−6. concentration: M
Given: You weigh out exactly 0.200 g of Fe(NH4)2(SO4)2·6H2O and dissolve it in the 100.00 mL volumetric flask. You then pipette 2.00 mL of this solution into the 50.00 mL volumetric flask to prepare the stock standard tris-bipyridyl-iron(II) solution. a. Calculate the molar concentration of iron(II) in this solution in the 50.00 mL volumetric flask. (The MW of Fe(NH4)2(SO4)2·6H2O is 392.14 g/mol) (answer a given the information above)
Write the balanced NET ionic equation for the reaction when NH₄Cl and Cu(C₂H₃O₂)₂ are mixed in aqueous solution. If no reaction occurs, simply write only NR. Be sure to include the proper phases for all species within the reaction.
0.7120 g of iron ore was dissolved and the iron was reduced to Fe2+ with Jones's reagent. Fe(II) was titrated with 0.02086 M KMnO4 and consumed 39.21 mL. What is the iron content of iron ore? Report the concentration as percentage of iron (Fe%) and iron oxide (Fe2O3%).
After 1,600 grams of an aluminum sulphate sample is dissolved in water, aluminum is precipitated in the form of Al (OH) 3. Calculate the percentage of aluminum sulphate in the sample, since the Al2O3 obtained after the precipitate is filtered and heated is 0.400 grams. (Al: 27, S: 32, O: 16 g/mol)
What tests would you use to identify a solution of FeCl3?
An ore containing Fe3O4 was analyzed by dissolving a 1.5419-g sample in concentrated HCl. HNO3 was then added to oxidize any Fe2+ to Fe3+. The Fe3+ was precipitated as Fe(OH)3 by adding NH3. The precipitate was collected by filtration and was finally heated yielding 0.8525 g of Fe2O3. Report the concentration of Fe3O4 in the sample as %(w/w). (Note: the final answer is said to be 53.4%)

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General Chemistry - Standalone book (MindTap Cour…

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ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning