In the laboratory you are given the task of separating Ag and Co2+ ions in aqueous solution.For each reagent listed below indicate if it can be used to separate the ions. If the reagent can be used to separate the ions, give the formula of the precipitate; if it cannot, type "NONE". (Omit states-of-matter from your answer.)ReagentSuitableK₂SKI???~PrecipitatechemPadXXHelpGreek??? ~chemPadXoXoK₂SO4NochemPadHelpGreekHelpXX->NONENONEGreek-

Let's approach this step-by-step:K2S (Potassium sulfide): - Ag+ forms a highly insoluble…

Answered: In the laboratory you are given the…

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...

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A solution of sodium hydroxide is standardized against potassium hydrogen phthalate (molecular mass = 204.224 g mol-1). From the following data, calculate the molarity of the NaOH solution. The mass of the KHP is 0.7840 g. Before the titration the buret reading was 0.8400 mL and afterwards it was 39.20 mL. A 85.12 mL sample of a solution of sulfuric acid, H2SO4, is neutralized by 59.82 mL of the NaOH solution from the problem above. Calculate the molarity of the sulfuric acid solution.
4.)
A solution contains 1.19×102 M ammonium carbonate and 1.39x102 M sodium sulfide. Solid nickel(II) nitrate is added slowly to this mixture. What is the concentration of sulfide ion when carbonate ion begins to precipitate? [sulfide] =| M
Suppose you are asked to determine the identity of a white solid. When you add water to the white solid, it dissolves and forms a clear solution. When you add a solution of Na, SO,, a white precipitate forms. Add Add H,O Na,SO, Determine the identity of the original solid. O PBCI, O MgCl, O ZNCI, O CaCl,
part b
6. The K, for the salt FeCO, is 3.07 x 10. A student mixes 500. mL of 8.2 x 10 M Fe(NO,), with 500. mL of 8.2 x 10 M Na,CO,. Calculate the molar concentrations of Fe²"c) and CO;²aq) in the 1.00 L of solution. a. b. Does a precipitate occur when the solutions are mixed, or does the solution stay clear? Explain
Copper(I) has both a chloride precipitate form and a complex form with cyanide in aqueous solutions. If the Ksp for CuCl(s) is 1.2 X 106 and the Kf for Cu(CN)2 (aq) is 1.6 X 1016, what would be the molar solubility of CuCl(s) in a solution that has a concentration of 0.271 M CN? Round your final answer to three decimal places.
Which of the following will occur when an aqueous solution of KBr is mixed with an aqueous solution of AGNO3? No precipitate will form. OA Aprecipitate of KNO3 will form. OB Oc A precipitate of AgBr will form. OD A precipitate of AgNo3 will form. DE Bright yellow precipitate will form.
Ammonium sulfate is added to an unknown mixture of ions. A precipitate forms. The solution is centrifuged, and the remaining solutions is decanted. Ammonium oxalate is then added to the solution and a precipitate forms. The solution is centrifuged, and the remaining solution is decanted. Sodium monohydrogen phosphate and sodium hydroxide are added to the decanted solution, and a precipitate forms. The precipitate is centrifuged and decanted. The solid is dissolved in acid, magnesium indicator is added, then sodium hydroxide is added until the solution turns cloudy blue, which settles when centrifuged. Sodium hydroxide is added to a fresh sample of the unknown. A damp piece of litmus paper over the opening of the test tube remains red. Select the ions present. Question 3 options: Ba2+ Ca2+ Mg2+ NH41+

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