11 [Review Topics][References]Use the References to access important values if needed for this question.A solution contains 1.05×102M zinc acetate and 1.04x10 M nickel(II) nitrate.Solid sodium cyanide is added slowly to this mixture.A. What is the formula of the substance that precipitates first?formulaB. What is the concentration of cyanide ion when this precipitation first begins?[CN] =Submit AnswerRetry Entire Group4 more group attempts remainingNextUS 7DELL5678 Hilis Bionde.Water Wave Lace F..fw sche[Review Topics][References]Use the References to access important values if needed for this question.A solution contains 7.74x10 M potassium hydroxide and 5.83×103 M sodium carbonate.Solid copper(II) nitrate is added slowly to this mixture.A. What is the formula of the substance that precipitates first?edformula =B. What is the concentration of copper(II) ion when this precipitation first begins?[Cu²* =MSubmit AnswerRetry Entire Group4 more group attempts remaining(PreviousNextUS ODELL

Answered: Image /qna-images/answer/90b90ea5-c58f-486a-9407-b1b3679e9a14.jpg

A solution contains 1.05x102 M zinc acetate and 1.04×10 M nickel(II) nitrate. Solid sodium cyanide is added slowly to this mixture. A. What is the formula of the substance that precipitates first? formula = B. What is the concentration of cyanide ion when this precipitation first begins? [CN]= M %3D

A solution contains 1.05x102 M zinc acetate and 1.04×10 M nickel(II) nitrate. Solid sodium cyanide is added slowly to this mixture. A. What is the formula of the substance that precipitates first? formula = B. What is the concentration of cyanide ion when this precipitation first begins? [CN]= M %3D

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter10: Solutions

Section: Chapter Questions

Problem 65QAP: Twenty-five milliliters of a solution (d=1.107g/mL)containing 15.25% by mass of sulfuric acid is...

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Consider a 1.50-g mixture of magnesium nitrate and magnesium chloride. After dissolving this mixture in water, 0.500 M silver nitrate is added dropwise until precipitate formation is complete. The mass of the white precipitate formed is 0.641 g. a. Calculate the mass percent of magnesium chloride in the mixture. b. Determine the minimum volume of silver nitrate that must have been added to ensure complete formation of the precipitate.
Twenty-five milliliters of a solution (d=1.107g/mL)containing 15.25% by mass of sulfuric acid is added to 50.0 mL of 2.45 M barium chloride. (a) What is the expected precipitate? (b) How many grams of precipitate are obtained? (c) What is the chloride concentration after precipitation is complete?
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One method for determining the purity of aspirin (C9H8O4) is to hydrolyze it with NaOH solution and then to titrate the remaining NaOH. The reaction of aspirin with NaOH is as follows: A sample of aspirin with a mass of 1.427 g was boiled in 50.00 mL of 0.500 M NaOH. After the solution was cooled, it took 31.92 mL of 0.289 M HCl to titrate the excess NaOH. Calculate the purity of the aspirin. What indicator should be used for this titration? Why?
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68. Aluminum ion may be precipitated from aqueous solution by addition of hydroxide ion, forming Al(OH)3. A large excess of hydroxide ion must not be added, however, because the precipitate of Al(OH)3 will redissolve as a soluble compound containing aluminum ions and hydroxide ions begins to form. How many grains of solid NaOH should be added to 10.0 mL of 0.250 M A1Cl3 to just precipitate all the aluminum?
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Relative solubilities of salts in liquid ammonia can differsignificantly from those in water. Thus, silver bromide issoluble in ammonia, but barium bromide is not (thereverse of the situation in water). Write a balanced equation for the reaction of anammonia solution of barium nitrate with an ammoniasolution of silver bromide. Silver nitrate is soluble inliquid ammonia. What volume of a 0.50 M solution of silver bromidewill react completely with 0.215 L of a 0.076 M solutionof barium nitrate in ammonia? What mass of barium bromide will precipitate fromthe reaction in part (b)?
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In order to determine the purity of ammonium sulfate, a sample with a mass of 0.850 g is dissolved in KOH. The equation for the reaction that takes place is NH4+(aq)+OH(aq)NH3(aq)+H2OThe ammonia liberated is distilled into a flask that contains 50.00 mL of 0.250 M HCI. Not all the HCI is consumed. The excess HCI reacts with 17.3 mL of 0.120 M NaOH. What is the mass percent of (NH4)2SO4 in the sample?
A sample of solid calcium hydroxide, Ca(OH)2, is allowed to stand in water until a saturated solution is formed. A titration of 75.00 mL of this solution with 5.00102M HCl requires 36.6 mL of the acid to reach the end point. Ca(OH)2(aq)+2HCl(aq)CaCl2(aq)+2H2O(l) What is the molarity?