A chemist in a quality control unit in a company works on silver halide ores. There were three samples A, B, and C. The solubility test is one of the simplest tests to distinguish between the silver halide samples, where concentrated NHOH, is used as the investigating solvent. It was found that sample A did not dissolve, sample B slowly dissolved, and sample C dissolved immediately. What are the chemical formulas of these samples? a) The chemical formulas of A, B, and C are AgCI, AgI, and AgBr respectively. b) The chemical formulas of A, B, and C are AgBr, Agl, and AgCl respectively. c) The chemical formulas of A, B, and C are Agl AgBr, and AgCl respectively. d) The chemical formulas of A, B, and C are AgCl, AgBr, and Agl respectively.

A chemist in a quality control unit in a company works on silver halide ores. There were three samples A, B, and C. The solubility test is one of the simplest tests to distinguish between the silver halide samples, where concentrated NHOH, is used as the investigating solvent. It was found that sample A did not dissolve, sample B slowly dissolved, and sample C dissolved immediately. What are the chemical formulas of these samples? a) The chemical formulas of A, B, and C are AgCI, AgI, and AgBr respectively. b) The chemical formulas of A, B, and C are AgBr, Agl, and AgCl respectively. c) The chemical formulas of A, B, and C are Agl AgBr, and AgCl respectively. d) The chemical formulas of A, B, and C are AgCl, AgBr, and Agl respectively.

Chemistry

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ISBN:9781133611097

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Chapter4: Types Of Chemical Reactions And Solution Stoichiometry

Section: Chapter Questions

Problem 123CP: In most of its ionic compounds, cobalt is either Co(II) or Co(III). One such compound, containing...

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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?
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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A student weighs out a 4.80-g sample of aluminum bromide, transfers it to a 100-mL volumetric flask, adds enough water to dissolve it, and then adds water to the 100-mL mark. What is the molarity of aluminum bromide in the resulting solution?
42. a. Fill in the following table as if it is a well plate and you are mixing two aqueous compounds at a time to see if a precipitate forms. If a precipitate is expected to form, indicate that by writing the correct formula for the precipitate in the corresponding box in the table. If no precipitate is expected to form, write “NO” in the box. CaCI2 Pb(NO3)2 (NH4)3PO4 Na2CO3 AgNO3 K2SO4 b. How do you prepare 300.0 mL of a 0.250 M CaCl2 solution using an available 2(X) M solution? Support your answer with calculations, but also make sure you describe how to prepare the solution.
What is the solid that precipitates, and how much of it forms, when an excess of sodium chloride solution is mixed with 10.0 mL of a 2.10 M silver nitrate solution?
In most of its ionic compounds, cobalt is either Co(II) or Co(III). One such compound, containing chloride ion and waters of hydration, was analyzed, and the following results were obtained. A 0.256-g sample of the compound was dissolved in water, and excess silver nitrate was added. The silver chloride was filtered, dried, and weighed, and it bad a mass of 0.308 g. A second sample of 0.416 g of the compound was dissolved in water, and an excess of sodium hydroxide was added. The hydroxide salt was filtered and heated in a flame, forming cobalt(III) oxide. The mass of cobalt(III) oxide formed was 0.145 g. a. What is the percent composition, by mass, of the compound? b. Assuming the compound contains one cobalt ion per formula unit, what is the formula? c. Write balanced equations for the three reactions described.
Using the general solubility rules discussed in Chapter 7, give the formulas of live substances that would be expected to be readily soluble in water and five substances that would be expected to not be very soluble in water. For each of the substances you choose, indicate the specific solubility rule you applied to make your prediction.
A 2.5624-g sample of a pure solid alkali metal chloride is dissolved in water and treated with excess silver nitrate. The resulting precipitate, filtered and dried, weighs 3.03707 g. What was the percent by mass of chloride ion in the original compound? What is the identity of the salt?
A 1.345-g sample of a compound of barium and oxygen was dissolved in hydrochloric acid to give a solution of barium ion, which was then precipitated with an excess of potassium chromate to give 2.012 g of barium chromate, BaCrO4. What is the formula of the compound?
An aqueous sample is known to contain either Mg2+ or Ba2+ ions. Treatment of the sample with Na2CO3 produces a precipitate, but treatment with ammonium sulfate does not. Use the solubility rules (see Table 4.1) to determine which cation is present.
In each of the following cases, does a precipitation reaction occur when solutions of the two water-soluble reactants are mixed? Give the formula of any precipitate that forms, and write a balanced chemical equation for the precipitation reactions that occur. (a) sodium carbonate and copper(11) chloride (b) potassium carbonate and sodium nitrate (c) nickel(11) chloride and potassium hydroxide

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