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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.

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Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

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BuyFindarrow_forward

Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 6, Problem 125CP
Textbook Problem
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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.

(a)

Interpretation Introduction

Interpretation: The mass percentage of compound along with balanced chemical equation and formula has to be written.

Concept introduction: The mass percent of compound is given by the calculated mass of the compound to the total mass. The mass percent of compound is given by the formula,

Masspercent(in%)=Calculatedmass(ing)Totalmass(ing)

Explanation of Solution

Given:

Record the given info

Mass of sample containing chlorine = 0.256g

Mass of sample containing cobalt    = 0.416g

Mass of silver chloride                     = 0.308g

Mass of cobalt (III) oxide                 = 0.145g

The mass of samples containing chlorine and cobalt are recorded with the masses of silver chloride and cobalt (III) oxide as shown above.

To calculate the mass percent of Cl-

Molar mass of Chlorine          = 35.45g

Molar mass of silver chloride = 143.4g

Moles of Cl- = 0.308gAgCl×35.45gAg143.4gAgCl=0.0761gCl

Therefore, the mass percent of Cl- is,

Mass percent of Cl- = 0.0761g0.256g=29.7%

Mass percent of Cl- = 29.7%

The mass percent of Cl- is calculated by plugging in the values of moles of Cl- to the total mass of sample. The moles of Cl- is calculated by plugging in the values of mass of silver chloride and molar masses of chlorine and silver chloride. The mass percent of Cl- is 29.7%

To calculate the mass percent of Co2+

Molar mass of cobalt                   = 117.86g

Molar mass of cobalt (III) oxide = 165.86g we

Moles of Co2+ = 0.145gCo2O3×117.86gCo165.86gCo2O3=0

(b)

Interpretation Introduction

Interpretation: To calculate the empirical formula of the compound

Concept introduction: The representation of simplest positive integer of a atoms in a compound is called as empirical formula.

(c)

Interpretation Introduction

Interpretation: To write the balanced equation of the precipitation reactions.

Concept introduction:

When two solutions containing soluble salts are mixed together, an insoluble salt so called precipitate is obtained and the reaction is called as precipitation reaction. These precipitation reactions help in the determination of various ions in the solution.’

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Chapter 6 Solutions

Chemistry: An Atoms First Approach
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