Concept explainers
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: 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,
Answer to Problem 137CP
The mass percentage of
Explanation of Solution
Given:
Record the given info
Mass of sample containing chlorine =
Mass of sample containing cobalt =
Mass of silver chloride =
Mass of cobalt (III) oxide =
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
Molar mass of Chlorine =
Molar mass of silver chloride =
Moles of
Therefore, the mass percent of
Mass percent of
Mass percent of
The mass percent of
To calculate the mass percent of
Molar mass of cobalt =
Molar mass of cobalt (III) oxide =
Moles of
Therefore, the mass percent of
Mass percent of
The mass percent of
To calculate the mass percent of water
Molar mass of water =
Assume that 100g of compound is,
The mass percent of hydrogen and oxygen is calculated by plugging in the molar mass of water and molar masses of hydrogen and oxygen to the total mass of the sample. The molar masses of hydrogen and oxygen were found to be
The mass percentages of
(b)
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.
Answer to Problem 137CP
The formula for the compound is
Explanation of Solution
To calculate the empirical formula of the compound
Out of 100 g of compound, there are
Dividing the moles by the smallest number,
The empirical formula of the compound becomes
The empirical formula of the compound is calculated by calculating the mole ratio of individual elements divide by the smallest number. The empirical formula of the compound is found to be
The empirical formula of the compound was calculated by using the mole ratio of individual elements divided by the smallest number. The empirical formula of the compound is found to be
(c)
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.’
Answer to Problem 137CP
This is redox reaction. Hence, an oxidizing agent is required and the oxidizing agent is
Explanation of Solution
To write the balanced equation of the precipitation reactions.
The reaction between cobalt chloride hexahydrate with base such as silver nitrate and sodium hydroxide yields precipitates of silver chloride and cobalt hydroxide with release of water and sodium chloride. The equation for this reaction can be given as,
Cobalt hydroxide oxidizes to cobalt (III) oxide and water.
Two moles of silver nitrate are required to react with cobalt chloride hexahydrate to give 2 moles of silver chloride as precipitate with side products being cobalt nitrate and water. Cobalt nitrate being water soluble remains inside the solution, thus precipitating silver chloride out of the solution.
Two moles of sodium hydroxide are required to react with cobalt chloride hexahydrate to give 2 moles of cobalt hydroxide with sodium chloride and water. Sodium chloride being soluble in water, dissociates as spectator ions thus remaining in the solution and a precipitate of cobalt hydroxide is precipitated out.
Cobalt hydroxide on heating is oxidized to cobalt (III) oxide with water.
The balanced form of these equations can be given as,
The reaction of heating cobalt hydroxide is oxidation-reduction reaction, where oxygen is used as oxidizing agent and cobalt (III) oxide is obtained.
The given reactions were found to be precipitation reaction and moles on the reactant and the product were obtained. The reaction of heating cobalt hydroxide is oxidation-reduction reaction, where oxygen is used as oxidizing agent to oxidized cobalt hydroxide to cobalt (III) oxide. The balanced equations are,
Want to see more full solutions like this?
Chapter 4 Solutions
Bundle: Chemistry, Loose-Leaf Version, 10th + OWLv2 with Student Solutions Manual, 4 terms (24 months) Printed Access Card
- 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?arrow_forwardWhat 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?arrow_forwardThe procedures and principles of qualitative analysis are coy cred in many introductory chemistry laboratory courses. In qualitative analysis, students learn to analyze mixtures of the common positive and negative ions, separating and confirming the presence of the particular ions in the mixture. One of the first steps in such an analysis is to treat the mixture with hydrochloric acid, which precipitates and removes silver ion, lead(II) ion, and mercury(I) ion from the aqueous mixture as the insoluble chloride salts. Write balanced net ionic equations for the precipitation reactions of these three cations with chloride ion.arrow_forward
- Potatoes can be peeled commercially by soaking them in a 3-M to 6-M solution of sodium hydroxide, then removing the loosened skins by spraying them with water. Does a sodium hydroxide solution have a suitable concentration if titration of 12.00 mL of the solution requires 30.6 mL of 1.65 M HCI to reach the end point?arrow_forwardhat kind of visual evidence indicates that a chemical reaction has occurred? Give an example of each type of evidence you have mentioned. Do all reactions produce visual evidence that they have taken place?arrow_forwardOn the basis of the general solubility rules given in Table 4.1, predict the identity of the precipitate that forms when the following aqueous solutions are mixed. If no precipitate forms, indicate which rules apply.arrow_forward
- If aqueous solutions of potassium sulfide and iron(III) chloride are mixed, a precipitate is formed. Write the complete and net ionic equations for this reaction, and name the precipitate.arrow_forwardArsenic acid, H3AsO4, is a poisonous acid that has been used in the treatment of wood to prevent insect damage. Arsenic acid has three acidic protons. Say you take a 25.00-mL sample of arsenic acid and prepare it for titration with NaOH by adding 25.00 mL of water. The complete neutralization of this solution requires the addition of 53.07 mL of 0.6441 M NaOH solution. Write the balanced chemical reaction for the titration, and calculate the molarity of the arsenic acid sample.arrow_forwardIn the spectroscopic analysis of many substances, a series of standard solutions of known concentration are measured to generate a calibration curve. How would you prepare standard solutions containing 10.0, 25.0, 50.0, 75.0, and 100. ppm of copper from a commercially produced 1000.0-ppm solution? Assume each solution has a final volume of 100.0 mL. (See Exercise 123 for definitions.)arrow_forward
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning
- Introductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage LearningWorld of Chemistry, 3rd editionChemistryISBN:9781133109655Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCostePublisher:Brooks / Cole / Cengage LearningGeneral Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage Learning