INTRO CHEMISTRY PACKAGE MOTT COMM COLLE
2018th Edition
ISBN: 9781323763605
Author: Tro
Publisher: PEARSON
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Textbook Question
Chapter 7, Problem 15E
Is the precipitate in a precipitation reaction always a compound that is soluble or insoluble? Explain.
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Check out a sample textbook solutionChapter 7 Solutions
INTRO CHEMISTRY PACKAGE MOTT COMM COLLE
Ch. 7 - Which process is a chemical reaction? a. Gasoline...Ch. 7 - How many oxygen atoms are on the reactant side of...Ch. 7 - Q3. What is the coefficient for hydrogen in the...Ch. 7 - Q4. Determine the correct set of coefficients to...Ch. 7 - Which compound is soluble in water? a. Fe(OH)2 b....Ch. 7 - Name the precipitate that forms (if any) when...Ch. 7 - Q7. Which set of reactants forms a solid...Ch. 7 - Q8. What is the net ionic equation for the...Ch. 7 - Q9. Complete the equation:
a.
b.
c.
d. No...Ch. 7 - Prob. 10SAQ
Ch. 7 - What are the products of the balanced equation for...Ch. 7 - Q12. Precipitation reactions are best classified...Ch. 7 - 1. What is a chemical reaction? List some...Ch. 7 - If you could observe atoms and molecules with the...Ch. 7 - 3. What are the main indications that a chemical...Ch. 7 - What is a chemical equation? Provide an example...Ch. 7 - Prob. 5ECh. 7 - To balance a chemical equation, adjust the...Ch. 7 - 7. Is the chemical equation balanced? Why or why...Ch. 7 - 8. What is an aqueous solution? List two...Ch. 7 - 9. What does it mean if a compound is referred to...Ch. 7 - Explain what happens to an ionic substance when it...Ch. 7 - Do polyatomic ions dissociate when they dissolve...Ch. 7 - What is a strong electrolyte solution?Ch. 7 - 13. What are the solubility rules, and how are...Ch. 7 - What is a precipitation reaction? Provide an...Ch. 7 - 15. Is the precipitate in a precipitation reaction...Ch. 7 - 16. Describe the difference between a molecular...Ch. 7 - What is an acid-base reaction? List an example and...Ch. 7 - Prob. 18ECh. 7 - What is a gas evolution reaction? Give an example.Ch. 7 - What is a redox reaction? Give an example.Ch. 7 - Prob. 21ECh. 7 - Prob. 22ECh. 7 - 23. Explain the difference between a synthesis...Ch. 7 - 24. Explain the difference between a...Ch. 7 - Which observation is consistent with a chemical...Ch. 7 - Which observation is consistent with a chemical...Ch. 7 - Vinegar forms bubbles when it is poured into the...Ch. 7 - When a chemical drain opener is added to a clogged...Ch. 7 - 29. When a commercial hair bleaching mixture is...Ch. 7 - When water is boiled in a pot, it bubbles. Has a...Ch. 7 - For each chemical equation (which may or may not...Ch. 7 - For each chemical equation (which may or may not...Ch. 7 - 33. Consider the unbalanced chemical equation.
A...Ch. 7 - Consider the unbalanced chemical equation....Ch. 7 - Prob. 35ECh. 7 - Write a balanced chemical equation for each...Ch. 7 - Write a balanced chemical equation for each...Ch. 7 - Write a balanced chemical equation for each...Ch. 7 - 39. When solid sodium is added to liquid water, it...Ch. 7 - When iron rusts, solid iron reacts with gaseous...Ch. 7 - 41. Sulfuric acid in acid rain forms when gaseous...Ch. 7 - Nitric acid in acid rain forms when gaseous...Ch. 7 - Prob. 43ECh. 7 - Prob. 44ECh. 7 - 45. Write a balance chemical equation for the...Ch. 7 - Write a balanced chemical equation for the...Ch. 7 - 47. Balance each chemical equation.
a.
b.
c.
d....Ch. 7 - Balance each chemical equation. a....Ch. 7 - 49. Balance each chemical equation.
a.
b.
c.
d....Ch. 7 - Balance each chemical equation. a....Ch. 7 - 51. Is each chemical equation correctly balanced?...Ch. 7 - Prob. 52ECh. 7 - Prob. 53ECh. 7 - Propane camping stoves produce heat by the...Ch. 7 - 55. Catalytic converters work to remove nitrogen...Ch. 7 - Prob. 56ECh. 7 - 57. Is each compound soluble or insoluble? For the...Ch. 7 - 58. Is each compound soluble or insoluble? For the...Ch. 7 - 59. Pair each cation on the left with an anion on...Ch. 7 - Pair each cation on the left with an anion on the...Ch. 7 - 61. Move any misplaced compounds to the correct...Ch. 7 - Prob. 62ECh. 7 - Complete and balance each equation. If no reaction...Ch. 7 - Complete and balance each equation. If no reaction...Ch. 7 - Write a molecular equation for the precipitation...Ch. 7 - Write a molecular equation for the precipitation...Ch. 7 - Correct any incorrect equations. If no reaction...Ch. 7 - 68. Correct any incorrect equations. If no...Ch. 7 - 69. Identify the spectator ions in the complete...Ch. 7 - Identify the spectator ions in the complete ionic...Ch. 7 - 71. Write balanced complete ionic and net ionic...Ch. 7 - Write balanced complete ionic and net ionic...Ch. 7 - Mercury(I) ions (Hg22+) can be removed from...Ch. 7 - 74. Lead ions can be removed from solution by...Ch. 7 - Write complete ionic and net ionic equations for...Ch. 7 - 76. Write complete ionic and net ionic equations...Ch. 7 - When a hydrochloric acid solution is combined with...Ch. 7 - 78. A breaker of nitric acid is neutralized with...Ch. 7 - 79. Complete and balance each acid-base...Ch. 7 - Complete and balance each acid-base reaction. a....Ch. 7 - 81. Complete and balance each gas evolution...Ch. 7 - Complete and balance each gas evolution reaction....Ch. 7 - Which reactions are redox reactions? a....Ch. 7 - Which reactions are redox reactions? a....Ch. 7 - Prob. 85ECh. 7 - 86. Complete and balance each combustion...Ch. 7 - 87. Write a balanced chemical equation for the...Ch. 7 - Write a balanced chemical equation for the...Ch. 7 - 89. Classify each chemical reaction as a...Ch. 7 - 90. Classify each chemical reaction as a...Ch. 7 - Prob. 91ECh. 7 - 92. A main source of soulful oxide pollutants are...Ch. 7 - Predict the products of each reaction and write...Ch. 7 - Predict the products of each reaction and write...Ch. 7 - Prob. 95ECh. 7 - 96. Predict the products of each reaction and...Ch. 7 - Predict the type of reaction (if any) that occurs...Ch. 7 - Prob. 98ECh. 7 - Classify each reaction in as many ways as...Ch. 7 - Classify each reaction in as many ways as...Ch. 7 - Hard water often contains dissolved Ca2+ and Mg2+...Ch. 7 - Lakes that have been acidified by acid rain...Ch. 7 - 103. What solution can you add to each cation...Ch. 7 - Prob. 104ECh. 7 - A solution contains an unknown amount of dissolved...Ch. 7 - Prob. 106ECh. 7 - Prob. 107ECh. 7 - Prob. 108ECh. 7 - 109. Shown here are molecular views of two...Ch. 7 - Precipitation reactions often produce brilliant...Ch. 7 - Prob. 111QGWCh. 7 - Memorize the solubility rules. Without referring...Ch. 7 - Define and give an example of each of the...Ch. 7 - Water samples often contain dissolved ions such as...
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- Decide whether a precipitate will form when the following solutions are mixed. If a precipitate forms, write a net ionic equation for the reaction. (a) potassium nitrate and magnesium sulfate (b) silver nitrate and potassium carbonate (c) ammonium carbonate and cobalt(lll) chloride (d) sodium phosphate and barium hydroxide (e) barium nitrate and potassium hydroxidearrow_forwardConsider 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.arrow_forwardA 50.00-mL sample of 0.0250 M silver nitrate is mixed with 0.0400 M chromium(III) chloride. (a) What is the minimum volume of chromium(III) chloride required to completely precipitate silver chloride? (b) How many grams of silver chloride are produced from (a)?arrow_forward
- Separate samples of a solution of an unknown soluble ionic compound are treated with KCl, Na2SO4, and NaOH. A precipitate forms only when Na2SO4 is added. Which cations could be present in the unknown soluble ionic compound?arrow_forwardUsing 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.arrow_forwardA student was given a 1.6240-g sample of a mixture of sodium nitrate and sodium chloride and was asked to find the percentage of each compound in the mixture. She dissolved the sample and added a solution that contained an excess of silver nitrate. The silver ion precipitated all of the chloride ion in the mixture as silver chloride. It was filtered, dried, and weighed. Its mass was 2.056g. What was the percentage of each compound in the mixture?arrow_forward
- A 100.0-mL aliquot of 0.200 M aqueous potassium hydroxide is mixed with 100.0 mL of 0.200 M aqueous magnesium nitrate. a. Write a balanced chemical equation for any reaction that occurs. b. What precipitate forms? c. What mass of precipitate is produced? d. Calculate the concentration of each ion remaining in solution after precipitation is complete.arrow_forwardName the reagent, if any, that you would add to a solution of iron(lll) chloride to precipitate (a) iron(lll) hydroxide. (b) iron(lll) carbonate. (c) iron(lll) phosphate.arrow_forwardRelative 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)?arrow_forward
- On the basis of the general solubility rules given in Table 7.1, predict which of the following substances are likely to be appreciably soluble in water. Indicate which specific rule(s) led to your conclusion. :math>Ba(NO3)2e. KCl :math>K2SO4f. Hg2Cl2 :math>PbSO4g. (NH4)2CO3 :math>Cu(OH)2h. Cr2S3arrow_forwardAn 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.arrow_forwardAn aqueous sample is known to contain either Pb2+ or Fe3+ ions. Treatment of the sample with Na2SO4 produces a precipitate. Use the solubility rules (see Table 4.1) to determine which cation is present. TABLE 4.1 Solubility Rules for Ionic Compounds in Waterarrow_forward
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