3. Given the following word equations, i. translate each word equation into a balanced chemical equation, including physical states, for each reactant and product. ii. indicate the type of reaction (precipitation reaction, acid-base neutralization reac- tion, or oxidation-reduction reaction). a. Silver nitrate reacts with potassium iodide to produce silver iodide precipitate and aqueous potassium nitrate. b. Zinc metal reacts with sulfuric acid to produce aqueous zinc sulfate and hydrogen gas. c. Phosphoric acid reacts with calcium hydroxide to produce water and calcium phosphate.

3. Given the following word equations, i. translate each word equation into a balanced chemical equation, including physical states, for each reactant and product. ii. indicate the type of reaction (precipitation reaction, acid-base neutralization reac- tion, or oxidation-reduction reaction). a. Silver nitrate reacts with potassium iodide to produce silver iodide precipitate and aqueous potassium nitrate. b. Zinc metal reacts with sulfuric acid to produce aqueous zinc sulfate and hydrogen gas. c. Phosphoric acid reacts with calcium hydroxide to produce water and calcium phosphate.

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter6: Chemical Reactions: An Introduction

Section: Chapter Questions

Problem 59AP

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Aqueous hydrogen fluoride (hydrofluoric acid) is used to etch glass and to analyze minerals for their silicon content. Hydrogen fluoride will also react with sand (silicon dioxide). (a) Write an equation for the reaction of solid silicon dioxide with hydrofluoric acid to yield gaseous silicon tetrafluoride and liquid water. (b) The mineral fluorite (calcium fluoride) occurs extensively in Illinois. Solid calcium fluoride can also be prepared by the reaction of aqueous solutions of calcium chloride and sodium fluoride, yielding aqueous sodium chloride as the other product. Write complete and net ionic equations for this reaction.
On Easter Sunday, April 3, 1983, nitric acid spilled from a tank car near downtown Denver, Colorado. The spill was neutralized with sodium carbonate: 2HNO3(aq)+Na2CO3(aq)2NaNO3(aq)+H2O(l)+CO2(g) a. Calculate H for this reaction. Approximately 2.0 104 gal nitric acid was spilled. Assume that the acid was an aqueous solution containing 70.0% HNO3 by mass with a density of 1.42 glcm3. What mass of sodium carbonate was required for complete neutralization of the spill, and what quantity of heat was evolved? (Hf for NaNO3(aq) = 467 kJ/mol) b. According to The Denver Post for April 4, 1983, authorities feared that dangerous air pollution might occur during the neutralization. Considering the magnitude of H, what was their major concern?
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