Textbook Question
The accompanying photo shows the reaction between a solution of Cd(NO3)2 and one of Na2S. (b) What ions remain in solution?
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Ch.4 - Reactions in Aqueous Solution
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232
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Table of contents
- Ch.1 - Introduction: Matter, Energy, and Measurement140
- Ch.2 - Atoms, Molecules, and Ions192
- Ch.3 - Chemical Reactions and Reaction Stoichiometry172
- Ch.4 - Reactions in Aqueous Solution156
- Ch.5 - Thermochemistry151
- Ch.6 - Electronic Structure of Atoms137
- Ch.7 - Periodic Properties of the Elements127
- Ch.8 - Basic Concepts of Chemical Bonding143
- Ch.9 - Molecular Geometry and Bonding Theories167
- Ch.10 - Gases147
- Ch.11 - Liquids and Intermolecular Forces97
- Ch.12 - Solids and Modern Materials129
- Ch.13 - Properties of Solutions126
- Ch.14 - Chemical Kinetics175
- Ch.15 - Chemical Equilibrium107
- Ch.16 - Acid-Base Equilibria127
- Ch.17 - Additional Aspects of Aqueous Equilibria133
- Ch.18 - Chemistry of the Environment88
- Ch.19 - Chemical Thermodynamics140
- Ch.20 - Electrochemistry137
- Ch.21 - Nuclear Chemistry99
- Ch.22 - Chemistry of the Nonmetals66
- Ch.23 - Transition Metals and Coordination Chemistry69
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry11
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Not the one you use?Change textbook
Chapter 4, Problem 95
Antacids are often used to relieve pain and promote healing in the treatment of mild ulcers. Write balanced net ionic equations for the reactions between the aqueous HCl in the stomach and each of the following substances used in various antacids: (a) Al(OH)3(s) (b) Mg(OH)2(s) (c) MgCO3(s) (d) NaAl(CO3)(OH)2(s) (e) CaCO3(s).
Verified step by step guidance1
Identify the chemical formula of the antacid: NaAl(CO_3)(OH)_2.
Write the balanced chemical equation for the reaction between NaAl(CO_3)(OH)_2 and HCl: NaAl(CO_3)(OH)_2(s) + HCl(aq) -> products.
Determine the products of the reaction. Typically, the reaction will produce water, carbon dioxide, and a salt. Consider the decomposition of carbonate and hydroxide ions.
Write the complete ionic equation by breaking down all aqueous compounds into their ions.
Cancel out the spectator ions to write the net ionic equation, focusing on the ions that participate in the reaction.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Net Ionic Equations
Net ionic equations represent the actual chemical species that participate in a reaction, excluding spectator ions. They focus on the ions and molecules that undergo a change during the reaction, providing a clearer picture of the chemical processes involved. This is particularly useful in acid-base reactions, where the transfer of protons is the primary focus.
Acid-Base Reactions
Acid-base reactions involve the transfer of protons (H+) from an acid to a base. In the context of antacids, the antacid neutralizes stomach acid (HCl) by reacting with it to form water and a salt. Understanding the properties of acids and bases, including their strength and dissociation in water, is essential for predicting the products of these reactions.
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Solubility and Precipitation
Solubility refers to the ability of a substance to dissolve in a solvent, while precipitation occurs when a solid forms from a solution during a chemical reaction. In the case of antacids, the solubility of the compounds involved, such as sodium aluminum carbonate, affects the reaction with hydrochloric acid and the formation of products. Recognizing which compounds are soluble or insoluble helps in writing accurate net ionic equations.
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Related Practice
Textbook Question
The commercial production of nitric acid involves the following chemical reactions:
4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g)
2 NO(g) + O2(g) → 2 NO2(g)
3 NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g)
(c) How many grams of ammonia must you start with to make 1000.0 L of a 0.150 M aqueous solution of nitric acid? Assume all the reactions give 100% yield.
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Textbook Question
The commercial production of nitric acid involves the following chemical reactions:
4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g)
2 NO(g) + O2(g) → 2 NO2(g)
3 NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g)
(a) Which of these reactions are redox reactions?
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Textbook Question
The commercial production of nitric acid involves the following chemical reactions:
4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(g)
2 NO(g) + O2(g) → 2 NO2(g)
3 NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g)
(b) Identify the element undergoing oxidation and the element undergoing reduction.
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Textbook Question
Uranium hexafluoride, UF6, is processed to produce fuel for nuclear reactors and nuclear weapons. UF6 can be produced in a two-step reaction. Solid uranium (IV) oxide, UO2, is first made to react with hydrofluoric acid (HF) solution to form solid UF4 with water as a by-product. UF4 further reacts with fluorine gas to form UF6. (a) Write the balanced molecular equations for the conversion of UO2 into UF4 and the conversion of UF4 to UF6. (b) Which step is an acid-base reaction?
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