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
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970
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Table of contents
- Ch.1 - Introduction: Matter, Energy, and Measurement111
- Ch.2 - Atoms, Molecules, and Ions166
- Ch.3 - Chemical Reactions and Reaction Stoichiometry138
- Ch.4 - Reactions in Aqueous Solution127
- Ch.5 - Thermochemistry104
- Ch.6 - Electronic Structure of Atoms109
- Ch.7 - Periodic Properties of the Elements107
- Ch.8 - Basic Concepts of Chemical Bonding102
- Ch.9 - Molecular Geometry and Bonding Theories120
- Ch.10 - Gases122
- Ch.11 - Liquids and Intermolecular Forces79
- Ch.12 - Solids and Modern Materials102
- Ch.13 - Properties of Solutions99
- Ch.14 - Chemical Kinetics153
- Ch.15 - Chemical Equilibrium83
- Ch.16 - Acid-Base Equilibria109
- Ch.17 - Additional Aspects of Aqueous Equilibria117
- Ch.18 - Chemistry of the Environment60
- Ch.19 - Chemical Thermodynamics109
- Ch.20 - Electrochemistry113
- Ch.21 - Nuclear Chemistry79
- Ch.22 - Chemistry of the Nonmetals52
- Ch.23 - Transition Metals and Coordination Chemistry57
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry7
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Not 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
A 1.248-g sample of limestone rock is pulverized and then treated with 30.00 mL of 1.035 M HCl solution. The excess acid then requires 11.56 mL of 1.010 M NaOH for neutralization. Calculate the percentage by mass of calcium carbonate in the rock, assuming that it is the only substance reacting with the HCl solution.
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