Textbook Question
(a) By titration, 15.0 mL of 0.1008 M sodium hydroxide is needed to neutralize a 0.2053-g sample of a weak acid. What is the molar mass of the acid if it is monoprotic?
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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 105a
Suppose you have 3.00 g of powdered zinc metal, 3.00g of powdered silver metal and 500.0 mL of a 0.2 M copper(II) nitrate solution. (a) Which metal will react with the copper(II) nitrate solution?
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Identify the metals involved in the reaction: zinc (Zn) and silver (Ag).
Write the balanced chemical equations for the possible reactions of each metal with copper(II) nitrate (Cu(NO_3)_2).
For zinc: Zn + Cu(NO_3)_2 \(\rightarrow\) Zn(NO_3)_2 + Cu. Zinc can displace copper from the solution because it is more reactive.
For silver: Ag + Cu(NO_3)_2 \(\rightarrow\) No reaction. Silver is less reactive than copper and cannot displace it from the solution.
Conclude that zinc will react with the copper(II) nitrate solution, while silver will not.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Reactivity of Metals
The reactivity of metals is determined by their ability to lose electrons and form positive ions. In a displacement reaction, a more reactive metal can displace a less reactive metal from its compound. Understanding the reactivity series of metals helps predict which metal will react with a given solution.
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Transition Metals
Displacement Reactions
Displacement reactions occur when a more reactive element displaces a less reactive element from a compound. In this scenario, zinc and silver are compared to copper(II) ions in the solution. The metal that is higher in the reactivity series will replace the copper ions, leading to the formation of a new compound.
Molarity and Stoichiometry
Molarity is a measure of concentration, defined as moles of solute per liter of solution. In this question, the concentration of copper(II) nitrate is given, which is essential for calculating the number of moles available for reaction. Stoichiometry allows us to relate the amounts of reactants and products in a chemical reaction, helping to determine the limiting reactant.
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Related Practice
Textbook Question
Suppose you have 3.00 g of powdered zinc metal, 3.00g of powdered silver metal and 500.0 mL of a 0.2 M copper(II) nitrate solution. (b) What is the net ionic equation that describes this reaction?
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Textbook Question
Citric acid, C6H8O7, is a triprotic acid. It occurs naturally in citrus fruits like lemons and has applications in food flavouring and preservatives. A solution containing an unknown concentration of the acid is titrated with KOH. It requires 23.20 mL of 0.500 M KOH solution to titrate all three acidic protons in 100.00 mL of the citric acid solution. Write a balanced net ionic equation for the neutralization reaction.
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Textbook Question
Citric acid, C6H8O7, is a triprotic acid. It occurs naturally in citrus fruits like lemons and has applications in food flavouring and preservatives. A solution containing an unknown concentration of the acid is titrated with KOH. It requires 23.20 mL of 0.500 M KOH solution to titrate all three acidic protons in 100.00 mL of the citric acid solution. Calculate the molarity of the citric acid solution.
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Textbook Question
(b) An elemental analysis of the acid indicates that it is composed of 5.89% H, 70.6% C, and 23.5% O by mass. What is its molecular formula?
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Textbook Question
(c) If 18.65 mLof the caesium hydroxide solution was needed to neutralize a42.3 mL aliquot of the hydroiodic acid solution, what is theconcentration (molarity) of the acid?
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