Skip to main content
Ch.20 - Electrochemistry
Tro - Chemistry: A Molecular Approach 5th Edition
Tro5th EditionChemistry: A Molecular ApproachISBN: 9780134874371Not the one you use?Change textbook
All textbooksTro 5th EditionCh.20 - ElectrochemistryProblem 59
Chapter 20, Problem 59

Determine whether or not each metal dissolves in 1 M HNO3. For those metals that do dissolve, write a balanced redox reaction showing what happens when the metal dissolves. a. Cu b. Au

Verified step by step guidance
1
Identify the standard reduction potential of HNO3 and the metal involved. For HNO3, the NO3- ion is reduced to NO2, and for Cu, the Cu metal is oxidized to Cu2+.
Compare the standard reduction potentials. The metal will dissolve if its oxidation potential is higher than the reduction potential of the nitrate ion in HNO3.
Write the half-reactions for the oxidation of Cu and the reduction of NO3-. For Cu: Cu(s) → Cu2+(aq) + 2e-. For NO3-: NO3-(aq) + 2H+(aq) + e- → NO2(g) + H2O(l).
Balance the electrons in the half-reactions. Multiply the Cu oxidation reaction by 1 and the NO3- reduction reaction by 2 to balance the number of electrons transferred.
Add the balanced half-reactions together to get the overall redox reaction: 3Cu(s) + 2NO3-(aq) + 8H+(aq) → 3Cu2+(aq) + 2NO2(g) + 4H2O(l).

Verified video answer for a similar problem:

This video solution was recommended by our tutors as helpful for the problem above.
Video duration:
6m
Was this helpful?

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Redox Reactions

Redox reactions involve the transfer of electrons between substances, leading to changes in oxidation states. In these reactions, one species is oxidized (loses electrons) while another is reduced (gains electrons). Understanding redox processes is crucial for predicting how metals interact with acids, such as nitric acid (HNO3), which can act as both an oxidizing agent and a source of protons.
Recommended video:
Guided course
03:12
Identifying Redox Reactions

Metal Reactivity

The reactivity of metals is determined by their ability to lose electrons and form cations. This property is influenced by factors such as ionization energy and electronegativity. In the context of HNO3, more reactive metals will dissolve readily, while less reactive metals, like copper (Cu), may not react significantly unless specific conditions are met.
Recommended video:
Guided course
03:12
Transition Metals

Balanced Chemical Equations

A balanced chemical equation represents a chemical reaction with equal numbers of each type of atom on both sides of the equation. Balancing is essential to accurately depict the conservation of mass and charge during a reaction. For metals dissolving in acids, writing a balanced equation helps illustrate the stoichiometry of the reactants and products involved in the redox process.
Recommended video:
Guided course
01:32
Balancing Chemical Equations
Related Practice
Textbook Question

Determine whether or not each metal dissolves in 1 M HCl. For those metals that do dissolve, write a balanced redox reaction showing what happens when the metal dissolves. a. Al b. Ag c. Pb

Textbook Question

Which metal could you use to reduce Mn2+ ions but not Mg2+ ions?

Textbook Question

Which metal can be oxidized with an Sn2+ solution but not with an Fe2+ solution?

Textbook Question

Determine whether or not each metal dissolves in 1 M HIO3. For those metals that do dissolve, write a balanced redox equation for the reaction that occurs. a. Au b. Cr

Textbook Question

Calculate E°cell for each balanced redox reaction and determine if the reaction is spontaneous as written. b. MnO2(aq) + 4 H+(aq) + Zn(s) → Mn2+(aq) + 2H2O(l) + Zn2+(aq) c. Cl2(g) + 2 F–(aq) → F2(g) + 2 Cl–(aq)

Textbook Question

Calculate E°cell for each balanced redox reaction and determine if the reaction is spontaneous as written. a. 2 Cu(s) + Mn2+(aq) → 2 Cu+(aq) + Mn(s)