Textbook Question
What is the molar solubility of BaF2 in a solution containing 0.0750 M LiF (Ksp = 1.7 x 10^-6)(a) 2.3 x 10^-5 M(b) 3.0 x 10^-4 M(c) 1.2 x 10^-2 M(d) 1.3 x 10^-3 M
1
views
Ch.17 - Applications of Aqueous Equilibria
Chapter 17, Problem 35
Consider the following table of standard reduction potentials: 
(b) Which substances can be oxidized by B2+? Which can be reduced by D?
Verified step by step guidance1
Identify the standard reduction potential for B2+ and D from the table.
Determine the standard reduction potential for B2+ and compare it with the given potentials to find substances that can be oxidized by B2+.
Identify substances with a lower reduction potential than B2+ as they can be oxidized by B2+.
Determine the standard reduction potential for D and compare it with the given potentials to find substances that can be reduced by D.
Identify substances with a higher reduction potential than D as they can be reduced by D.
Verified video answer for a similar problem:
This video solution was recommended by our tutors as helpful for the problem above.
Video duration:
4mWas this helpful?
Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Standard Reduction Potentials
Standard reduction potentials (E°) indicate the tendency of a species to gain electrons and be reduced. A higher E° value means a greater likelihood of reduction, while a lower or negative E° suggests a lesser tendency. These values are measured under standard conditions and are crucial for predicting the direction of redox reactions.
Recommended video:
Guided course
01:10
Standard Reduction Potentials
Oxidation and Reduction
Oxidation is the process of losing electrons, while reduction is the gain of electrons. In a redox reaction, one species is oxidized and another is reduced. The ability of a substance to be oxidized or reduced can be determined by comparing their standard reduction potentials, where a substance with a lower E° can be oxidized by one with a higher E°.
Recommended video:
Guided course
01:53Oxidation and Reduction Reactions
Electrochemical Series
The electrochemical series is a list of standard reduction potentials for various half-reactions, arranged from highest to lowest. This series helps predict which substances can oxidize or reduce others. By analyzing the potentials, one can determine the feasibility of redox reactions and identify which species can act as oxidizing or reducing agents.
Recommended video:
Guided course
02:46Electrochemical Cells
Related Practice
Textbook Question
What is the molar solubility of AgI in 0.20 M NaCN? (a) 6.2 x 10^-4 M(b) 1.0 x 10^-1 M(c) 7.6 x 10^-2 M(d) 2.1 x 10^-3 M
Textbook Question
A solution containing sulfide ions is added to a solution of 0.036 M Cu2+ and 0.044 M Fe2+. At what concentration of sulfide ion will a precipitate begin to form? What is the identity of the precipitate? (a) 1.4 x 10^-16 M, FeS(b) 3.6 x 10^-35 M, CuS(c) 3.6 x 10^-35 M, FeS(d) 1.4 x 10^-16 M, C
Textbook Question
The strong acid HA is mixed with an equal molar amount of aqueous NaOH. Which of the following pictures represents the equilibrium state of the solution? (Na+ ions and solvent water molecules have been omitted for clarity.)
(A) (B) (C) (D)
Textbook Question
The following pictures represent initial concentrations in solutions that contain a weak acid HA (pKa = 6.0) and its sodium salt NaA. (Na+ ions and solvent water molecules have been omitted for clarity.) .(c) Draw a picture that represents the equilibrium state of solution (1) after the addition of two OH-ions.
Textbook Question
The following pictures represent initial concentrations in solutions that contain a weak acid HA (pKa = 6.0) and its sodium salt NaA. (Na+ ions and solvent water molecules have been omitted for clarity.)
. (b) Draw a picture that represents the equilibrium state of solution (1) after the addition of two H3O+ ions.
1
views