- Lesson 123.1: Explain how an acid-base indicator works to show the pH of a solution.
- Lesson 123.2: Does the value of K for an indicator change when the indicator is a...
- Lesson 123.3: The solubility product constants Kap at 25 8C for several chlorides...
- Lesson 123.4: Imagine you prepare a 0.10 M solution of nitric acid, HNO3, and a 0...
- Lesson 123.5: Use the table on page 648 to predict the color of these indicators ...
- Lesson 123.6: Use Le Chteliers principle to explain why bromocresol green is blue...
- Lesson 123.7: Determine the pH value at which thymolphthalein changes color. Th e...
- Lesson 123.8: Methyl violet changes color from the yellow HIn molecule to the blu...
- Lesson 123.9: Look up the source, structure, and properties of a particular indic...
Solutions for Chapter Lesson 123: Applying Le Chteliers Principle
Full solutions for Living by Chemistry | 2nd Edition
A carbohydrate that contains an aldehyde group.
A polymer that is formed under conditions in which the monomers do not react directly with each other, but rather, each monomer is added to the growing chain, one at a time.
In UV-Vis spectroscopy, the region of the molecule responsible for the absorption (the conjugated p system).
conservation of orbital symmetry
During a reaction, the requirement that the phases of the frontier MOs must be aligned.
A process during which a protein unfolds under conditions of mild heating.
Polymers that return to their original shape after being stretched.
Important biological molecules that catalyze virtually all cellular processes.
Any process with a negative DG.
Ground-state electron confi guration
The lowest-energy electron confi guration for an atom or molecule.
heat of fusion
The enthalpy change, ?H, for melting a solid. (Section 11.4)
A hydrogen atom with two electrons in its valence shell; H:!
Compounds formed when hydrogen reacts with alkali metals and also the heavier alkaline earths (Ca, Sr, and Ba); these compounds contain the hydride ion, H-. (Section 22.2)
A measure of the strength of an acid: Ka = Keq 3H2O4 = 3H3O+ 4 3A- 4 3HA4
A compound containing a carbonyl group bonded to two carbons.
metallic elements (metals)
Elements that are usually solids at room temperature, exhibit high electrical and heat conductivity, and appear lustrous. Most of the elements in the periodic table are metals. (Sections 2.5 and 12.1)
The product formed when either d-ribose or 2-deoxy-d-ribose is coupled with certain nitrogen heterocycles (called bases).
A series of reactions by which a set of organic starting materials is converted to a more complicated structure.
The emission of electrons from a metal surface induced by light. (Section 6.2)
A large molecule of high molecular mass, formed by the joining together, or polymerization, of a large number of molecules of low molecular mass. The individual molecules forming the polymer are called monomers. (Sections 12.1 and 12.8)
A compound whose carbon skeleton can be divided into two or more units identical with the carbon skeleton of isoprene