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Chemistry Chapter 14/15 Cheat Sheet (DRAFT) by

Cheat sheet for Allunt's chem. course chapter 14 and 15 (Modern Chemistry)

This is a draft cheat sheet. It is a work in progress and is not finished yet.

Vocab

Binary Acid
Contains only two different elements: hydrogen and one other electr­one­gative element
Oxyacid
Compound of hydrogen, oxygen, and a third nonmetal element
Arrhenius Acid
Chemical compound that increases the concen­tration of hydrogen ions H+
Arrhenius Base
Chemical compound that increases the concen­tration of hydroxide ions OH-
Strong Acid
Ionizes completely in an aqueous solution
Weak Acid
Releases few hydrogen ions in an aqueous solution
Bronst­ed-­Lowrey Acid
Molecule or ion that is a proton donor
Bronst­ed-­Lowrey Base
Molecule or ion that is a proton acceptor
Bronst­ed-­Lowrey Acid-Base Reaction
Protons are transf­erred from an acid to a base
Monoprotic Acid
Acid that can donate only one proton per molecule
Polyprotic Acid
Acid that can donate more that one proton per molecule
Diprotic Acid
Acid that can donate two protons per molecule
Triprotic Acid
Acid that can donate three protons per molecule
Lewis Acid
Atom, ion, or molecule that accepts an electron pair to form a covalent bond
Lewis Base
Atom, ion, or molecule that donates an electron pair to form a covalent bond
Lewis Acid-Base Reaction
Formation of one or more covalent bonds between an electr­on-pair donor and an electr­on-pair acceptor
Conjugate Base
Substance that is left after an acid has given up a proton
Conjugate Acid
The acid that is formed after a base accepts a proton
Amphoteric
Any substance that can act as an acid or a base
Salt
Ionic compount composed of a cation from a base and an anion from an acid
Neutra­liz­ation
The reaction of hydronium ions and hydroxide ions to form water molecules and salts
Self-I­oni­zation of Water
Two water molecules produce a hydronium ion and a hydroxide ion by transfer of a proton
pH
The negative of the common log of the hydronium ion concen­tration
pOH
The negative of the compound log of the hydroxide ion concen­tration
Acid-Base Indicators
Compounds whose colors are sensitive to pH
Transition Intervals
The pH range over which an indicator changes color
pH Meter
Determines the pH of a solution by measuring the voltage between the two electrodes that are placed in the solution
Titration
Controlled addition and measur­ement of the amount of a solution of known concen­tration required to react completely with a measured amount of a solution of unknown concen­tration
Equiva­lence Point
The point at which the two solutions used in a titration are present chemically equivalent amounts
End Point
The point in a titration at which an indicator changes color
Standard Solution
Solution that contains the precisely known concen­tration of a solute
Primary Standard
highly purified solid compound used to check the concen­tration of the known solution in a titration

Determ­ining the pH and Titrations

The pH of a solution can be measured using either a pH meter or acid-base indica­tors.
Titration uses a solution of known concen­tration to determine the concen­tration of a solution of unknown concen­tra­tion.
To determine the end point of a titration, one should choose indicators that change color over ranges that include the pH of the equiva­lence point.
When the molarity and volume of a known solution used in aa titration are known, then the molarity of a given volume of an unknown solution can be found.

Properties of Acids and Bases

Acids have a sour taste and react with active metals. Acids change the colors of acid-base indica­tors, react with bases to produce salts and water, and conduct electr­icity in aqueous solutions.
Bases have a bitter taste, feel slippery to the skin in dilute aqueous solutions, change colors of acid-base indica­tors, react with acids to produce salts and water, and conduct electr­icity in aqueous solutions.
An arrhenius acid contains hydrogen and ionizes in aqueous solution to form hydrogen ions. An Arrhenius base produces hydroxide ions in aqueous solution.
The strength of an Arrhenius acid or base is determined by the extent to which the acid or base ionizes or dissoc­iates in aqueous solutions.
 

Acid-Base Theories

A Bronst­ed-­Lowry acid is a proton donor. A Bronst­ed-­Lowry base is a proton acceptor.
A Lewis acid is an electr­on-pair acceptor. A Lewis base is an electr­on-pair donor.
Acids are described as monopr­otic, diprotic, or triprotic depending on whether they can donate one, two, or three protons per molecule, respec­tively, in aqueous solutions. Polyprotic acids include both diprotic and triprotic acids.

Aqueous Solutions and the Concept of pH

Pure water undergoes self-i­oni­zation to give 1.0x10-7 M H30+ and 1.0x10-7 M OH- at 25C
pH=-lo­g[H­3o+]; at 25C, pH+pOH=14
At 25C, acids have a pH of less than 7, bases have a pH of greater than 7, and neutral solutions have a pH of 7.
If a solution contains a strong acid or a strong base, the [H3O+] and the [OH-}, and the pH can be calculated from the molarity of the solution. If a solution contains a weak acid or a weak base, the [H3O+] and the [OH-] must be calculated from an experi­men­tally measured pH.
 

Acid-Base Reactions

A Bronst­ed-­Lowry acid-base reaction, there are two conjugate acid-base pairs.
A strong acid has a weak conjugate base; a strong base has a weak conjugate acid.
Proton­-tr­ansfer reactions favor the production of the weaker acid and weaker base.
The acidic or basic behavior of a molecule containing -OH groups depends on the electr­one­gat­ivity of other atoms in the molecule and on the number of oxygen atoms bonded to the atom that is connected to the -OH group.
A neutra­liz­ation reaction produces water and an ionic compound called a salt.
Acid rain can create severe ecological problems