Integrated SequencePhysics Chemistry Organic Biology

WikiPremed Resources

Module 8 in the Syllabus
Curriculum

Acids & Bases Practice Items
Problem set for Acids & Bases in PDF format

Answer Key
Answers and explanations

Acids and Bases Images
Image gallery for study with links to larger teaching JPEGs for classroom presentation

Question Drill for Acids and Bases
Conceptual Vocabulary Self-Test

Basic Terms Crossword Puzzle

Basic Puzzle Solution

Overview of Acids and Bases
The definition of an acid or a base depends on the system you are using. In the Arrhenius definition of acids and bases, an acid is a substance that releases hydrogen ions when dissolved in water, and a base is a substance that releases hydroxide ions. Although in chemistry today, the Brønsted-Lowry definition has largely superseded it, under the Arrhenius definition it is possible to predict the result of the neutralization of an acid with a base, which is a salt and water.

If a chemist doesn't specify which acid-base system they are using, it can be assumed they are working within the Brønsted-Lowry system. A Brønsted acid is any substance that can donate a hydrogen ion. A Brønsted base is defined as any substance that can accept a hydrogen ion. In other words, a Brønsted acid is a proton donor, and a Brønsted base is a proton receiver. The Brønsted-Lowry system implies the acid-base reaction to occur within a system of conjugate acid-base pairs governed by an equilibrium. Acids increase the concentration of hydrogen ions, while bases decrease the concentration of hydrogen ions. The acidity or basicity of a solution can therefore can be measured by its hydrogen ion concentration (or pH, the negative logarithm of concentration).

The Lewis definition of acids (as electron pair receivers) and bases (as electron pair donors) is actually broader than either the Arrhenius or Brønsted-Lowry. The Lewis system provides a productive framework for viewing many chemical events from nucleophilic approach to the formation of coordination complexes, although the Brønsted-Lowry system is the traditional framework for discussion and problem solving involving acid-base equilibria.

Acids and Bases on the MCAT
As with Solutions, the previous chapter, every MCAT will have a number of questions deriving from the material in Acids & Bases. Although big, multi-variable quantitative acid-base equilibrium questions are a standard of Chem 101, you are not likely to run into such questions on the MCAT. However, the MCAT definitely will call on you to demonstrate that you understand the basic concepts of acid-base equilibrium. Buffers & indicators are MCAT favorites, as well as titration curves.

Conceptual Vocabulary
AcidAn acid is traditionally considered any chemical compound that, when dissolved in water, gives a solution with a pH less than 7.0.
BaseA base is most commonly thought of as a substance that can accept protons.
pHpH is a measure of the acidity or alkalinity of a solution.
Strong acidA strong acid is an acid that dissociates completely in an aqueous solution.
Sodium hydroxideSodium hydroxide, also known as lye, caustic soda and sodium hydrate, is a caustic metallic base.
HydroniumHydronium is the common name for the cation derived from protonation of water. It is the simplest type of an oxonium ion.
Acid-base reactionAn acid-base reaction is a chemical reaction that occurs between a proton donor and a proton receiver.
Lewis baseA Lewis base is any molecule or ion that can form a new coordinate covalent bond, by donating a pair of electrons.
Hydrochloric acidHydrochloric acid is the aqueous solution of hydrogen chloride gas.
Lewis acidA Lewis acid can accept a pair of electrons and form a coordinate covalent bond.
Weak baseA weak base is a chemical base that does not ionize fully in an aqueous solution
Weak acidA weak acid is an acid that does not ionize in solution to a significant extent.
AlkaliAn alkali is a basic, ionic salt of a group I or group II element.
Sodium carbonateSodium carbonate is a sodium salt of carbonic acid.
Acid dissociation constantAn acid dissociation constant is an equilibrium constant for the dissociation of a weak acid.
Buffer solutionBuffer solutions are solutions that resist change in Hydronium ion and the hydroxide ion concentration (and consequently pH) upon addition of small amounts of acid or base, or upon dilution.
Acid-base titrationAn acid-base titration is a volumetric method in chemistry that allows quantitative analysis of the concentration of an unknown acid or base solution, making use of the neutralization reaction that occurs between acids and bases.
ProtonationProtonation is the addition of a hydrogen ion to an atom, molecule, or ion.
pH indicatorA pH indicator is a halochromic chemical compound that is added in small amounts to a solution so that the pH of the solution can be determined easily.
AmmoniaAmmonia is a compound consisting of one nitrogen atom singly bound to three hydrogen atoms, normally encountered as a gas with a characteristic pungent odor.
Hydrogen chlorideHydrogen chloride has the formula HCl.
Sulfuric acidSulfuric acid is a strong mineral acid once known as oil of vitriol. Each molecule contains a sulfur atom, two hydrogen atoms and four oxygen atoms.
Equivalence pointThe equivalence point or stoichiometric point occurs during a chemical titration when the amount of titrant added is equivalent, or equal, to the amount of analyte present in the sample.
Mineral acidA mineral acid is an acid derived from inorganic substances by chemical reaction as opposed to organic acids.
NeutralizationNeutralization is a chemical reaction, also called a water forming reaction, in which an acid and a base react and produce a salt and water.
OxoacidAn oxoacid is an acid which contains oxygen.
Nitric acidNitric acid, also known as aqua fortis and spirit of nitre, is an aqueous solution of hydrogen nitrate.
Phosphoric acidPhosphoric acid, also known as orthophosphoric acid, is a mineral acid having a molecular structure with one phosphorus atom, four oxygen atoms, and three hydrogen atoms.
BicarbonateA bicarbonate is an intermediate form in the deprotonation of carbonic acid.
SuperbaseA superbase is an extremely strong base.
SuperacidA superacid is an acid with an acidity greater than that of 100% sulfuric acid.
Proton affinityThe proton affinity of an anion or of a neutral atom or molecule is a measure of its gas-phase basicity.
HydronHydron is the general name for the positive hydrogen cation, used to reflect ions formed from the naturally abundant hydrogen, as opposed to proton, which only refers to the most common isotope of hydrogen.
BuretteA burette is a vertical cylindrical piece of laboratory glassware with a volumetric graduation on its full length and a precision tap, or stopcock, on the bottom.



The WikiPremed MCAT Course is a free comprehensive course in the undergraduate level general sciences. Undergraduate level physics, chemistry, organic chemistry and biology are presented by this course as a unified whole within a spiraling curriculum.

Please read our policies on privacy and shipping & returns.  Contact Us.
MCAT is a registered trademark of the Association of American Medical Colleges, which does not endorse the WikiPremed Course.


Creative Commons License
The work of WikiPremed is published under a Creative Commons Attribution Share Alike 3.0 License. There are elements of work here, such as a subset of the images in the archive from WikiPedia, that originated as GNU General Public License works, so take care to follow the unique stipulations of that license in printed reproductions. You can use the resources here for commercial or non-commercial purposes, but please give attribution and a link to the production credits and edit history of the resource. For the works here which began as my individual work, please attribute "John Wetzel, an author at wikipremed.com".