Chapter 2.3 Solutions

Acid

Molecules capable of releasing a hydrogen ion; solutions having an H+ concentration greater than that of pure water (that is, pH less than 7)

Acidic Solutions

Any solutions with a pH less than 7

Acidity

Concentration of free, unbound hydrogen ion in a solution; the higher the H+ concentration, the greater the acidity

Alkaline Solutions

Any solutions having H+ concentration lower than that of pure water (i.g. having a pH greater than 7)

Amphiphatic Molecule

A molecule containing polar or ionized groups at one end and nonpolar groups at the other

Base

Any molecule that can combine with H+; (nucleotide) molecular ring of carbon and nitrogen that, with a phosphate group and a sugar, constitutes a nucleotide

Concentration

Amount of solute per unit volume of solution

Dehydration

Type of chemical reaction in which two smaller molecules, such as amino acids, are joined to form a larger molecule; a single molecule of water is lost in the process

Hydrolysis

Breaking of chemical bond with addition of elements of water (-H and -OH) to the products formed (aka Hydrolytic Reaction)

Hydrophilic

Attracted to, and easily dissolved in, water

Hydrophobic

Not attracted to, and insoluble in, water

Mole

The amount of a compound in grams equal to its molecular weight

Molecular Weight

Sum of atomic weights of all atoms in molecule

pH

Expression of a solution’s acidity; negative logarithm to base 10 of H+ concentration; pH decreases as acidity increases

Solutes

Substances dissolved in a liquid

Solution

Liquid (solvent) containing dissolved substances (solutes)

Solvent

Liquid in which substances are dissolved

Strong Acids

Acids that ionize completely to form hydrogen ions and corresponding anions when dissolved in water

Weak Acids

Acids whose molecules do not completely ionize to form hydrogen ions when dissolved in water