Ch 15: Acids and Bases Flashcards
acid properties
- aqueous solutions of acids have a sour taste
- acids change the color of acid-base indicators
- some acids react with active metals to release hydrogen gas
- acids react with bases to produce salts and water
- some acids conduct electric current
binary acid
an acid that contains only two elements: hydrogen and one of the more electronegative elements
binary acid nomenclature
- the name of a binary acid begins with the prefix hydro-
- the root of the name of the second element follows this prefix
- the name then eds with the suffix -ic
oxyacid
an acid that is a compound of hydrogen, oxygen, and a third element, usually a nonmetal
base properties
- aqueous solutions of bases taste bitter
- bases change the color of acid-base indicators
- dilute aqueous solutions of bases feel slippery
- bases react with acids to produce salts and water
- bases conduct electric current
Arrhenius acid
a chemical compound that increases the concentration of hydrogen ions in aqueous solution (H+)
Arrhenius base
a substance that increases the concentration of hydroxide ions OH- in an aqueous solution
strong acid
one that ionizes completely in aqueous oslution
weak acid
acids that are weak electrolytes are known as weak acids
alkaline
when a base completely dissociates in water to yield aqueous OH- ions, the solution is referred to as alkaline
Bronsted-Lowry acid-base reaction
protons are transferred from one reactant (the acid) to another (the base)
Bronsted-Lowry acid
a molecule or ion that is a proton donor
Bronsted-Lowry base
a molecule or ion that is a proton acceptor
monoprotic acid
an acid that can donate only one proton (h+) per mole
polyprotic acid
an acid that can donate more than one proton per molecule
lewis acid
an atom, ion, or molecule that accepts an electron pair to form a covalent bond
lewis base
an atom, ion, or molecule that donates an electron pair to form a covalent bond
lewis acid-base reaction
the formation of one or more covalent bonds between an electron-pair donor and an electron-pair acceptor
lewis acid-base reaction
the formation of one or more covalent bonds between an electron-pair donor and an electron-pair acceptor
conjugate base
the species that remains after a Bronsted-Lowry acid that has given up a proton
conjugate acid
the species that remains after a Bronsted-Lowry acid that has gains a proton
What does the extent of the reaction between a Bronsted Lowry acid and base depend on?
The relative strength of the acids and bases involved; the stronger an acid/base, the weaker its conjugate.
amphoteric
any species that can react as either an acid or a base
hydroxyl group
the covalently bonded -OH group in an acid
neutralization
the reaction of hydronium ions and hydroxide ions to form water molecules
salt
an ionic compound composed of a ation from a base and an anion from an acid
