Acids and Bases Flashcards
Arrhenius Theory of Acids and Bases
a substance that donates a H+ is an acid and a substance that donates a OH- is a base
neutralization reaction
when an acid is mixed with a base, a salt and water forms
Bronsted-Lowry Acid
substance that donates a H+
Bronsted-Lowry Base
substance that accepts a H+
hydronium is a
pronated water molecule
conjugate acid/base pair
two substances that differ by 1 H+
amphiprotic substance
species that can act as an acid or a base
most common amphiprotic substance
water
titration
types of volumetric analysis where the concentration of a solution can be determined through stoichiometry using a standard solution
titrant
solution that is standardized of known concentration
analyte
solution tested of unknown concentration
equivalence point
point in the titration where the moles of the titrant are equal to the moles of the analyte
acid/base indicators
complex molecules that change in the presence of an acid or a base
bromothymol blue
green when neutral, blue when basic, yellow when acidic
phenolphthalein
turns pink in the presence of a base
What is the difference between a concentrated acid and a strong acid?
concentration refers to the amount of molecules in a solvent and strength refers to the extent of ionization
strong acid
acid that ionizes completely
6 strong acids
perchloric, hydroiodic, hydrobromic, hydrochloric, nitric, sulfuric
weak acid
acid that only partially ionizes in water
acid ionization constant
Ka; equilibrium constant for weak acids
all weak acids have a
ka<1
strong base
base that ionizes completely
strong bases include the OH- bound to a
group 1A or 2A element
weak base
base that partially ionizes in water
base ionization constant
Kb; equilibrium constant for weak bases
binary acid(Hx)
the strength of a binary acid is determined by bond length
bond length
the distance between the H and its anion
binary acids: the larger the anion,
the longer the bond, the longer the bond the weaker the bond, the weaker the bond, the easier the H+ ionizes(stronger acid)
the more H+ on the binary acids,
the weaker the acid
hydrohalic acids are
the strongest acids
hydrohalic acids
acids made with halogens
ternary acids(oxo-acids, oxy-acids)
the strength of ternary acids are determined by the number of oxygens and the electronegativity of the center atom
ternary acids: the stronger acid has
more oxygens; if oxygens are the same, the acid with the more electronegative center atom is stronger
carboxyllic acids
the strength of a carboxyllic acid is determined by the polarization of the -O-H- bond
carboxyllic acid: the fewer carbons in the base chain
causes increased polarization, making a stronger acid
the substance that has the higher Ka value will
act as the acid, the proton donor
shifts in equilibria for acid-base systems
the direction of strong acid and strong base forming the weak acid and base is favored
the strong acid and the strong base are
always on the same side of the equation
leveling effect
the effect that all strong acids ionize completely in water gives the impression that they are all the same strength
