pH and buffers

Question 1

In arrhenius acids and bases
acids are
bases are

Answer 1

ACID – any substance that ionizes in water to produce hydrogen ions.
BASE – any substance that ionizes in water to produce hydroxide ions.

Question 2

In bronsted-lowry acids and bases
acids are
bases are

Answer 2

ACID – any substance that can donate a proton or a proton donor
BASE – any substance that can accept a proton or a proton acceptor

Question 3

In lewis acids and bases,
acids and bases are

Answer 3

ACID– any substance that can accept an electron pair in completing the stable group of one of its own atoms.
BASE – any species that donates a pair of electrons to a Lewis acid to form a Lewis adduct. Example: OH- and NH3 are Lewis bases because they can donate a lone pair of electrons.

Question 4

is the measurement of the acidity and the basicity of a substance

Answer 4

pH

Question 5

TRUE or FALSE
For strong electrolytes, the concentration of the strong acid/base will be the concentration of the hydrogen ions. Strong electrolytes are substances that completely dissociate in water.

Answer 5

TRUE

Question 6

TRUE or FALSE
For weak electrolytes: Weak electrolytes are substances that do not completely dissociate in water, and the acid dissociation constant, Ka, will determine the extent of dissociation. Thus, for the given equation, the concentration of the hydrogen ions will be calculated using the acid dissociation constant, Ka.

Answer 6

TRUE

Question 7

For very strong acids: pKa is

Answer 7

less than 1

Question 8

For moderately strong acids: pKa is

Answer 8

is equal from 1 to 5

Question 9

For weak acids: pKa is

Answer 9

5 to 15

Question 10

For extremely weak acids: pKa

Answer 10

is greater than 15