Chapter 14: Acid-Base Equilibrium

Question 1

arrehenius definition of an acid

Answer 1

increase the concentration of H+ when put in an aqueous solution

Question 2

arrehenius definition of a base

Answer 2

increases OH- concentration when put in an aqueous solution

Question 3

bronsted-lowry definition of an acid

Answer 3

an acid is a proton donor, any species that donates an H+

Question 4

bronsted-lowry definition of a base

Answer 4

a base is a proton acceptor, any species that accepts an H+

Question 5

how do you find pH?

Answer 5

-log [H+]

Question 6

how do you find [H+]?

Answer 6

10^-pH

Question 7

how do you find pOH?

Answer 7

-log[OH-]

Question 8

how do you find [OH-]?

Answer 8

10^-pOH

Question 9

what should pH and pOH equal?

Answer 9

14

Question 10

what does is it mean when Kb is larger than Ka?

Answer 10

the equation is basic

Question 11

what happens when the concentrations of products are greater than the concentration of reactants?

Answer 11

the reactants will hold the stronger values for acid and base

Question 12

what does more hydrogens in a molecule mean for the acidity?

Answer 12

the more hydrogens, the more acidic the solution will be

Question 13

how do you find Ka from pKa?

Answer 13

Ka= 10^-pKa

Question 14

how do you determine the strongest acid based off of molarity and pKa?

Answer 14

the smaller the pKa and the smaller the concentration, the more acid the value is

Question 15

how do you find Kb from Ka?

Answer 15

1.0 x 10^-14 / Ka

Question 16

how do you find [OH-] from [H3O+] and vice vera?

Answer 16

1.0 x 10^-14 / [H3O+] or [OH-]

Question 17

how do you find pH from [OH-]?

Answer 17

take the log of [OH-], which gives you pOH, then subtract by 14 to give you pH

Question 18

What are the strong acids?

Answer 18

H2SO4, HI, HBr, HNO3, HCl, HClO4

So I Brought No Clean Clothes

Question 19

what are the strong bases?

Answer 19

any element from group 1 or 2 with an OH- group