acids and bases up to %ionization

Question 1

Bronsted acid

Answer 1

a substance that is capable of donating a proton

HA –> H+ + A-

Question 2

Bronsted base

Answer 2

a substance that is capable of accepting a proton

B + H –> BH+

Question 3

Conjugate acid

Answer 3

an acid formed when a base accepts a proton

Question 4

Conjugate base

Answer 4

a base formed when an acid donates a proton

Question 5

conjugate pair

Answer 5

an acid and a base that only has a proton as their difference. E.G H2SO4 –>

Question 6

Diprotic and Triprotic

Answer 6

Diprotic is a substance that has 2 donatable protons

Triprotic has 3

Question 7

Amphoteric

Answer 7

a substance that can behave like an acid or a base depending on what it reacts with

Question 8

An electrolyte

Answer 8

An electrolyte is any substance that can be dissolved in water to give positive and negative ions

Question 9

Is water an electrolyte

Answer 9

water is a weak electrolyte because it can autoionize to a small extent

Question 10

Equilibrium constant

Answer 10

the equilibrium constant explains that at equilibrium, the concs of the forward and reverse reaction remains the same even though the reaction is still occurring
It is represented by K

K= [products] / [reactant]

Question 11

Kw

Answer 11

This is the equilibrium constant of water.

Kw= [OH-] [H+] = 10^-14 at 25 celsius

Question 12

At 25 celsius, what is the concentration of water

Answer 12

10^-14 M

Question 13

At 25 celsius, what is the concentration of H+ in water

Answer 13

10^-7 M

Question 14

pH

Answer 14

The measure of acidity

pH= -log[H+]

Question 15

Strong acid and base

Answer 15

A strong acid or base is one that can completely ionize in water

Question 16

ionization

Answer 16

the breakdown of substances into positive and negative ions

Question 17

weak acid and base

Answer 17

A weak acid or base does not completely ionize in water. They can approach 100% ionization but can’t reach it.

Question 18

Relationship between concentration and weak acid/base strength

Answer 18

As the concentration decreases, the strength of the weak acid/base increases. Meaning that at very low concentrations, weak acids/bases can ionize more but not completely. The lowest Ka or Kb is the strongest.

Question 19

are conjugates weak or strong?

Answer 19

conjugate acids/bases are always weak

Question 20

examples of strong acids

Answer 20

HCLO4, HCLO3, H2SO4, HNO3, HI, HBR, HCL

Question 21

examples of weak bases

Answer 21

NaOH, KOH, LiOH, Sr(OH)2, Br(OH)2 etc

Question 22

Ka

Answer 22

Ka is the strength of the acid. It is also referred to as the acid dissociation constant so the higher Ka is, the stronger the weak acid.

Ka= [products]/[reactant]

Question 23

how do we determine the pH of a weak acid when Ka is available,

Answer 23

use the ice table

Question 24

% ionization

Answer 24

It is used to show how much acid was ionized.

% ionization = [ionized acid]/[initial conc] x 100