Lecture 20

Question 1

Strong or weak acid HCl

Answer 1

strong

Question 2

Ionization of acids

Answer 2

when dissolve in water, acids and bases dissociate into two ions.

Question 3

Oxy acids have acid hydrogens attached to an oxygen atom

Answer 3

h2SO4, HNO3 example

Question 4

Carboxylic acids have COOH

Answer 4

HC2H3O2 (only one H in the formula is acidic

Question 5

Bases structure

Answer 5

OH ions (NaOH, Ca(OH))2. Mostly amine groups (derivitaves of ammonia)-Molecular bases contain structures that react with H+

Question 6

Acid base reactions (neutralization reactions)

Answer 6

Acid and Base neutralize each others properties. Acid + Base –> Salt + water (salt must be aq)

Question 7

acids with metal oxides

Answer 7

Acids react with metal oxides to produce water and a dissolved salt. ex: HCl reacts with potassium oxide to form water and potassium chloride (2HCl (aq)+ K2O (s)—> H2O(l) + 2KCl (aq)

Metals go into the solution and usually produce Hydrogen gas. Salt contains the metal ion usually.

Question 8

bronsted-Lowry acids and bases

Answer 8

Acid is a proton donor
Base is a proton acceptor

Question 9

Acids and bases and conjugates

Answer 9

Acid - Conjugate base Base- Conjugate acid

Question 10

Titration

Answer 10

Titrant (known solution) added from a buret.

Question 11

Indicators

Answer 11

Chemicals are added to help determine the endpoint

Question 12

Endpoint- definiton

Answer 12

of the titration occurs when the reaction is complete

Question 13

Base solution -

Answer 13

Titrant in the buret

Question 14

Endpoint (color)

Answer 14

At the titrants endpoint, just enough base has been added to neutralize all the acid, at this point the indicator changes color.

Question 15

Ion product of water

Answer 15

Kw (h30+] x [OH-] = 1x 10^-14=kw
If h30 increases then OH must decrease (inversely proportional)

Question 16

Acidic and basic solutions kw for neutral, acidic, and basic

Answer 16

Neutral = 1x10^-7
Acidic H3O > 1 x 10^-7 OH < 1 x 10^-7
Basic H3O < 1 x 10^-7 OH > 1 x 10^-7

Question 17

Acidity and basicity of solution expressed as PH is

Answer 17

pH <7 = acidic
pH >7 =basic
pH = 7 = neutral

Question 18

POH =

Answer 18

pOH = -log[OH-]
[OH-] = 10^(-pOH)
pOHwater= -log[10^-7] = 7

**NEED TO KNOW OH- to find pOH. same as ph.
pOH 0 is [OH-] =1M (can be negative or larger than 14)
pOH14 is [h3O+] =1M
pH + pOH=14.00