Chemistry - Acids and Bases

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Know the common industrial acid known as muriatic acid.

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1

Know the common industrial acid known as muriatic acid.

HCl (hydrochloric acid)

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2

Know the acid manufactured in the largest amount.

H2SO4 (Sulfuric acid)

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3

Be able to choose the strongest base from a list of compounds.

H2O, NaOH, NH3, HCl

NaOH is the strongest. The reason? OH- is hydroxide ions, making bases stronger.

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4

In a given reaction be able to identify the conjugate acid-base.

EX: HF + H2O > F- + H3O

HF is the acid

H2O is the base

F- is the conjugate base

H3O is the conjugate acid

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5

The stronger an acid is, the (stronger/weaker) its conjugate base.

The stronger a base, the (stronger/weaker) its conjugate acid.

weaker, weaker. Remember: it’s always inverse

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6

Acid strength (increases/decreases) with (increasing/decreasing) polarity and (increasing/decreasing) bond strength.

increases, increasing, decreasing

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7

Acid + Base > ? + ?

Acid + Base > water + salt

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8

If you have barium carbonate + HCl > ? + ?

barium chloride + carbon dioxide

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9

diprotic

donates 2 protons

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10

binary

2 acids mixed together (hydrogen + something with electro negativity)

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11

When an acids donates a proton, it becomes a

conjugate base

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12

It can be an acid or a base (ex: H2O)

amphoteric

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13

HBrO

hypobromous acid

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14

HI

hydroiodic acid

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15

H2SO4

sulfuric acid

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16

H2CO3

carbonic acid

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17

HCl

hydrochloric acid

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18

HNO2

nitrous acid

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19

hydrosulfuric acid

H2S

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20

perchloric acid

HCLO4

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21

phosphorous acid

H3PO3

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22

nitric acid

HNO3

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23

List the conjugate acid and base pairs. Identify each reactant + product as an acid or a base.

HF + H2O > F- + H3O

PAIRS:

HF + F-

H2O + H3O

ACID OR BASE:

HF + F- = acidic

H2O + H3O = basic

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24

List the conjugate acid and base pairs. Identify each reactant and product as a proton donor or acceptor.

H2O + NH3 > NH4 + OH-

PAIRS:

H2O + OH-

NH3 + NH4

DONORS AND ACCEPTORS:

H2O + OH- = donors

NH3 + NH4 = acceptors

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25

Acid Base Neutralization formula equation

HCL + NaOH > NaCL + H2O

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26

Acid Base Neutralization overall net ionic equation

H3O+ + CL- + Na+ + OH- > Na+ + Cl- + 2H2O

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27

Acid base Neutralization net ionic equation

H3O+ + OH- > 2H2O

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28

periodic acid

HIO4

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29

iodic acid

HIO3

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30

hypoiodous acid

HIO

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31

List HIO4, HIO3, HIO from weakest to strongest

HIO, HIO3, HIO4

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32

Explain the difference between strong acids and weak acids

Any acid that fully dissociates into ions is strong, if it doesn’t it’s weak

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33

Explain how the production of sulfur trioxide, SO3, in industrial processes results in acid rain. Write an equation for the reaction.

SO3 produces as a gas. It dissolves in the water vapor in the clouds. This produces sulfuric acid solution that falls like rain or snow.

SO3 + H2O > H2SO4

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34

List five properties of aqueous acids

Sour taste

change in color of acid-base indicator

some react with metal to release hydrogen gas

react w/ bases to produce salt and H2O

conduct electric current

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35

Write the balance equations that describe the three stage ionization of phosphoric acid in a dilute aqueous solution

  1. H3PO4 + H2O > H3O + H2PO4

  2. H2PO4 + H2O > H3O + HPO4 2-

  3. HPO4 2- + H2O > H3O PO4 3-

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