Chemistry Unit 10 Mr McMullen

Based off the unit 10 review list

Properties of Acids

Looks like water

Tastes sour

At first feels like water, then it burns

Acids reacts to produce H2 gas when reacting with metal

Conducts electricity

Turns lithiums red

Turns menthol orange to red

Phenolphtaline turns colorless

pH<7

Properties of bases

looks like water

Has a bitter taste (medicine)

Feel slippery then start to burn

Only reacts with Al & Zn

Conducts electricity

Turns litmus blue

Keeps methyl orange orange

Turns phenolphtaline pink

pH > 7

Which acids are found in acid rain

Carbonic acid

Sulfuric acid

Nitric acid

Sulfurous acid

Nitrous acid

Which gases are responsible for producing acid rain

Carbon Dioxide - CO2

Carbon Oxide - CO

Sulfur Dioxide - SO2

Nitrogen Dioxide - NO2

Nitrogen Oxide - NO

What is a Neutralization reaction

Acid + Base —> Water + Salt

HCl + NaOH —> H2O + NaCl

Arrhenius acid definition

A substance that dissociates in water to produce hydrogen ions

Ex. Substances HCl, H2SO4, HNO3, H2CO3

Ex. Image

Arrhenius Base definition

A substance that dissociates in water to produce hydroxide Ions

Ex substances. KOH, LiOH, Ca(OH)2

Arrhenius three limitations

1. Oversimplified what happens between acids and water ex. Image

2. Restricted acids and bases to water solutions

3. Excludes based without hydroxide ex. NaHCO3, NH3, CaCO3

Bronstead-Lowrery Acid definition

A substance that donates H+ ions (proton donator)

Bronstead-Lowery Base definition

A substance that accepts H+ ions (Proton acceptor)

Amphoteric

A substance that can react as either an acid or a base ex. H2O

Conjugate acid/base pairs and definition

Acids and baseS that differ by 1 H+ ion

H2SO4 | HSO4-1

H3O+1 | H2O

HCO3-1 | CO3-2

Strong acid definition and examples

An acid that completely ionizes to form many H3O+1 ions in water

Ex. HCl, HNO3, H2SO4

Weak acid definitions and examples

An acid that partially ionizes to form few H3O+1 ions in water

Ex. HC2H3O2, H2CO3

Titration

A lab procedure where a standard solution is used to determine the unknown concentration of an acid or base

Standard Solution

The acid or base of known concentration

Equivalence point

The neutralization point at which the concentration of the H3O+ ions are equal to the OH- ions

End point

The point at which the indicator changes color

Monoprotic

Acid with one ionizable hydrogen (HCl)

Diprotic

Acid with two ionizable hydrogen (H2SO4)

Triprotic

Acid with three ionizable hydrogens (H3PO4)