INTRODUCTION

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Many ways to classify compounds Are they ionic or covalent? A common method is to separate into ACIDS and BASES. INTRODUCTION. We see, use, and eat acids everyday Sour grapefruit Tart taste of carbonated drinks Tangy taste of salad dressing. acids. - PowerPoint PPT Presentation

Transcript of INTRODUCTION

Page 1: INTRODUCTION
Page 2: INTRODUCTION

INTRODUCTION

Many ways to classify compounds Are they ionic or covalent?

A common method is to separate into ACIDS and BASES

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ACIDS We see, use, and eat acids everyday

Sour grapefruit Tart taste of carbonated drinks Tangy taste of salad dressing

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Acidic juices are added to food to improve taste and help absorb nutrients

Stomach acid helps us digest food

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ACIDS - 2

Have corrosive properties Acid rain can dissolve caves, buildings, and

statues Used to remove rust and purify/process

metals

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BASES

Bitter tasting compounds with a slippery feel

Includes many cleaning products Soap Over cleaner

Some medical drugs are bases lidocaine

We eat some basic foods eggs and baking soda

Also known as alkaline

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SAFETY

Some acids and bases can be corrosive Can burn throat or stomach if swallowed Can burn skin or eyes on contact

NEVER attempt to identify an acid or base in the lab by taste or feel!

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PH SCALE

pH Scale: a number scale for measuring how acidic or how basic a solution is

Acids: have a pH of less than 7 when dissolved in water

Bases: have a pH of more than 7 when dissolved in water

Neutral: has a pH of 7 (not an acid or a base)

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PH OF COMMON SUBSTANCES

The more acidic a solution is, the lower the pH Lemon juice – pH 2 Tomato juice – pH 4

The more basic (or alkaline) a solution is, the higher the pH Think of alkaline Earth metals includes Ca

and Mg which are basic when they react in water

Soap– pH 10 Oven Cleaner – pH 13

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Neutral substances are neither acidic nor basic Pure Water – pH 7 Saliva – pH 6.5-7.4 Human blood – pH of 7.3

to 7.5 (slightly basic)

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USING THE PH SCALE

1 unit of change represent a 10 times change in the degree of acidity/basicity

Q: What is the increase in acidity if the pH drops from 6 to 4?

A: A 2 unit drop is a 10² or 100 times increase in acidity!

IMPACT: Even a small increase in acidity harms coral reefs and organisms that require a specific pH level to survive (ex. organisms that use calcium to make their shells)

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PH INDICATORS

Many common acids and bases form colourless solutions (look like water)

pH Indicators: chemicals that change colour depending on the pH of the solution they’re placed in

So what are some common indicators you could use?

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1. LITMUS PAPER Litmus is extracted from lichens and dried

onto thin paper strips 2 forms: RED and BLUE

When BLUE litmus paper is placed in an acidic solution the paper will turn red

When RED litmus paper is placed in a basic solution it will turn blue

Can use both to tell if something is neutral BLUE will stay blue and RED will stay red

HELPFUL HINT! BAR = Blue + Acid Red

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2. UNIVERSAL INDICATOR

Contains many indicators that turn different colours depending on a solution’s pH

Uses a digital pH meter or pH computer probe to measure the electrical property of the solution, determining its pH

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3. OTHER PH INDICATORS

Not all indicator change colour at pH 7 like litmus

Phenolphthalein: colourless in acidic/slightly basic solutions but turns PINK in moderately-highly basic solutions

Bromothymol blue, indigo carmine, methyl orange, and methyl red all named after their colour change Methyl orange: changes from red to yellow over

pH of 3.2-4.4

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ACIDS

Can sometimes identify acids by their chemical formulas

Many compounds (HCl) take on acid properties after mixing with water

Ex.: HCl dissolved in water is written as HCl (aq), where (aq) means “aqueous” or “dissolved in water to make a solution

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ACIDS - 2

Chemical formulas usually have an “H” (hydrogen) on the left side of the formula HCl (aq)

In acids that contain CARBON, “H” may be written on the right side CH₃COOH (aq)

If no state of matter is given, the name may be given beginning with “Hydrogen” Hydrogen chloride

If the acid is aqueous (ex. HCl (aq)), a different name is used that ends in “-ic acid” Hydrochloric acid

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NAMING ACIDS

Basic pattern when “O” (oxygen) is present Names that begin in “hydrogen” and end in “-ate”

are changed by dropping “hydrogen” from the name and changing the suffix to “-ic acid”

Ex.: Hydrogen carbonate carbonic acid

Names that begin with “hydrogen” and end with “-ite” change by dropping the hydrogen and replacing the suffix with “-ous acid”

Ex.: Hydrogen sulphite sulphurous acid

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Basic pattern when “O” (oxygen) is absent Combine the 2 element names, then

replace the ending with “-ic acid” Ex.: hydrogen fluoride hydrofluoric

acid Ex.: hydrogen iodide hydriodic acid

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The chemical formula of an acid usually starts with hydrogen (H). Acids with a carbon usually have the C written

first. HCl(aq) = hydrochloric acid, HNO3(aq) = nitric acid,

CH3COOH(aq) = acetic acid Naming acids

Hydrogen + …-ide = hydro…ic acid HF(aq) = hydrogen fluoride = hydrofluoric acid

Hydrogen + …-ate = …ic acid H2CO3(aq) = hydrogen carbonate = carbonic acid

Hydrogen + …-ite = …ous acid H2SO3(aq) = hydrogen sulphite = sulphurous acid

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BASES

Usually written with an “OH” on the right side of the formula

Some bases are much stronger than others Magnesium hydroxide founds in antacids

while sodium hydroxide is found in drain cleaner

Caustic: solutions made from highly reactive bases

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BASES - 2

Examples of common bases: NaOH(aq)

Mg(OH)2(aq)

Ca(OH)2(aq) NH4OH(aq)

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PRODUCTION OF IONS

Acids and bases can conduct electricity because they release ions in solution. Acids release hydrogen ions, H+

Bases release hydroxide ions OH–

The pH of a solution refers to the concentration of H+ (aq) ions it has.

Concentration of H+ ions refers to the number of H ions in a specific volume

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Square brackets are used to signify concentration, [H+], [OH–]

High [H+] = low pH, very acidic High [OH–] = high pH, very basic

A solution cannot have BOTH high [H+] and [OH–]; they cancel each other out and form water. This process is called neutralization.

H+ + OH– H2O

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Environmental Example: After the mining of minerals, the remaining

ground rock (tailings) are usually deposited in a tailings pond

The tailings can release acids, lowering the pH of the water and affecting the environment

Can counteract this problem by adding a base to raise the pH level back to normal

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PROPERTIES OF ACIDS AND BASES


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