• Acid and base are terms used by chemists to classify chemicals according to their pH.

• ACID - A class of compounds whose water solutions taste sour, turn blue litmus to red, and react with bases to form salts.

Acids generally give up a hydrogen ion (H+) in solution.

• BASE - A class of compounds that taste bitter, feel slippery in water solution, turn red litmus to blue, and react with acids to form salts.

Bases generally create hydroxide ion (OH-) in solution.

• NEUTRAL - These are items that are neither acids or bases.

• There are 4 main ways to determine if a substance is an acid or a base. They are: Red litmus paper, Blue litmus paper, a pH meter, and Red Cabbage Juice.

• Acids and bases neutralize each other. This reaction called neutralization produces water and a salt.

Title: Acids, Bases, and Salts

Acids and Bases• Acid and base are terms used by chemists

to classify chemicals according to their pH.

• The pH is the negative logarithm of the hydronium ions (H3O+) ion concentration of an aqueous solution; used to express acidity.

• Low pH has high a concentration of H3O+ and high pH means low concentration of H3O+.

• pH is the measure of the acidity or basicity of a solution.• The pH scale ranges from 0 to 14. • 0 through 6 being acidic.• 7 is considered neutral .• 8 through 14 being basic.

the negative logarithm of the hydronium ions (H3O+) ion concentration of an aqueous solution; used to express acidity. Low pH has high a concentration of H3O+ and high pH means low concentration of H3O+.

A class of compounds whose water solutions taste sour, turn blue litmus to red, and react with bases to form salts, generally give up a hydrogen ion (H+) in solution.

.

Acids produce solutions that:

• Taste sour

• Turn blue litmus paper red

• Conduct electricity

• react with metals to liberate a hydrogen gas

• are corrosive (to corrode means to wear away, corrosion, acid rain)

• lose the above properties when reacted with a base.

Examples of acids:

• Vinegar

• Lemon Juice

• Soft Drink

• Battery Acid

• Stomach Acid

• Apple Juice

• Black Tea

• Strong Acids – any acid that dissociates completely in aqueous solution.

• Weak Acids – any acid that dissociates only partially in aqueous solution.

Strong Acids Weak Acids

1. chloric acid, HClO3

2. hydorbromic acid, HBr

3. hydorchloric acid, HCl

4. sulfuric acid, H2SO4

5. nitric acid, HNO3

1. acetic acid, Ch3COOH

2. boric acid, H3BO3

3. hydorfluoric acid, HF

4. phosphoric acid, H3PO4

5. sufurous acid, H2So3

A class of compounds that taste bitter, feel slippery in water solution, turn red litmus to blue, and react with acids to form salts, generally create hydroxide ion (OH-) in solution.

Bases produce solutions that:

• taste bitter

• turn red litmus blue

• conduct electricity

• feel slippery

• are corrosive (basic solution in glass container)

• lose the above properties when reacted with an acid.

Examples of bases:

• Detergent

• Baking Soda

• Drain Cleaner

• Ammonia

• Soaps (hand, dish)

• Antacid

• Strong Bases – any base that dissociates completely.

• Weak Bases – any base that dissociates only partially in aqueous solution.

Strong Bases Weak Bases

1. barium hydroxide, Ba(OH)2

2. calcium hydroxide, Ca(OH) 2

3. potassium hydroxide, KOH

4. sodium hydroxide, NaOH

5. trisodium phosphate, Na3PO4

1. ammonia, NH3

2. aniline, C6H5NH 2

3. potassium carbonate,K 2 CO3

4. sodium carbonate, Na 2 CO3

5. trimethylamine, (CH3) 3N

• These are items that are neither acids or bases.

• Neutral items will turn blue and red litmus paper green.

• The main example of a neutral item is: Pure Water, and Salts

Physical Properties of Acids & Bases

• ACIDS• Acids taste sour (e.g. vinegar, lemon juice).• Acids are harmful to living cells.• Aqueous solutions of all acids contain hydrogen ions.• Acid turns blue litmus red.• Strong acids are corrosive.

• BASES• Alkalis are taste bitter• Strong alkalis are corrosive.• Aqueous solutions of all alkalis contain hydroxide ion.• Alkalis turns red litmus blue.• Soapy touch.

Chemical Properties of Acids

With metals•Metals above copper in the reactivity series will react with acids, giving off hydrogen gas, forming a salt.Mg(s) + H2SO4(aq) MgSO4(aq) + H2(g)

With bases (metal oxides and hydroxides)•The base dissolves in the acid and neutralizes it. A salt is formed.

H2SO4(aq) + CuO(s) CuSO4(aq) + H2O(l)

With metal carbonates•With metal carbonates, effervescence occurs, salt, water and carbon dioxide gas is produced.

2HCl(aq) + CaCO3(s) CaCl2(s) + H2O(l) + CO2(g)

USES OF ACIDS• HCl in stomach

• H2SO4 in car batteries, as drying agent’

• HNO3 in manufacturing of fertilizers

• Ethanoic acid in food industry

• Fatty acids in soap making

• Ascorbic acid in medicine

Chemical Properties of Bases

• Neutralization.

• Ammonium salts are decomposed when mixed with a base e.g. sodium hydroxide. The ammonia is readily detected by its pungent odor (strong smell) and by turning damp red litmus blue.

NaOH + NH4Cl ==> NaCl + H2O + NH3  Ionically: NH4

+ + OH- ==> H2O + NH3 

– This reaction can be used to prepare ammonia gas and as a test for an ammonium salt.

• Red litmus paper

• Blue litmus paper

• pH

• Red Cabbage Juice

•Robert Boyle discovered litmus paper

•certain plant extracts, such as litmus, can be used to distinguish acids from bases.

• blue and red litmus paper turn red when dipped in an acid

• red and blue litmus paper turn blue when exposed to a base

• pH is the measure of the acidity or basicity of a solution.• The pH scale ranges from 0 to 14. • 0 through 6 being acidic.• 7 is considered neutral .• 8 through 14 being basic.

the negative logarithm of the hydronium ions (H3O+) ion concentration of an aqueous solution; used to express acidity. Low pH has high a concentration of H3O+ and high pH means low concentration of H3O+.

• red cabbage can be used as an acid/base indicator

• after boiling the red cabbage, pour a small amount of the juice into a small sample of a substance your checking

• the juice will turn blue if the substance is a base

• the juice will turn red if the substance is an acid

What happens when you mix an acid and a base?

• When an acid and a base are mixed, they react to neutralize each other, this is called neutralization.

• This results in the formation of water and a salt.

• A salt is any ionic compound that results from a neutralization reaction.

• Since salts are made of ions, they share the same properties of ionic compounds, including crystal shape, high melting points and boiling points, and electric conductivity.

What happens when you mix an acid and a base?

USES OF SALTSS. No. SALT USE

1 Ammonium Chloride In torch batteries

2 Ammonium Nitrate In fertilizers

3 Calcium Chloride As drying agent

4 Iron Sulphate In Iron tablets

5 Magnesium Sulphate In medicine

6 Potassium Nitrate In gunpowder etc.

7 Silver Bromide In photography

8 Sodium Chloride Making NaOH

9 Sodium Stearate In making soap.

There are three common acid-base theories:

• the Arrhenius theory

• the Bronsted-Lowry theory

• the Lewis theory

• Svante Arrhenius was a Swedish chemist.

• In 1887, he published a paper concerning acids and bases.

• He concluded that solutions with acids and bases in them released particles when dissolved.

• He concluded that acids were substance which separated (ionized) in water solution to produce hydrogen ions (H+, or free protons).

• He also believed that bases were substance which ionized to produce hydroxide ions (OH-) in water solution.

• HCl H+ + Cl-

• NaOH Na+ + OH-

• T. M. Lowry was an English scientist, while J. N. Bronsted was a Danish scientist.

• In 1923, they independently proposed a new definition of the terms acid and base.

• They stated that in a chemical reaction, any substance which donates a proton is an acid and any substance which accepts a proton is a base.

• When hydrogen chloride gas is dissolved in water, ions are formed:

• HCl + H2O H3O+ + Cl-acid base

BronstedLowry

• Gilbert Newton Lewis was and American chemist.

• In 1923, proposed an even broader definition of acids and bases.

• Lewis focused on electron transfer instead of proton transfer.

• He defined and acid as an electron-pair acceptor, and a base as an electron-pair donor.

• This definition applies to solutions and reactions which do not even involve hydrogen or hydrogen ions.

THEORY ACID DEFINITION BASE DEFINITION

Arrhenius Theory

Bronsted-Lowry Theory

Lewis Theory

Any substance which releases H+ ion in water solution.

Any substance which donates a proton.

Any substance which can accept an electron pair.

Any substance which releases OH- ions in water solution.

Any substance which accepts a proton.

Any substance which can donate an electron pair.

• Proteins in your hair, nails, cell membranes, and other parts of you body consist of amino acids.

• Enzymes that catalyze reactions in your body are composed of amino acids.

• Hydrochloric acid is in your stomach to aid in the digestion of food.

• Organic bases are major components of DNA and products of the digestion of proteins.

• DNA contains thousands of sites where H+ ion transfer can take place

• Therefore DNA fits the definition of a Bronsted acid.

• DNA is a weak acid, but it is stronger than phosphoric acid.

• ACID - A class of compounds whose water solutions taste sour, turn blue litmus to red, and react with bases to form salts.

• BASE - A class of compounds that taste bitter, feel slippery in water solution, turn red litmus to blue, and react with acids to form salts.

• NEUTRAL - These are items that are neither acids or bases. There are 4 main ways to determine if a substance is and acid or a base. They are: Red litmus paper, Blue litmus paper, pH, and Red Cabbage Juice.

• Background information on acids and bases. <http://educ.queensu.ca/~science/main/concept/chem/c10/C10CDMJ1.htm>

• Acids and Bases. <http://www.bookrags.com/research/acids-and-bases-woc/>

• Acids and bases Lab. <http://www. Scribd.com/doc/2977162/Acids-and-Bases-Lab/>

• Smoot, Robert C.; Price, Jack S.; Smith, Richard G. Chemistry A Modern Course. Chapter 24, Acids, Bases, and Salts.

• Holt, Rinehart, and Winston, Inc. Chemistry Visualizing Matter. Chapter 13, Acids and Bases.