HONORS: Acids & Bases

Acid

a substance that increases the hydrogen ion (H+) concentration in a solution

Acid

These taste sour, can conduct an electric current in an aqueous solution, and have a pH below 7

Acid

These react with carbonates to produce carbon dioxide gas

Acid

These react with active metals to produce hydrogen gas

Acid

Turns blue litmus paper red

Acid

These neutralize bases

Dissociation/Ionization

Ions separate in solution

Monoprotic Acid

Produces one hydrogen ion in an aqueous solution since it contains 1 hydrogen in the chemical formula (Examples include HCl, HNO3, HC2H3O2)

Diprotic Acid

Produces two hydrogen ions in an aqueous solution since it contains 2 hydrogens in the chemical formula (Examples include H2SO4, H2CO3)

Triprotic Acid

Produces three hydrogen ions in an aqueous solution since it contains 3 hydrogens in the chemical formula (Examples include H3PO4)

Hydronium ion

Formed when hydrogen ions are attracted to surrounding water molecules (H3O+)

Base

Substance that produces hydroxide ions in an aqueous solution

Base

These taste bitter & feel slippery, can conduct can conduct an electric current in an aqueous solution, and have a pH above 7

Base

Turn red litmus paper blue

Base

These neutralize acids

Base

These can react with a fat or oil to form soap

Monobasic base

Produces one hydroxide ion in an aqueous solution since it contains 1 hydroxide in the chemical formula (Examples include NaOH and KOH)

Dibasic base

Produces two hydroxide ions in an aqueous solution since it contains 2 hydroxide ins the chemical formula (Examples include Mg(OH)2 and Ba(OH)2)

Strong acid

Ionize completely into hydrogen ions and negative ions (Examples include HCl, HNO3 and H2SO4)

Weak acid

Ionize slightly in solution, where only a few acid molecules dissociate into hydrogen ions and negative ions (Examples include H3PO4, H2CO3, H2SO3, HNO2 and HC2H3O2)

Strong base

Ionize completely into positive ions and hydroxide ions (Examples include KOH, NaOH, LiOH and Ba(OH)2)

Neutralization Reactions

A reaction between an acid and base that forms a salt and water

Anhydrous

Without water

Acid Anhydride

A non-metal oxide that reacts with water to form an acidic solution (acid)

Acid Anhydride

SO2, NO2, N2O5 are examples of this type of anhydride

Base Anhydride

A metallic oxide that reacts with water to form a basic solution (base)

Base Anhydride

CaO, MgO, Na2O are examples of this type of anhydride

Indicators

Changes the color of solution based on pH identifying an acidic or basic solution (Examples include phenol red, litmus paper, phenolphthalein)

Buffers

Able to resist small changes in pH but cannot prevent pH changes

Buffer

Made by mixing a weak acid with its conjugate base or by mixing a weak base with its conjugate acid

Conjugate base

Substance that remains after hydrogen ions has been released by the acid

Conjugate acid

Substance formed when the base acquires hydrogen ions from the acid

Acidosis

A condition where blood pH is below 7.34

Acidosis

A condition brought on by failure to expel carbon dioxide from your lungs, like with pneumonia or a heart attack

Acidosis

A condition that increases the amount of carbon dioxide in the body ultimately increasing the amount of carbonic acid in the blood

Alkalosis

A condition where blood pH is higher than 7.45

Alkalosis

A condition brought on by releasing too much carbon dioxide from your lungs, like during hyperventilation

Alkalosis

A condition that decreases the amount of carbon dioxide in your body and ultimately decreases the amount of carbonic acid in the blood

Titration

An analytical process used to determine the unknown concentration (molarity) of a solution

Standard Solution

The solution in a titration of known concentration

End point

Point in titration where the solution changes color

Equivalence point

Point in titration where the number of moles of the base are equal to the number of moles of the acid

Electrolytes

Can conduct an electric current in an aqueous solution

pH

Used to express the concentration of an acid or base by calculating the amount of hydrogen or hydronium ions in the solution

pOH

Used to express the concentration of an acid or base by calculating the amount of hydroxide ions in the solution

Bicarbonate Buffer System

Naturally found in the body to help maintain the pH level of our blood between 7.35-7.45

Acid Rain

Rain containing acids that form in the atmosphere when pollutants, like nitrogen oxides and sulfur oxides, combine with water

Weak base

Ionize slightly in solution, where only a few base molecules dissociate into positive ions and hydroxide ions (Examples include NH3, CaCO3, Mg(OH)2, NaHCO3 and Ca(OH)2)

pH

power of hydrogen

pOH

power of hydroxide

Acid rain

rain that has a pH lower than 5.6

Molarity

moles of solute/liters of solution

Nucleic acid

Made from acidic and basic components (Examples include DNA and RNA)

Amino acids

a simple organic compound containing both a carboxyl (—COOH) and an amine (—NH2) group.

Amino acids

Combine to form proteins (there are 10-400 amino acids in each protein)

Amino acids

Are weak organic acids (20 different types and 10 are essential)

Carboxylic acid group

O=C-OH

Amine group

NH2

Proteins

Long chains of amino acids (proteins are made in the ribosomes of cells and are connected by peptide bonds)

Peptide bond

The chemical bond that forms between the carboxyl group of one amino acid and the amine group of another amino acid

Condensation reaction

a chemical reaction in which two or more molecules combine to produce water

Dipeptide

Two amino acids bonded together

Fatty acid (saturated)

A long chain hydrocarbon in which all carbons in the hydrocarbon are connected by single bonds and it ends in a carboxylic acid group (these long chains are non-polar)

Fatty acid (unsaturated)

A long chain hydrocarbon in which at least one double bond occurs between the central carbons and it ends in a carboxylic acid group (these long chains are non-polar)

Glycerol

A three-carbon alcohol to which fatty acids are covalently bonded to triglycerides

Glycerol

a three-carbon alcohol with a hydroxyl group attached to each carbon

Triglycerides

an compound, formed through a condensation reaction, made up of a single molecule of glycerol and three molecules of fatty acids (can be saturated or unsaturated)