Acid and bases

I hate chemy :(

Arrhenius Theory

Acid dissolves in water to produce H+ ions

Bases dissolves in water to produce OH- ions

Problemos:

In acidic solutions H+ is not formed but H3O is formed due to hydrogen bonding

Hydrogen polyatomics + compounds neither oxides or hydroxides cannot be applied to arrhenius theory

Bronsted-Lowry Theory

Acids gives protons (H+ ions) to other reactant

Basis accepts protons (H+ ions) from other reactant

• can only be classified for a specific reason

• ambiprophic (can be both acid and base)

• product formed from base = conjugate base

• product formed from a base accepting a proton = conjugate acid

Titration

A titration lab is a quantitative analytical chemistry technique used to determine the concentration of an unknown substance (the analyte) by precisely reacting it with a solution of known concentration (the titrant).

Acid-Base titration

An acid-base titration is a quantitative chemical analysis technique that uses the neutralization reaction between an acid and a base to determine the unknown concentration of one of the solutions.

Titrant

the solution with a known concentration aka the solution in the burette

Analyte

the solution with an unknown concentration aka solution in the flask (bottom)

Burette

clear tube with volume markings along its length and a tap at the bottom

End point

the point which the indicator titration change colour ; sharp change (clear → pink)

Equivalence point

the point where the amount of titrant is just enough to react with all the reactant of analyte (Nacid = Nbase)

Indicator

used to show the change of colour when pH changes

Phenolphtalein:

0-8 = colourless

8-10 = pink

10+ = red

Types of bases

Strong base: dissociates completely in water

Weak base: a base that produces few hydroxide ions in water (does not dissociate that well)

pH scale

“power of hydrogen”

used to describe acidity or bascidity of concentrations of H+ ions

Types of acids

Strong acid: an acid that ionizes completely in water

Weak acid; an acid that ionizes very slightly in a solution

Dissociation

when ionic bonds in a compound breaks apart (dissolving)

base dissociates in water produces OH-

Ionization

When a covalent bond breaks resulting in the formation of ions that then dissociate

acid that ionizes in water produces H+ ions

Concentration

amount of solute per quantity of solvent

Strength

behaviour of compounds in a solution