Titrations and Titration curves

Strong acid into strong base

Neutral equivalence point

Strong base into strong acid

Neutral equivalence point

Weak acid into strong base

Basic equivalence point

Strong base into weak acid

Basic equivalence point.

Weak base into strong acid

Acidic equivalence point

Strong acid into weak base

Acidic equivalence point.

Weak acid pH

3

Weak base pH

9

Strong acid pH

1

Strong base pH

13

titration

is a method of determining the concentration of a solution by reacting a known volume of that solution with a solution of known concentration

titrant

the solution of known concentration that is added to the burette

Burette

measuring instrument consisting of a graduated glass tube with a tap at the bottom

Pipette

A glass or transparent plastic tube used to accurately measure small amounts of liquid

hydronium ion

H₃O⁺

hydrogen ion

H⁺

hydroxide ion

OH⁻

Neutralisation reaction

an acid and a base in an aqueous solution react to produce a salt and water

Neutralisation ionic equation

H⁺ (aq) + OH⁻ (aq) ⇌ H₂O (l)

salt

an ionic compound made up of a cation from a base and an anion from an acid

Neutral salt

results from reaction of strong acid and strong base

Acidic salt

results from reaction of strong acid and weak base

Basic salt

results from reaction of weak acid and strong base

Acid-base indicator

a compound whose colour is sensitive to pH

Equivalence point

the point at which moles of hydrogen ions from the acid equal the moles of hydroxide ions from the base

End point

the point at which the indicator that is used in titration changes colour

Phenolphthalein

acid/neutral = colourless; basic = pink

concurrent

agreeing or consistent

Acid + Base

salt + water

Acid + Metal

salt + hydrogen gas

Acid + metal carbonate

salt + water + carbon dioxide

neutralisation complete equation

acid + base ⇌ salt + water

titration curve

A graph of pH vs volume of titrant added.