Topic

Common Strong Acids

Common Alkalis

Hydrochloric Acid (Strong Acid)

HCl

Sulphuric Acid (Strong Acid)

Nitric Acid

HNO3 (Strong Acid)

H2SO4

Acetic Acid (Strong Acid)

Melting point: -42 °C

Boiling point: 83 °C

Boiling point: -85.05 °C

Melting point: Concentration-dependent

Boiling point: 337 °C

Melting point: 10 °C

CH₃COOH

Boiling point: 118 °C

Melting point: 16.6 °C

Sodium Hydroxide

Ammonia

Lime Water

Ca(OH)2

NaOH

Method for Preparing insoluble salts

NH3

Moderate Alkalinity

High Alkalinity

Moderate Alkalinity

Definitions

Strong Acid: An acid solute that completely dissociates completely into ions when dissolved.

Alkali: A solution which contains excess OH^- ions, turns litmus paper blue and has a PH of more than 7.

Acid: Acids are molecular compounds that dissolve in water to produce hydrogen ions and an anion. Bases are ionic compounds consisting of hydroxide ions and a cation.

1) Grab your goggles to protect your eyes.

2) Mix the silver chloride solution with the sodium chloride solution in the beaker and then filter the mixture.

3) Rinse the beaker with some bits of distilled water so that the solution can easily slow and then pour this through the funnel.

4) Pour a little amount of distilled water over the precipitate in the funnel.

5) Carefully remove the filter paper containing the precipitate and dry it in a warm oven or out in the sun.

Reactivity Series (As you go down the list, the reactivity decreases)

Potassium

Sodium

Calcium

Magnesium

Aluminium

Carbon

Method for Preparing a salt from insoluble base

1) Gently heat 40ml of sulphuric acid

Zinc

Iron

Tin

Lead

Hydrogen

Copper

Silver

Gold

2) In the beaker add copper oxide(one spatula at a time), until no more will dissolve – you will see excess black powder in beaker.However, make sure you calmly stir it.

3) Allow beaker to cool and then pass through filter paper into conical flask.

4) Evaporate filtered solution over your bunsen burner.

Indicators

Methyl Orange

Phenolphthalein

Litmus Paper

Acid: Red

Alkali: Blue

Acid: Red

Alkali: Yellow

Acid: Colorless

Alkali: Pink

Salts: Salts are ionic compounds that consists of the positive ion (CatIon) of a base and the negative ion (Anion) of an acid.


Neutrelisation: A chemical reaction where an acid and a base react together.


Base: A base is a substance that can neutralize the acid by reacting with hydrogen ions.

Reactions of acids

Acid + Metal Hydroxide -------> Salt + Water

Acid + metal -------> Salt + Hydrogen

Acid + Metal Oxide -----> Salt +Water

Solubility

Common Salts of sodium, potassium and ammonium

Nitrates

Chlorides

Common sulphates

Common Carbonates and Hydroxides

Insoluble (except for sodium, sodium potassium and ammonium)

PH Scale

Soluble (except silver chloride and lead chloride)

Soluble

Soluble

Soluble (Except lead, barium and calcium sulphate

Acid + Metal Carbonate ------> Salt + Water + Carbon Dioxide

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PH 0-6 Acidic

PH 8-14 Alkaline

PH 7 Neutral

Method for making soluble salts

1) Measure out a set amount of acid into a chronicle flask using a pipette.

2) Add a few drops of indicator

3) Slowly add alkali to the acid, using a burette until you reach the endpoint, this is when the acid has been completely neutralized and the indicator changes color

3) Carry out the reaction using exactly the same volumes of acid and alkali but with no indicator. So the salt wont be easily contaminated with the indicator.

4) The solution that remains when the reaction is complete contains only salt and water

Slowly evaporate some of the water and then leave the solution to crystallise.