Dilution Of Acids And Alkalis Flashcards
Dilution of acids and alkalis
During dilution of a solution the number of particles (ions or molecules) of solute in every cm3 decreases.
When an acid is diluted by a factor of 10 the pH increases by a factor of 1
When an alkali is diluted by a factor of 10 the pH decreases by a factor of 1
Dilution and water
Pure water is a very poor conductor of electricity. This shows water contains ions.
The very low conductivity shows water contains a very small number of ions
This shows that pure water contains a very small number of H+ and OH- ions
Acids contains more H+ ions than is present in pure water
Alkalis contain more OH- ions than his present in pure water
Diluting an acid or alkali decreases the concentration of H+ or OH- to bring them down to the same concentration as present in pure water
Conductivity in water
The low conductivity of water shows very few molecules dissociate (break up) to form ions.
Pure water is neutral because there are equal numbers of H+ and OH- ions
This reaction is called the dissociation of water. This means all solutions contain small numbers of H+ and OH- ions
Conductivity of acids
All acids conduct electricity meaning acidic solutions must be ionic
When they dissolve in water they dissociate into ions
All acids contain hydrogen and form hydrogen ions when dissolved in water
Hydrogen ions are positively charged meaning they are attracted to the negative electrode and form hydrogen gas
Types of acids
Citric acid Folic acid Lactic acid Tartaric acid Ethanoic acid Ascorbic acid Amine acids Fatty acids
All acids contain the hydrogen ion
Alkali ionic formulae
Metal hydroxides have ionic bonding
When an ionic compound is melted or in solution the ions are free to move the + is inserted between the ions in a formula to show they have moved apart
Neutralisation
When an acid and alkali are mixed together they cancel each other out and the pH moves towards 7. This is called neutralisation.
A neutralisation reaction is one in which a base reacts with an acid to form a salt and water.
Types of salt
Hydrochloric acid - chloride Nitric acid - nitrate Sulfuric acid - sulfate Sulfurous acid - sulfite Carbonic acid - carbonate Ethanoic acid - ethanoate