Acids and bases Flashcards
Arrhenius’s theory of Acids
Compounds that ionise in water to form H+ ions (molecular compound that forms ions)
What is a strong acid
Acid that dissociates and releases all of its hydrogen ions (single arrow)
What is a weak acid
Acid that only partially releases hydrogen ions (double arrow)
Examples of strong acids
H2SO4, HBr, HI, HNO3, HClO4, HCL
Types of acids
polyprotic, monoprotic, diprotic, triprotic
Polyprotic
Describes any acid that is capable of donating more than 1 proton
Monoprotic
Donate 1 proton
Diprotic
Donate 2 protons
Triprotic
donate 3 protons
Arrhenius theory of bases
Compounds that dissociate in water (forms hydroxide ions)
What is a bases strength dependent on
Dependent on the concentration of ions in solution and ability to accept hydrogen ions (protons) from an acid
describe a strong base
Releases hydroxide ions in solution, don’t accept protons easily
Weak base
partially ionise into hydroxide ions in solution
Example of strong bases
All group 1 and 2 SOLUBLE hydroxides, Ca(OH)2 and Mg(OH)2 even though they have low solubility
Properties of acids
Turn litmus paper from blue —> red, electrical conductors, pH of less than 7, sour, corrosive
Properties of bases
Turn litmus paper from red —> blue, electrical conductors, pH of more than 7, bitter, caustic and slippery
pH scale
Measure of the amount of alkalinity or acidity in solution, Measure of the amount of protons (hydrogen ions) that are present in an aqueous solution
How does the pH scale work
less than 7- acidic
7 or 8- neutral
9 or more- basic
Indicators
weak acid or base that change colour based on the pH of a substance
Universal indicator
mixture of several indicators, displays a variety of colours over the pH scale (allows a range of 1-14)
Electrolytes
ions in a solution
Dissociation
producing ions in a solution (ionic solids where the ions already present are separated)
Ionisation
covalent substances where the solid reacts to form ions
Strong electrolytes
Exist completely as ions when dissolved in solution, High electrical conductivity in solution, All soluble ionic compounds (HCl, H2SO4, HNO3, AgCl, Mg(OH)2)