17. Acids and Bases
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33 Terms
Give the formulae for: hydrochloric acid, sulfuric acid, sulfurous acid, nitric acid, phosphoric acid, ethanoic acid, carbonic acid, and citric acid.
HCl, H2SO4, H2SO3, HNO3, H3PO4, CH3COOH, H2CO3, H8C6O7.
Acid definition
A substance that donates a proton in a Bronsted-Lowry acid-base reaction.
Base definition
A substance that accepts a proton in a Bronsted-Lowry acid-base reaction.
Strong acid/base definition
A substance that ionises/dissociates essentially completely in an aqueous solution.
Weak acid/base definition.
An acid/base that only partially ionises/dissociates in an aqueous solution, where an equilibrium is established.
Concentrated solution definition
A solution containing a relatively large amount of solute per unit volume.
Dilute acid/base definition
A solution containing a relatively small amount of solute per unit volume.
What is an alkali?
A soluble base.
Give the formula for: sodium hydroxide, ammonia, calcium hydroxide (limewater)
NaOH, NH3, Ca(OH)2
Properties of acids
Contain H+ ions, turn litmus paper red, corrosive, sour, pH<7, conductive.
Properties of bases
Contains OH- ions, turn litmus paper blue, caustic, slippery, bitter, pH>7, conductive.
Dissociation definition
The process where an ionic compound breaks apart into separate, charged ions.
Ionisation definition
The process where neutral molecules react with a solvent to form charged ions.
What is the Arrhenius definition of an acid?
A substance that is ionised in water to produce hydrogen ions.
Polyprotic acid definition
Acids that can react with water to form more than one hydrogen ion per molecule.
Give an example of a monoprotic, diprotic and triprotic acid.
CH3COOH, H2SO4, H3PO4.
When is a reversible arrow (⇌)used in equations?
When both the forward and reverse reactions happen at the same time, and neither side goes completely to completion (when weak acids/bases are reacting)
What is the Arrhenius definition of a base?
A substance that dissociates in water to form hydroxide ions.
Why are acids/bases conductive?
Acids ionise to produce H+ ions and bases ionise to produce OH- ions, and these charged particles allow them to conduct electricity.
Electrolyte definition
A substance that conducts an electric current when it is melted or dissolved in water.
2 limitations of the Arrhenius model?
Doesn’t explain why some substances that don’t contain hydrogen form acidic solutions, and why some substances that don’t contain hydroxide ions form basic solutions.
Restricted to acids and bases that dissolve in water.
Give 3 examples of strong and weak acids.
Strong - HCl, H2SO4, HNO3
Weak - CH3COOH, H2CO3, H3PO4
Give 3 strong bases and 1 weak base.
Strong - NaOH, KOH, Ca(OH)2
Weak - NH3
What does the strength of an acid or base depend on?
How completely it ionises/dissociates in water - solutions of strong acids/bases contain ions with no unreacted molecules remaining.
What is the equation used to determine the pH of a solution?
pH = -log10(H+)
Acid + metal hydroxide —> ?
Salt + water
Acid + base —> ?
Salt + water
Acid + metal (hydrogen)carbonate —> ?
Salt + water + carbon dioxide
What tests are used for carbonate salts and hydrogen gas?
Limewater test for carbonate salts, pop test for hydrogen gas.
Acid + metal —> ?
Salt + hydrogen gas.
Base + ammonium salt —> ?
Salt + ammonia + water
What is an advantage of the Bronsted-Lowry theory in comparison to the Arrhenius theory?
It describes acid-base reactions as proton transfer, so it can also account for bases like NH3 which don’t contain OH ions.
2 Ways to distinguish between different strengths/concentrations of acids
Measure electrical conductivity, measure pH.