Chapter 11 - Acids & Bases Flashcards
Accuracy
How close a measured value is to its actual value.
Properties of Acids
- sour taste
- turn litmus paper red
- pH below 7
- corrosive
- conduct electricity in solution
- donate a proton
Acidic Proton
The proton which is donated in an acid base reaction.
Alkali
A base which dissolves in water, such as sodium hydroxide.
Amphiprotic
A substance that can act as both an acid and base, such as water. (Note: contain H and have a non-bonding pair).
Properties of Bases
- bitter taste
- turn litmus paper blue
- pH above 7
- caustic (and corrosive)
- conduct electricity in solution
- receives proton
Bronsted-Lowry Theory
An acid base theory which states that an acid is a substance that donates a hydrogen ion, and a base is a substance that receives a hydrogen ion.
Calcification
The process used by sea creatures to absorb calcium and carbonate ions in sea water to form calcium carbonate shells.
Conjugate Base
An acid that has lost an H+ ion.
Conjugate Acid
A base that can gained an H+ ion.
Decalcification
The deterioration of sea creature shells due to lack of calcium, most likely caused by the increasing number of hydronium ions reacting with carbonate in seawater.
Diprotic Acid
An acid that can donate 2 protons, in 2 reactions.
Hydronium Ion
H3O+
Hydroxide Ion
OH-
Indicator
A substance that changes colour in certain pHs. (e.g. red cabbage).
Monoprotic Acid
An acid that can only donate 1 proton, such as HCl.
pH
A logarithmic scale measuring the concentration of hydronium ions in a solution. (<7 is acidic; >7 is basic).
Polyprotic Acid
An acid that can donate more than one proton, via multistage reactions.
Precision
How closely a set of measurements agree with each other. (e.g. 21.95, 21.96, 21.93).
Tripotic Acid
An acid that can donate 3 protons, in 3 reactions.
Strong Acids
Hydrochloric Acid (HCl)
Sulfuric Acid (H2CO3)
Nitric Acid (HNO3)
Weak Acids
Ethanoic Acid (CH3COOH)
Carbonic Acid (H2CO3)
Phosphoric Acid (H3PO4)
Strong Bases
Sodium Hydroxide (NaOH)
Potassium Hydroxide (KOH)
Calcium Hydroxide (Ca(OH)2)
Weak Bases
Ammonia (NH3)
Acid + Metal Hydroxide Formula
Acid + Metal Hydroxide → Salt + Water
Neutralisation Reaction
The reaction between an acid and a base, resulting in the formation of a salt, water, and a neutral pH (sometimes).
Acid + Metal Carbonate Formula
Acid + Metal Carbonate → Salt + Water + Carbon Dioxide
Acid + Metal Hydrogen Carbonate Formula
Acid + Metal Hydrogen Carbonate → Salt + Water + Carbon Dioxide
Acid + Metal Formula
Acid + Metal → Salt + Hydrogen Gas
Self Ionisation of Water
The slight reaction water has with itself, due to its ability to act as both an acid and a base.
Acidity
The measure of the concentration (in molar) of hydronium ions present in a solution.
Ionic Product of Water
[OH-][H3O+] = 1.0 x 10^-14 (at 25°C)