Water Flashcards
Bronsted Lowry acid
Acids are proton donors (can donate H+ ions)
Bronsted Lowry base
are proton acceptors (accepts H+ ions)
Common acids names and formulas
HCl, H2SO4, HNO3, CH3COOH,
Common base names and formulas
NaOH, NH3, Na2CO3
Solvent:
Liquid that dissolves a substance
Solute:
Substance being dissolved
Solution:
Solvent and solute mixture
Saturated solution
asolutionin which no more solute can be dissolved in the solvent.
Unsaturated solution
a solution with less solute than the saturated solution.
Supersaturated solution
a solution with more solute than the saturated solution (i.e. some solute is unable to dissolve).
Conjugate acid
A conjugate acid is the same as the starting base plus H+.
Conjugate base
A conjugate base is the same as the starting acid minus H+.
Products of acid and metal
salt and hydrogen
Products of acid and metal carbonate
salt, carbon dioxide and water
Products of acid and metal hydroxide
salt and water
Strong acid definition and common examples
Donate protons easily
Completely ionise in solution
HCl - hydrochloric acid.
HNO3 - nitric acid.
H2SO4 - sulfuric acid.
HBr - hydrobromic acid.
HI - hydroiodic acid.
HClO4 - perchloric acid.
weak acids definition and common examples
Does not donate protons easily
Partially ionise in solution
HCOOH – methanoic acid
CH3COOH – ethanoic acid.
HF – hydrofluoric acid
HCN – hydrocyanic acid
HNO2 – nitrous acid
Calculation to find pH
pH = – log [H+]
Calculation to find [H+]
[H+] = 10^-pH
pH scale range for acids and pH scale range for bases
Each one-unit change in the pH scale corresponds to a ten-fold change in H+ concentration,
0-6 acids 7 neutral 8-14 base/alkali
Latent Heat of Fusion
the amount of heat energy required to change 1 mole of a substance from a solid to a liquid at its melting point
Latent Heat of Vaporization
the heat energy required to change 1 mole of a substance from liquid to a gas at its boiling point
