Define Acids and bases according to the Bronsted-Lowry and Lewis Theories
Bronsted-Lowry Acid- A substance that acts as an H+ donor
Bronsted-Lowry Base- A substance that acts as an H+ receptor (must have a lone pair to create the dative covalent bond.
Lewis Acid- A substance that acts as a lone pair receptor
Lewis Base- A substance that acts as a lone pair donor
When acids react with bases, it forms a dative covalent bond
Why? Because the base has a lone pair of electrons while the proton has none, so both are donated when the bond is carried out
Ligands in complex ions are lewis bases
Deduce whether or not a species could act as a Bronsted-Lowry and/or a Lewis Acid
Deduce the formula of the conjugate acid (or base) of any Bronsted Lowry acid/base
Conjugate base- The substance that remains when an acid loses an H+ ion
Conjugate acid- The substance that remains when a base gains an H+ ion
Ex. H2CO3 + NaOH à Na+ + HCO3- + H2O
Amphitropic- Species that can act as either an acid or a base (example, water)
Ex. 2H2O à H3O+ + OH-
Helpful Terminology:
Monoprotic- Acids and bases that can only gain/lose ONE H+ ion
Diprotic- Acids and bases that can gain/lose TWO H+ ions
Polyprotic- Acids and bases that can gain/lose MULTIPLE H+ ions
Outline the characteristic properties of acids and bases in aqueous solutions
Acids turn litmus paper red
Bases turn litmus paper blue
Alkalis- Bases that dissolve in H2O
Acid + Active metals à Salt and H2 gas
Acid + base à Salt and H2O
Heat is also released as this reaction is exothermic
Acid + [hydro]carbonates à Salt, H2O, and CO2
Acids usually have an H+ somewhere
Bases usually have OH-
Distingush between strong and weak acids and bases in terms of the extent of dissociation, reaction with water, and electrical conductivity
Strong Acid is one that dissociates almost completely in water
Strong Base is one that dissociates almost completely in water
When shocked with electricity, strong acids and bases conduct very well in water
Weak acids dissociate poorly in water
Weak bases dissociate poorly in water
When shocked with electricity, weak acids and bases conduct poorly with water
State whether a given acid or base is strong or weak
Examples of Strong Acids: HCl, H2SO4, HNO3
Examples of Weak Acids: Carbonates, carbonic acid (aqueous CO2), Organic Acids (ethanoate + cyanide) , Intermediate Acids (conjugate bases),
Examples of Strong Bases- Anything with hydroxides
Examples of Weak Bases- Amines, carbonates, and anions of weak acids
Distinguish between strong and weak acids and bases, and determine the relative strengths of the acids and bases using experimental data
Strong acids and bases react faster than weak acids and bases. This means that any thing used to identify an acid-base reaction (color change, temperature change, gas formation) will be quicker with a stronger base
Distinguish between aqueous solutions that are acidic, neutral, or alkaline using the pH scale. AND Identify which of the two or more aqueous solutions is more acidic or alkaline using pH values
pH stands for power hydrogen, and is a logarithmic representation of the amount of H+ in the equilibrium
pH = - log [H+] [H+] = 10-pH
If pH > 7, the solution is acidic
If pH < 7, the solution is basic
If pH = 7, the solution is neutral
State that each change in one pH unit represents a 10-fold change in [H+] AND deduce changes in [H+] when the pH of a solution changes by more than one pH unit.
When pH increases by a power of 1, H+ decreases by a power of 10 (they are negative logs, remember???)
When pH increases by x, [H+] increases by 10X
When pH decreases by x, [H+] decreases by 10X
Thanks, really quick review. But acids have pH <7
ReplyDeleteand bases are > 7
Yeah. Thats a mistake. Good notes though.
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