Acid-base THeory

Acids:

  • They have Hydrogen in them and this hydrogen gives its acidic properties. More specifically, its the hydronium ion that forms which gives it its acidic properties

  • This is formed by placing molecular compound in water. It then ionizes and forms a new aq products, which holds the acidic properties.

  • Has to be aq

Bases:

  • Recognized by hydroxide. This is what gives it its base properties when they are dissolved in water.

Arrhenius:

  • Acids ionize and release H+ into a solution and bases dissociate and release OH- into a soltion

Ie:

Acids: HNO —> H+ + NO3-

Bases: Ba(OH)2 —> Ba2+ + 2OH-

Revised verison:

An acid reacts with water to increase the hydronium ion concentration

A base dissolves in water to increase the hydroxide concentration

The Bronstead- Lowry concept:

  • Bronstead- Lowry acids: They give protons and the that accepts the protons is Bronstead Lowry Base.

  • Bronsted Lowry base: They accept protons

Conjugate pairs:

  • When a species behaves as an acid and the product formed is therefore capable of acting like a base

    • HCL + H2O —> H3O + Cl

  • The stregnth of the conjugate help determins if the acid is strong or weak. Strong acids ionize completely, weak acids don’t.

  • When a species as like a base its called the conjugate acids

Amiphorotic:

A compounds that can act as proton acceptor in one reaction and as a protons donor in another

Classfying acids:

The more concentrated acid is, the more dangerous it is. The strength of an acid does not include danger level.

Strong acids:

  • Ionizes completely in water

  • Halogen0containing: HCL, HI, HBr (not HF), H2SO4 HNO3, HCIO4

  • Rest of the acids are weak

Weak Acids:

  • Only a small portion of the acid ionizes and rest just dissolves into a molecular acid

Strong bases:

  • Group 1 hydroxides & group 2 hydrooxides

Weak bases:

Organis molecules that have nitrogen atoms with lone pairs of electrons that can act like BL bases and take protons from water

Reactions of Acids and Bases:

  • Acids and bases neutralize eachother and from water and an ionic compound

  • Acids can be synthesized by adding a non-metal oxide to water (H2SO4 + 2NaOH —> Na2SO4+ 2H2O)

  • Acids react with metal to produce hydrogen gas and a new ionic compound

  • Acids react with carbonate compounds to produce an inoic compound, carbon dioxide, and water

  • Acids react with hydrogen carbonate compounds to produce an ionic compound, carbon dioxide, and water.

  • Bases may be synthesized by the reaction of metal oxide and water

  • Placing a metal oxide in an acid it will react with water first and then neautralization will occur based on the solubility.

Lewis Acids and Bases:

  • Lewis acid is an electron pair acceptor & Lewis base is an electron pair donor

  • Ie. An acid that has an empty orbital can use it to accept a lone pair of electrons from the base to form a coordinate covalent bond.

Nucleophile: A lewis base, its lone pair is attracted to other nuclei

Electrophile: A lewish acid. its attracted to the lone pair of electrons on the lewis base hi rat, it’s Milaj/