Chemistry - Acids and Bases

Acid

H+

Any substance that donates protons

Base

OH-

Any substance that accepts protons

Proton

H+ ion

Neutralization

Acid + Base → ionic salt + water

Amphiprotic / Amphoteric

Species that can act as Bronsted-Lowry acid or base

Bronsted-Lowry Theory

Identifies acids and bases as either a proton donor or proton acceptor

Conjugate acid-base pair

Differed by a h+ in the opposite reaction

I.E. NH3 + H2O → NH4+ + OH-

NH3 is the conjugate base of the NH4+

H2O is the conjugate acid of OH-

Acids + Reactive Metals

Acid + Metal → Salt + Hydrogen gas

I.E. Zn + 2HNO3 → Zn(NO3)2 +H2

Bases + Metal

Acid + Metal oxide → salt + water

Acids undergo neutralizing reactions with a base & alkalis to produce salt + water

I.E. CuO + HSO → CuSO + H2O

NaOH + HNO3 → NaNO3 + H2O

Acids + Metal carbonates

Acid + Metal carbonates → salt + water + carbondioxide

I.E. MgCO3 + 2HCl → MgCl2 + H2O +CO2

Alkalis

Bases soluble in water