Acid and Bases and example compounds to recognize

Arrhenius base

Produces hydroxide ions (OH-) in water

Bronsted-Lowry acid

Proton (H+) donor

Bronsted-Lowry base

Proton (H+) acceptor

Conjugate acid-base pair rule

A strong acid has weak conjugate base and a weak acid has a stronger conjugate base.

Auto-ionization of water (Kw)

Kw= 1.0×10^-14 at 25 degrees Celsius

Ka x Kb=

Ka x Kb=Kw= 1.0 × 10^-14

pH +pOH=

14 at 25 degrees Celsius

pH formula

pH= -log[H+]

pOH formula

pOH= -log[OH-]

pKa formula

pKa= -log Ka

Examples of strong acids?

HCl

HBr

HI

HNO3

H2SO4(first H+ only)

HClO4

Strong bases examples

NaOH

KOH

(Ca(OH)2)

(Ba(OH)2)

Ka>1 × 10^-3 means?

Strong acid ( almost complete dissociation)

Ka<1 × 10^-6 means?

Weak acid use small x approximation.

Relationship between Ka and pKa

Lower pKa the stronger the acid is

Relationship between Kb and pKb

Lower pKb stronger the base

(S)

Solid

Example NaCl sodium chloride Cristal

(l)

Liquid

Example: H2O(l) water

(g)

Gas

Example CO2 carbon dioxide

(aq)

Aqueous (dissolved in water)

Example: Na+ sodium ion in solution

Name all of them