Chemistry 2 Exam 3 Chapter 17

Strong Acids

• Hydrochloric acid: (HCl)

• Hydrobromic acid: (HBr)

• Hydroiodic acid: (HI)

• Sulfuric acid: (H₂SO₄)

• Nitric acid: (HNO₃)

• Phosphoric Acid (H3PO4)

• Perchloric acid: (HClO₄)

• Chloric acid: (HClO₃)

pH, Ka, strength 

The higher Ka value, lower PH, stronger the acid

Weak Acids

• Acetic acid: CH3COOH (organic) or

  

• Hydrofluoric acid: HF

Strong Bases

• Sodium Hydroxide: NaOH

• Potassium Hydroxide: KOH

• Ammonia: NH3

• Amine (organic):  R [any organic compound] -NH2

• Aniline (organic):C6H5NH2

• Pyridine (organic):C5H5N

• Sodium Bicarbonate: NaHCO3

• Sodium Carbonate: Na2CO3

Weak bases

Binary Acids

molecular compounds composed of hydrogen and one other nonmetal element

Sulfuric Acid

(H₂SO₄)

(

Nitric Acid

(HNO₃)

Acetic Acid

(CH₃COOH)

Phosphoric Acid

(H₃SO₄)

Arrehnius Acid-Bases

• Acid: Produces H+ in a solution

  • H+/H2O

  • HCl/H2O

  • H+ +H2O = H3O+

• Base: Produces OH- in a solution

  • -OH (aq)

  • -OH/H2O

  • NaOH/H2O

Bronsted Lowry Acid Base 

an acid as a proton (H+)  donor and a base as a proton (H+)  acceptor

Strength of Acid Bases

• STRONG Acid/Bases—> Strong electrolytes (forms ions) + COMPLETLY ionizes (weak bonds)

  

• WEAK Acids/Bases—> Weak electrolytes + PARTIALLY ionizes (strong bonds)

  

Ionization constant (Ka or Kb)  

• ignore solids or liquids

• [products]/[reactants]

• The higher the Ka or Kb value= the stronger the acid/base—> the more it dissociates or breaks down in a solution 

Autoionization of Water

water acts with itself as an acid

and a base to form ion

K_w

acid vs base

ph scale + equation

x small

x small does not work if it is similar/close to initial and K values of a weak acid

acids /bases equations

Pka

polyprotic acid

both donates and gains

only lewis acid

Bastosity

number of atoms + size of the atom

summary of all of them

just a lewis acid

anything that has these C+,Fe, Al, and B

because they all accept e-

lewis bases