Acids and Bases

Naming AcidsBinary Acids (contains H & 1 other element)

• Hydro- and –ic if anion does not contain oxygen

HCl-hydrochloric acid

Oxyacids (contain H, O, & other elements)

• -ic anion ends in –ate

H2SO4 - SO4 is sulfate = sulfuric acid

• -ous anion ends in -ite

H2SO3-SO3 is sulfite = sulfurous acid

Common Acids

• Sour milk (lactic acid)

• Vinegar (acetic acid)

• Carbonated beverages (phosphoric acid)

• Lemons, oranges (citric acid)

• Apples (malic acid)

• Grape Juice (tartaric acid)

Sulfuric Acid

• Most commonly used product in the world

• Petroleum

• Automobile batteries

• Dehydration agent• Metallurgy• Refining

Nitric Acid

• Stains proteins yellow• Suffocating odor• Stains skin• Causes burns

• Explosives

• Rubber

• Plastics

• Dyes

• Pharmaceuticals

Phosphoric Acid

• Manufacturing fertilizers for plants and animal feed

• Flavoring agent in beverages• Cleaning agent for dairy equipment

Hydrochloric acid

• Produced in the stomach• Cleaning agent

• Maintain acidity in pools

Common Properties of Acids

• Sour taste

• Produce hydronium H3O+ ions

• Change the color of acid-base indicators

• React with active metals to release hydrogen gas

• React with bases to produce salts and water

• Conduct electric current

Bases

Common Bases

• Lye (sodium hydroxide)

• Milk of magnesia (magnesium hydroxide)

• Antacids (aluminum hydroxide)

Common Properties of Bases

• Taste bitter

• Produce hydroxide OH- ions

• Change the color of acid-base indicators

• Feel slippery

• React with acids to produce salts and water

• Conduct electric current

Specific Definitions of Acids/Bases

Arrhenius Acids and Bases

• Arrhenius acid-increases H+ ions (H3O+)

H2SO4 + H2O H3O+ +HSO4-

• Arrhenius base-increases OH- ions

Ca(OH)2Ca+2 + 2OH-

Weak/Strong

• Weak acid-weak electrolyte (end in -COOH)• Strong acid-ionizes completely, strong electrolyte

(HCl)• Alkaline-base completely dissociates in water to

yield OH- ions

NaOH Na+ + OH-

• Strong bases-completely dissociates, strong

electrolyte (end in OH)

Bronsted-Lowry

• Bronsted-Lowry Acid-proton donor

• Bronsted-Lowry Base-proton acceptor

HCl + NH3NH4+ + Cl-

• Monoprotic acid-donates one proton HCl

• Diprotic acid-donates two protons H2SO4

• Triprotic acid-donates three protons H3PO4

Conjugate Acids and Bases

• Conjugate base-the species that remains after a Bronsted-Lowry acid has given up a proton

HF + H2O F- + H3O+

Acid Conj. Base• Conjugate acid-the species that is formed when a

Bronsted-Lowry base gains a proton

HF + H2O F- + H3O+

Base Conj. Acid

Strength of Acid/Conj. Base

Strong acidweak conjugate base

Weak acidstrong conjugate base

Other Terms

• Amphoteric compound-any species that can react as either and acid or a base

• Neutralization-the reaction of hydronium ions and hydroxide ions to form water molecules and salt

Self-ionization of water H3O+ + OH- 2H2O or

H20 + H2OH3O+ + OH-

• Salt-an ionic compound composed of a cation from a base and an anion from an acid

Buffers

• A solution that resists a change in its pH even when a strong acid or base is added to it.

• A solution is buffered by the presence of a weak acid and its conjugate base.

• Added H+ reacts with base

• Added OH- reacts with weak acid

Titration Practice Problems

Ex 1A 30.mL volume of HCl is

titrated with 23mL of 0.20M NaOH. What is the molarity of HCl in this solution?

Answer

0.15M

Ex 2 A 26mL volume of NaOH is

titrated with 23mL of 0.20MHCl. What is the molarity of NaOH in this solution?

Answer

0.18M

Ex 3A 40.mL volume of H2SO4 is

titrated with 38mL of 0.24M NaOH. What is the molarity of H2SO4 in this solution?

Answer

0.11M

Acid/Base Rhapsody

Is this the real life? Is this just fantasy? No protons around here. Hydronium reality. Open your book and take a look and seeeeeeeeeeeee…. I’m just a poor student – prof. give me your sympathy. Marks are easy come, they’re easy go. Sometimes they’re high, sometimes they’re low. As long as you understand it, it doesn’t really matter to me - to me.

Mama, just had my class, Learned about Arrhenius, Bronsted Lowry, Lewis acids. Conjugate acid/base pairs. Amphoteric and hydrides pull my hair. Mama, oo-ooo-ooo-ooh, Some salts with hydrolize. If I don’t call again this time tomorrow. Carry on, carry on, I’m studying for this test.

Mama lots to learn acids strong and weak.

Leveling affect- an A is what I seek.

Acid-ionization constants-O, my brain is sore.

Oxyacids, indicators change color!

Mama oooooooooo.

Water auto-ionizes forms hydroxide and hydronium all the time. What??

I see a little acid and its conjugate base - Got a buffer! Got a buffer! Will you do the calculation?! Want a certain pH, find the pka that’s near. Bronsted-Lowry, Bronsted-Lowry,Bronsted-Lowry, Bronsted-Lowry rules the day. O-o-o-o-ow… I’m just a poor student spent my money at dance clubs. He’s just a poor student studies titrations at home. Spare him this question of a polyprotic acid.

Easy come easy go-indicator tells youNow is the endpoint near

I overshot again (and over)I overshot again (and over)I think I got it now…. I got it nowOhOhOhOhOhOhIndicator, indicator, indicator lets me knowThe lab TA has a buret to decide for me.for me, for me, For MEEEEEEEEEEEEEEEEEEEEE!!!!!!

So you think you can do an acid/base titration!!! But when you overshoot the endpoint, it just leads to frustration.Oh, maybe, just a little more base maybe.

I’ll think I’ll get it right. I got to get it right this time.

Doesn’t really matter-acid or base the same.

Doesn’t really matter

Doesn’t really matter to meeeeeeeeeee.

Doesn’t really matter to me.