The student will: understand the concept of acids/bases. will identify from a reaction strong/weak acid/base. will be able to explain dissociation or ionization and its relationship to strength of acid/base. Will be able to identify a monoprotic, diprotic, triprotic acid. will be able to compare/ contrast pH of liquids no ws

Acids Vs. Base What do lemons and pickles taste like? What does soap feel like? Acids & Bases do the same thing except from opposite directions Acids taste sour Lemon, oranges, grapefruit = citric acid Yogurt, sour milk = lactic acid Carbonated drinks = carbonic acid Vinegar = acetic acid Bases taste bitter Soap = bitter Shell of nuts = bitter

Acids & Bases 6 acids SulfuricH 2 SO 4 NitricHNO 3 HydrochloricHCl PhosphoricH 3 PO 4 CarbonicH 2 CO 3 Acetic Acid HC 2 H 3 O 2 What do you notice? What makes an acid an acid?

Bases Sodium Hydroxide NaOH Magnesium Hydroxide Mg(OH) 2 Aluminum Hydroxide Al(OH) 3 Potassium Hydroxide KOH Calcium HydroxideCa(OH) 2 Barium HydroxideBa(OH) 2 What do you notice? What makes a base a base? (OH) or the ability to make an (OH) AmmoniaNH 3 Sodium Hydrogen CarbonateNaHCO 3 Base solutions are sometimes called ALKALINE SOLUTIONS

Back to Acids HCl + H 2 0H + +Cl - Acids … ionize themselves… break apart into their ions. Remember water is very polar HCl + H 2 0 H Cl- You may see…either….. H or H + These have names: Hydronium ion, hydrogen ion, proton ion

Back to Bases Bases dissociate ….. Break apart producing hydroxide NaOH + H 2 0Na+ + OH- NH 3 + H 2 0NH OH-

Which ion accounts for the alkalinity of bases in water solutions? 1.Hydronium ion 2.Sodium ions 3.Hydroxide ions 4.Alkali metals

Which of the following is an alkali? 1.Mg(OH) 2 2.H 2 SO 4 3.HCl 4.ZnCO 3

Before ionization After ionization Contents of solution Strong Acid HAcid H+ A- Weak Acid HAcidH+ W H+B-

Strong vs. Weak Can tell 2 ways memorize them arrows Strong acids:HCl, H 2 SO 4, HNO 3 ionize completely Weak acids: H 2 CO 3, HC 2 H 3 O 2, H 3 PO 4 Strong Base: group 1, 2 metals dissociates completely Weak base: NH 3

HF + H 2 0F - + H H 2 SO 4 + H 2 0HSO 4 + H 3 0 +

Strength of acids depends on: H+ production polarity of bonds ionization The greater the polarity of bond = greater strength The greater the ionization = greater strength The ease with which the hydrogen to the element bond can be broken Strong acids= HCl, HNO 3, H 2 SO 4 Weak Acid = H 3 PO 4, H 2 CO 3, HC 2 H 3 O 2 Notice: strength of acid does not depend on number of hydrogens

Strength of bases depends on: OH- production polarity of bonds dissociation of hydroxide Base solutions are sometimes called alkaline solutions Strong Bases: NaOH, KOH, Ca(OH) 2, Ba(OH) 2 Weak Base: NH 3

According to the dissociation theory, the ion present in all basic solutions is… 1.O -2 2.OH - 3.H 3 O -1 4.OH -2

The term strong and weak refer to… 1.The concentration of the electrolyte. 2.The degree of ionization 3.The amount of solvent 4.The number of electron pairs 5.The number of hydrogens

Monoprotic Diprotic Triprotic HCl, H 2 SO 4, HNO 3 H 3 PO 4, H 2 CO 3, HC 2 H 3 O 2

Return to strength of Acid/Base Memorize list -- look at arrows -- measure the pH. What makes an Acid an Acid? What makes a base a base? Pure water is neutral pH = 7 “self- ionizes” Water molecule + water molecule = hydronium ion + hydroxide ion Neutral because equal number of hydronium and hydroxide( ½ ½ ) H30+H30+ OH -

pH scale Power of the hydrogen pH scale measures: the concentration of the hydromium ion or hydroxide ion. pH = 0… Units of 10 Ph paper/ instruments

The will student will: understand the concept of acids/bases will identify from a reaction strong/weak acid/base will be able to explain dissociation or ionization and its relationship to its strength. Will be able to identify a monoprotic, diprotic, triprotic acid will be able to compare/contrast pH of liquids no ws