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? Acids taste sour Lemon, oranges, grapefruit = citric acid Yogurt, sour milk = lactic acid Carbonated drinks = carbonic acid Vinegar = acetic acid What does soap feel like? Bases taste bitter Soap = bitter Shell of nuts = bitter Acids & Bases do the same thing except from opposite directions Acids & Bases 6 acids Sulfuric Nitric Hydrochloric Phosphoric Carbonic Acetic Acid H2SO4 HNO3 HCl H3PO4 H2CO3 HC2H3O2 What do you notice? What makes an acid an acid? Bases Sodium Hydroxide Magnesium Hydroxide Aluminum Hydroxide Potassium Hydroxide Calcium Hydroxide Barium Hydroxide NaOH Mg(OH)2 Al(OH)3 KOH Ca(OH)2 Ba(OH)2 What do you notice? What makes a base a base? (OH) or the ability to make an (OH) Ammonia Sodium Hydrogen Carbonate NH3 NaHCO3 Base solutions are sometimes called ALKALINE SOLUTIONS H+ HCl + H20 Acids … ionize themselves… Back to Acids + Cl- break apart into their ions. Remember water is very polar HCl + H20 H30+ + ClYou may see…either….. H30+ or These have names: Hydronium ion, hydrogen ion, proton ion H+ Back to Bases Bases dissociate ….. Break apart producing hydroxide NaOH + H20 NH3 + H20 Na+ + NH4+ + OHOH- Which ion accounts for the alkalinity of bases in water solutions? 1. 2. 3. 4. Hydronium ion Sodium ions Hydroxide ions Alkali metals Which of the following is an alkali? 1. 2. 3. 4. Mg(OH)2 H2SO4 HCl ZnCO3 Before ionization After ionization HAcid H+ A- HAcid H+ W Strong Acid Weak Acid H+ B- Contents of solution Strong vs. Weak Can tell 2 ways memorize them arrows Strong acids: HCl, H2SO4, HNO3 Weak acids: H2CO3, HC2H3O2, H3PO4 Strong Base: group 1, 2 metals Weak base: NH3 ionize completely dissociates completely HF + H20 H2SO4 + H20 F- + H30+ HSO4 + H30+ 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, HNO3, H2SO4 Weak Acid = H3PO4, H2CO3, HC2H3O2 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: NH3 According to the dissociation theory, the ion present in all basic solutions is… 1. 2. 3. 4. O-2 OHH3O-1 OH-2 The term strong and weak refer to… 1. 2. 3. 4. 5. The concentration of the electrolyte. The degree of ionization The amount of solvent The number of electron pairs The number of hydrogens Monoprotic Diprotic Triprotic HCl, H2SO4, HNO3 H3PO4, H2CO3, HC2H3O2 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? H30+ Pure water is neutral pH = 7 “self- ionizes” OH- Water molecule + water molecule = hydronium ion + hydroxide ion Neutral because equal number of hydronium and hydroxide( ½ ½ ) pH scale Power of the hydrogen pH scale measures: the concentration of the hydromium ion or hydroxide ion. pH = 0…..14 0 3 Units of 10 Ph paper/ instruments 7 10 14 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