I. Introduction to Acids & Bases Acids & Bases. A. Properties  electrolytes  turn litmus red  sour taste  react with metals to form H 2 gas  slippery.

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Presentation transcript:

I. Introduction to Acids & Bases Acids & Bases

A. Properties  electrolytes  turn litmus red  sour taste  react with metals to form H 2 gas  slippery feel  turn litmus blue  bitter taste ChemASAP  vinegar, milk, soda, apples, citrus fruits  ammonia, lye, antacid, baking soda

B. Definitions Acids Acids form hydronium ions (H 3 O + ) HCl + H 2 O  H 3 O + + Cl – H HHHH H Cl OO – + acid

B. Definitions  Bases  Bases form hydroxide ions (OH - ) NH 3 + H 2 O  NH OH - H H H H H H N NO O – + H H H H base

B. Definitions - can be an acid or a base.  Amphoteric - can be an acid or a base.  Monoprotic Acid – can donate only one proton (H+) per molecule. Examples: HCl, HNO 3  Polyprotic Acid – can donate more than one proton (H+) per molecule. Example: H 2 SO 4 (diprotic) H 3 PO 4 (triprotic)

C. Strength  Strong Acid/Base 100% ionized in water strong electrolyte - + HCl HNO 3 H 2 SO 4 HBr HI HClO 4 NaOH KOH Ca(OH) 2 Ba(OH) 2

C. Strength  Weak Acid/Base does not ionize completely weak electrolyte - + HF CH 3 COOH H 3 PO 4 H 2 CO 3 HCN NH 3

E. Neutralization Reactions Strong acid + Strong base  Salt + Water Ex. HCl (aq) + NaOH (aq)  NaCl (aq) + H 2 O

Acids & Bases II. Aqueous Solutions and the Concept of pH

A. Self-Ionization of Water H 2 O + H 2 O H 3 O + + OH - Water molecules produce a hydronium ion and a hydroxide ion by transfer of a proton.

 Any solution in which [H 3 O + ] = [OH - ] is neutral.  Any solution in which [H 3 O + ] > [OH - ] is acidic.  Any solution in which [H 3 O + ] < [OH - ] is basic. B. Neutral, Acidic, and Basic Solutions

pH = -log[H 3 O + ] C. The pH Scale 0 7 INCREASING ACIDITY NEUTRAL INCREASING BASICITY 14 pouvoir hydrogène (Fr.) “hydrogen power”

C. The pH Scale pH of Common Substances

C. The pH Scale pH = -log[H 3 O + ] pOH = -log[OH - ] pH + pOH = 14

pH  pH = -log [H+] [H+] = 10 -pH  pOH = -log [OH-]  pH + pOH = 14

Calculations with pH Ans: x 10 –8 M Q: What is the pH if [H + ]= 6.3 x 10 –5 ? pH = – log [H + ] ‘(-)’, ‘log’, ‘6.3’, ‘EE’, ‘(-)’, ‘5’, ‘)”, ‘ENTER’) Q: What is the [H + ] if pH = 7.4? [H + ] = 10 –pH mol/L (’10 x ’, ‘(-)’, ‘7.4’, “)” ‘ENTER‘)