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Characteristics of Acids: Table K Electrolytes pH scale: less than 7 Litmus: RED Phenolphthelein: colorless Contains a high concentration of Hydrogen ions (H + ) or Hydronium Ion (H 3 O + ) H 2 O + H + = H 3 O + React with certain metals to produce hydrogen gas (H 2 ) – TABLE J
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Metal must be higher than H 2 to react
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Characteristics of Bases: Table L Electrolytes pH scale: greater than 7 Litmus: BLUE Phenolphthelein: pink Contains a high concentration of Hydroxide ions (OH - ) Tastes bitter; feels slippery/soapy
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Characteristics of Salts An ionic compound that has positive ions other than hydrogen (H + ) and negative ions other than hydroxide (OH - ). Example: NaCl (Na + and Cl - ). Salts conduct electricity (salts are electrolytes). ACIDS, BASES & SALTS ARE ELECTROLYTES
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Beware of Tricks... Organic Acids have a functional group –COOH, so when you see a compound with carbon and this functional group it is an acid!! Ex: CH 3 COOH Alcohols have a functional group –OH (hyroxyl), not OH - (hydroxide); alcohols are not bases!! Ex: CH 3 OH
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Table K Table L
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Strong Acids & Bases HCl HBr HI HNO 3 H 2 SO 4 HClO 3 HClO 4 NaOH KOH Ca(OH) 2 LiOH RbOH CsOH Ba(OH) 2 NH 3 is a weak base!!
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ARRHENIUS THEORY OF ACIDS & BASES has H and releases H + in An Arrhenius Acid has H and releases H + in an aqueous solution. an aqueous solution. The H + ion is the only positive ion in these solutions. The H + ions are always attached to H 2 O forming H 3 O + (hydronium ions). has OH (hydroxide) and releases OH - (hydroxide ion) in an aqueous solution. An Arrhenius base has OH (hydroxide) and releases OH - (hydroxide ion) in an aqueous solution. The OH - ion is the only negative ion in these solutions.
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Bronsted-Lowry Theory (Alternate Acid-Base Theory) Bases Accept Acids Donate Bases: H + acceptor (proton acceptor) Acids: H + donor (proton donor)
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Conjugate Acid Base Pairs 1. NH 4 + + OH - → NH 3 + H 2 O 2. H 3 PO 4 + NO 2 - → HNO 2 + H 2 PO 4 - 3. HI (aq) + H 2 O (l) → H 3 O + (aq) + I - (aq) Some substances can sometimes act like an acid and sometimes act like a base. Examples are H 2 O & HSO 4 -
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Neutralization Reactions ACID + BASE = WATER + SALT (IONIC SOLID)
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Titration Titration is a lab process in which a volume of a solution of known concentration is used to determine the concentration of another solution. M A V A =M B V B
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Example 1: What is the molarity of HCl (aq) if 10. milliliters of 4.0 M NaOH (aq) neutralizes exactly 20. milliliters of HCl (aq)?
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Example 2: What is the molarity of NaOH (aq) if 10. milliliters of 2 M HBr (aq) neutralizes exactly 5. milliliters of NaOH (aq)?
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pH Scale Movement from one whole number to the next represents a change by a power of 10. Acids: 1-7, [H 3 O + ] > [OH - ] Neutral: 7, [H 3 O + ] = [OH - ] Bases: 7-14, [H 3 O + ] < [OH - ]
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Meaning of pH & pOH pH = -log[H + ] pH = -log[1.0X10 -5 ] = -(-5) = 5 The solution is acidic. pOH = -log[OH - ] pOH is the concentration of OH - instead of the concentration of H + pH + pOH = 14
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