acids, bases, & salts a modified presentation by miss nielsen
TRANSCRIPT
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Acids, Bases, &
Saltsa modified presentation by Miss Nielsen
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Activity
• 4 posters around the room.• 2 minutes with group at each poster• Write as many examples that you can think
of for the particular question on the poster paper
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The Questions
• What are Properties of Acids?• What are properties of Bases?• What are some examples of Acids in daily
life?• What are some examples of Bases in daily
life?
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What is an ACID?• pH less than 7• Neutralizes bases• Forms H
+ ions in solution
• Corrosive-• reacts with most metals to form
hydrogen gas• Good conductors of electricity
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Common Acids • HCl- hydrochloric- stomach acid• H2SO4- sulfuric acid - car batteries
• HC2H3O2- acetic acid - vinegar
• H2CO3-carbonic acid – sodas
• H3PO4- phosphoric acid -flavorings
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Weak vs. Strong Acids
• Weak Acids do not ionize completely: Acetic, Boric, Nitrous, Phosphoric, Sulfurous
• Strong Acids ionize completely: Hydrochloric, Nitric; Sulfuric, Hydriodic
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What is a BASE?• pH greater than 7• Feels slippery• Dissolves fats and oils• Usually forms OH- ions in
solution• Neutralizes acids
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Weak vs. Strong Bases
• Weak Bases: ammonia; potassium carbonate, sodium carbonate
• Strong Bases: sodium hydroxide; sodium phosphate; barium hydroxide; calcium hydroxide
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Common Bases
• NaOH- sodium hydroxide (LYE) soaps, drain cleaner• Mg (OH)2 - magnesium hydroxide-antacids
• Al(OH)3-aluminum hydroxide-antacids, deodorants
• NH4OH-ammonium hydroxide- “ammonia”
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Acids and Bases in Solution• HCl + H20 H3O + + Cl-
(more hydronium ions, more acidic)• NaOH in water Na+ + OH-
(more hydroxide ions, more basic)• NaOH + HCl NaCl + HOH
Acid + Base yields type of salt and water
• NH3 + H20 NH4+ + OH- ammonia
gas + water yields ammonium and hydroxide ions
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Theories of Acids and Bases
• In the 1800’s chemical concepts were based on the reactions of aqueous solutions.
• Svante Arrhenius (Mr. Deis’s favourite Swedish Chemist) developed a concept of acids and bases relevant to reactions in H2O.
• Arrhenius acid – produces hydrogen ions in water.• Arrhenius base – produce hydroxide ions in water.
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Theories of Acids and Bases
Other Theories discussed further in your chemistry careers:
Bronsted-Lowry acid- donates a hydrogen ion/proton in a reaction.
Bronsted – Lowry base – accepts a hydrogen ion/proton in a reaction.
Lewis Acid – electron pair acceptor
Lewis Base – electron pair donator
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Examples of Arrhenius Acids/Bases
• HNO3
• KOH• Ba(OH)2
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Neutralization Reaction
• A neutralization reaction is the reaction of an acid with a base to produce salt and water.
• Example
H2SO4 + NaOH NaHSO4 + H2O
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What is a SALT?• A salt is a neutral substance produced from the
reaction of an acid and a base.• Composed of the negative ion of an acid and the
positive ion of a base.• One of the products of a Neutralization Reaction• Examples: KCl, MgSO4, Na3PO4
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Textbook Questions
• p.711,# 2,16,17a Q. Write dissociation equations for the following Arrhenius acids and bases:• HNO3
• KOH• HClO4
• H3PO4
• Ba(OH)2
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What is pH?
• Scale based on logarithmic values to measure how acidic or alkaline a substance is
• Traditional Scale from 0-14
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pH of Common Substances
Timberlake, Chemistry 7th Edition, page 335
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Calculating pH
• pH• Water has an equilibrium concentration of its two ions: • 1.00x10-7M H+
(aq) and 1.00x10-7M OH-(aq)
• When one concentration rises, the other decreases by the same amount to re-establish equilibrium.
• Developed by Swedish chemist, Soren Sorensen, the calculation for the pH of a solution is…
• pH = -log10 [H+(aq)]
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[H+(aq)] (mol L-1) pH1.0 x 10-7 1.0 x 10-6 1.0 x 10-5 3.5 x 10-7 1.0 x 10-4 3.5 x 10-7
pH values: XX.YY (X=sig Y=not sig)
Calculating pH
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• Introductory pH calculations• Calculate the pH when:
– A. [H+(aq)] = 3.0x10-5 M
• B. [H+(aq)] = 2.77x10-12 M
– [OH-(aq)] = 3.4x10-11 M (now, pOH and what
“14” means)• Calculate the pH for each:
– [H+(aq)] = 6.300x10-4 M
– [OH-(aq)] = 2.99x10-2 M
– [H+(aq)] = 13 M
– [OH-(aq)] =2.5 M
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• Now…– When pH changes by 2, what does that do to the [H+
(aq)] ?
– pH = 5.77. Calculate the [H+(aq)] (a reverse operation!)
• Strong Acids– 0.20 M HCl. Find pH– 0.300M H2SO4. Find pH
– 4.6x10-8 M HNO3. Find pH
• Strong Base– 0.150 M NaOH. Find pH– 0.10 M barium hydroxide solution. Find pH– 5.70g of potassium hydroxide in a 100 mL solution. Find pH– Magnesium hydroxide has a pH = 13.40. Find the original
magnesium hydroxide concentration.• Neutral Ionic
– 0.10 M NaCl. Find pH
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Textbook Questions
• Questions: p.713,#43,45,47,49,81,82
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ACID/BASE CHEMISTRY IN REAL LIFE
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Situations in which pH is controlled
• “Heartburn” – stomach is acidic, Tums (calcium carbonate) neutralizes stomach acid
• Planting vegetables and flowers – fertilizers control pH, plants have own pH (Spruce trees)
• Fish Tanks and Ponds – Fish require a certain pH to survive, without that pH, fish will not survive (Miss Nielsen has personal experience with this!)
• Blood – carbon dioxide in blood stream• Swimming pools – pH around 7.5 to maintain the proper
pH without having skin irritation
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Acid Rain
Pollution in the air (sulfur dioxide, carbon dioxide, nitrogen dioxide) combines with water to form various acids.
.
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Rapid changes in pH can kill fish and other organisms in lakes and streams.Soil pH is affected and can kill plants and create sinkholes
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pH in the Digestive System• Mouth-pH around 7. Saliva contains amylase, an
enzyme which begins to break carbohydrates into sugars.
• Stomach- pH around 2. Proteins are broken down into amino acids by the enzyme pepsin.
• Small intestine-pH around 8. Most digestion ends. Small molecules move to bloodstream toward cells that use them
• Bile – pH around 8 created in liver, stored in gall bladder and is used to break down fats (which are acids),
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Edible pH Scale
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Review Videos Featuring Mr.Lederer
• http://ca.youtube.com/watch?v=dzXeb_jm9sQ&feature=related
• http://ca.youtube.com/watch?v=W_ALHNjFtMg&feature=related
• http://ca.youtube.com/watch?v=PqYySv1L60g&feature=related