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Acids, Bases and Reaction Rates
Unit 14 Acids, Bases and Reaction Rates
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Acids and Bases And others…
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Acids For thousands of years people have known that vinegar, lemon juice and many other foods taste sour. However, it was not until a few hundred years ago that it was discovered why these things taste sour – They taste sour because they are all acids. The term acid, in fact, comes from the Latin term acere, which means "sour"
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Acid Characteristics Acids have a PH of less than 7. Acids taste sour
Acids are corrosive to metals Acids can ‘burn' your skin Acids change litmus paper red Litmus paper helps to determine acids and bases Acids become less acidic when mixed with bases.
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Examples of Acids orange juice, lime juice or lemon juice (citric acid) vinegar (acetic acid) aspirin (salicylic acid) yogurt (lactic acid) Coca-Cola (phosphoric acid) toilet bowl cleaner (sulfuric acid) bathroom cleaner (muriatic acid) wine (tartaric acid and/or malic acid) vitamin C tablets (ascorbic acid) urine (uric acid)
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Bases Bases can also be called alkalis.
Bases can be thought of as the chemical opposite of acids. A reaction between an acid and base is called neutralization We will talk more about this tomorrow An example of base: soap
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Base Characteristics Bases have a pH more than 7 Bases feel slippery
Converts fats and oils in skin to glycerin (slick feel) In a sense, bases dissolve your skin… think of getting Clorox bleach on your skin Bases turns litmus paper to a blue color. Bases become less basic when mixed with acids. Bases reacts with acids to form salt and water
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Base Examples Mustards Many medicines
Ie. Magnesium oxide – treats indigestion Bleaches, soaps, toothpastes, window cleaners and other cleaning agents Sodium Hydrogen Carbonate (bread soda). Sodium hydroxide (NaOH) or caustic soda Calcium hydroxide ( Ca(OH)2 ) or limewater Ammonium hydroxide (NH4OH) or ammonia water Magnesium hydroxide ( Mg(OH)2 ) or milk of magnesia
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pH Scale Measure of how acidic or how basic More Acidic More Basic
Pure water Baking Soda Stomach Acid Egg Whites Mineral Lime Vinegar Rain NaOH HCl Lemon Juice Ammonia Drano Soda Tums More Acidic More Basic
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ACIDS 1 - HCL 2 – Stomach Acid 3 – Lemon Juice 4 - Vinegar 5 - Soda 6 – Rain Water BASES 8 – Egg Whites 9 – Baking Soda 10 - Tums 11 - Ammonia 12 – Mineral Lime 13 - Drano 14 - NaOH Neutral: 7 – Pure Water
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Acids and Bases… and others
Identification
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Identifying Acids Acids start with “H” Examples: HCl H2SO4
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Identifying Bases Bases end in “OH” (hydroxides) Examples: NaOH
Ca(OH)2
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Identifying Metals Metals are single elements found on the left side of the periodic table Separated from non-metals by metalloids (staircase) Examples Al Li Can you name any other ones?
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Identifying Carbonates
Carbonates end with the elements “CO3” Examples Na2CO3 MgCO3
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Identifying Salts Salts are two elements bonded together from opposite sides of the periodic table or with a polyatomic ion What is polyatomic ions? Examples NaCl AlF3 KNO3
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Reactions with Acids
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Let’s Review… How do we know which chemicals are… Bases? Acids?
Carbonates? Salts? Metals?
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Let’s practice~ Classify the following chemicals…
NaCl HCl Li2CO3 Mg KOH Ag MgCO3 BeF2 Al(OH)3 Groups: Metals Acid Bases Carbonates Salts Metals – Ag, Mg Acids – HCl Base – Al (OH)3, KOH Carbonates – Li2CO3, MgCO3 Salts – NaCla, BeF2
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Review – Charges on Ions
Group (Periodic Table) Example Charge Why? Alkali metal Alkaline earth metal Nitrogen group Chalcogens Halogens Alkali metals +1 (loses 1 electron so have full outer orbital) Alkaline earth metals +2 (loses 2 electrons so have full outer orbital) Nitrogen group -3 (gains 3 electron so have full outer orbital) Chalcogens -2 (gains 2 electron so have full outer orbital) Halogens -1 (gains 1 electron so have full outer orbital)
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Review Writing Formulas
Let’s practice: Lithium iodide Magnesium hydroxide Hydrogen gas Sodium Calcium carbonate Li +1, I -1 LiI Mg +2, OH -1 Mg(OH)2 H H2 Na (not in compound = no charge, not an ion) Ca +2, CO3 -2 Ca2(CO3)2 , but if both 2s CaCO3
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Review Balancing Equations
___ NaNO3 + ___ PbO ___ Pb(NO3)2 + ___ Na2O ___ AgI + ___ Fe2(CO3)3 ___ FeI3 + ___ Ag2CO3
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ACIDS REACT WITH METALS
Acid is a compound, metal is an element… So what type of reaction? HCl Li _________ + __________ HF Mg _________ + _________ H2S + Al _________ + _________ Therefore… Acid Metal salt H2 What type of reaction involves a compound and an element? - single displacement -what side of the periodic table is the metal on? Left (positive) -therefore the metal will displace the element on the left of the (the positive element)– so will displace the hydrogen out of the compound to produce salt and H2 gas HCl + Li LiCl +H2 HF + Mg MgF2 + H2 (need to criss cross) H2S + Al Al2S3 + H2 (need to criss cross) **DON’T FORGET TO BALANCE!!!
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Acid + Carbonate salt + CO2 + H2O
ACIDS WITH CARBONATES Acid is a compound, carbonate is an compound… So what type of reaction? HCl MgCO3 ________ + _________ HI Li2CO3 ________ + ________ H2S + Na2CO3 _______ + _________ Acid + Carbonate salt + CO2 + H2O What type of reaction involves two compound? - double displacement -positives switch H2CO3 very reactive, breaks down almost immediately into H2O and CO2 HCl + MgCO3 MgCl2 + H2CO3 MgCl2 + CO2 + H2O HI + Li2CO3 LiI + H2CO3 LiI + CO2 + H2O H2S + Na2CO3 Na2S + H2CO3 Na2S + CO2 + H2O **DON’T FORGET TO BALANCE EQUATIONS!!
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Acid and Base Reactions
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ACIDS and BASES REACTIONS
What distinguishes acids? What distinguishes bases?
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ACIDS and BASES Acid is a compound, base is an compound…
So what type of reaction? __ HCl + __ NaOH __ NaCl + __ HOH H2O __ HF + __ Ca(OH)2 __Ca F2 + __ H2O Acid + Base salt + H2O
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Titration Neutralizing an acid or base MA x VA = MB x VB M = molarity
V = volume A = acid B = base
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Practice If you add 10mL of acid to 20mL of a .10M basic solution, what will the molarity of the acid be? MA x VA = MB x VB Lets look at volume and molarity… Less concentrated, we need more More concentrated, we need less
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