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Acids and Bases
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pH Scale
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Apply the Numbers
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NOTE [ BRACKETS ] = CONCENTRATION (MOLARITY)
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Determining Strength Dissociation: compound breaking into ions HCl H + Cl -
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Determining Strength [H+] or [H 3 O+] = Acidic Strength [OH-] = Basic Strength
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Using Water to Determine Strength K w = [H+] x [OH-] = 1.0x10 -14 Reference table!!!!!!!!!
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Determining Strength We use the concentrations to determine if a solution is acidic or basic. Careful, since we are using a negative coefficient. The larger the coefficient = the smaller number. (this’ll make sense shortly)
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Always get to this if confused
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Cokes are slightly acidic, if the [H+] in a solution is 1x10^5 M, is the solution acidic, basic, neutral? What is the [OH-] of the solution?
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Is a [H+] = 6.0x10^-10 M solution acidic, basic, or neutral? (think logically, not # crunching)
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Crunching Molarity and Kw can be complicated. pH
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[H+] pH = -log [H+ ] Ref table
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[OH-] pOH = -log[OH-] Ref table
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What iF I gave you a hydroxide concentration and asked for pH pH + pOH = 14 Ref table
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What is the [OH-] from a solution with a pH of 4.5?
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What is the pH of a solution with a pOH of 3.2?
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What is the pOH of a solution with [H+] = 3.5x10^-8 M
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Acid Dissociation HCl --> H + and Cl -1-
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Sour Taste React with metals Turn litmus paper RED http://www.cybered.net/library/Teaching_Resources/Chemistry/Properties_of_Acids/Image_Gallery/Properties-HydrogenHydroniu.jpg 3 Properties of Acids
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Acid Examples
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Bases
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Bases end in “OH” (hydroxide) NaOH KOH Mg(OH) 2
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BASES Break into (OH) - ions
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Base Dissociation Mg(OH) 2 --> Mg +2 and (OH) -
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Properties of Bases Bitter taste Slippery feel (like soap) Turn litmus paper BLUE http://www.cybered.net/library/Teaching_Resources/Chemistry/Properties_of_Acids/Image_Gallery/Properties-HydrogenHydroniu.jpg
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Acid + Base Acid + Base --> Water + Salt
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pHpH
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What is pH pH measures how ACIDIC (H) + a solution is
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Every solution has both acidic (H) + and basic (OH) - ions in it, whichever ions have more will tell us the type of solution
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The pH scale 0 --> 14 Color your pH scale according to the following slide
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Neutral pH 7.0 Pure Water
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Base pH Level pH greater than 7.0
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Base pH Strength (common sense) Higher = Stronger
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pH 12 stronger base than pH 9
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Acids pH Levels pH below 7.0
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Acid pH Strength (Reverse of common sense) Lower Number = Stronger
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pH 1 is stronger acid than pH 5
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How much does strength increase or decrease? Moving up/down on pH scale is by a factor of 10x
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Compare pH of 4 to a pH of 5 Acidic pH of 4 is 10x more acidic than pH of 5 Basic pH of 5 is 10x more basic than pH of 4
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Compare pH 9 to pH 12 Acidic pH 9 is 1000x more acidic (10x10x10) than pH 12 Basic pH 12 is 1000x more basic than pH 9
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http://www.cybered.net/library/Teaching_Resources/Chemistry/Properties_of_Acids/Image_Gallery/Properties-PHconcept.jpg pH=0 Strongly Acidic pH=7 neutral pH=14 Strongly basic
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What substance would you use to neutralize an acid with a pH of 1.5? A. Milk C. Ammonia B. Vinegar D. Water
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Neutralization To neutralize a solution ADD Opposite! Add base to neutralize an acid Add acid to neutralize a base
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Easy step Neutralizing pH calculation find neutralizing pH 14 – pH given = pH needed to neutralize
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What pH would neutralize a stomach acid (ph of 2)
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Pepto Bismol vs Milk of Magnesia pH ~6.0 pH ~10.0 Which would be better? Think about it!
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Give dissociation of calcium hydroxide
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pOH is 11.64, and you have 2.55L of solution, how many grams of Calcium hydroxide are in solution?
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1.5L of solution containing 5.6 g of hydroiodic acid, what is the pH
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