Acid and Base Strength
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Transcript of Acid and Base Strength
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Acid and Base StrengthAcid and Base Strength
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AcidsHave a sour taste.
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AcidsTurn blue litmus red.Turn methyl orange red.
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AcidsWill react with:some metals to produce a salt and H2.metal oxides to produce a salt and H2O.metal carbonates to produce a salt, H2O, and CO2.
bases to produce a salt and H2O.Mg + 2HCl MgCl2 + H2
MgO + 2HCl MgCl2 + H2OMgCO3 + 2HCl MgCl2 + H2O + CO2Mg(OH)2 + 2HCl MgCl2 + 2H2O
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AcidsAre electrolytes.
Conduct an electric current when dissolved.
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BasesHave a bitter taste.
Coffee itself is acidic, but it contains an alkaline compound – caffeine – which contributes to its bitter taste.
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BasesFeel slimy or slippery to the touch.
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BasesTurn red litmus blue.Turn methyl orange yellow.Turn phenolphthalein pink.
Litmus pH scale.
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BasesReact with acids to produce salt and H2O.HCl + NaOH NaCl + H2O
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BasesAre electrolytes.
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Properties of Acids◦Taste sour.◦Turn litmus red.◦Proton (H+) donors.◦ Inc. [H3O+] in aqueous
solutions.
Properties of Bases◦Taste bitter.◦Turn litmus blue.◦Proton acceptors.◦ Inc. [OH-] in aqueous
solutions.
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pH Scale◦Traditionally 0 - 14.
Can have pH < 0 or > 14.◦pH < 7 Acidic solution.◦pH = 7 Neutral solution.◦pH > 7 Basic solution.
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pH ScalepH Scale
Acidic Basic
0 1 2 3 4 5 6 7 8 9 10
11
12
13
14
pH Scale
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HCl, A Strong AcidHCl, A Strong Acid
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HF, A Weak AcidHF, A Weak Acid
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As [H+] Increases, [OH-1] Decreases
1x10-13 M1x10-12 M1x10-11 M1x10-10 M1x10-9 M1x10-8 M1x10-7 M1x10-6 M1x10-5 M1x10-4 M1x10-3 M1x10-2 M1x10-1 M
1x10-13 M1x10-12 M1x10-11 M1x10-10 M1x10-9 M1x10-8 M1x10-7 M1x10-6 M1x10-5 M1x10-4 M1x10-3 M1x10-2 M1x10-1 M
[H+ ]
[OH-
1 ]
Neutral Solution
Acid added to neutral solutionBase added to neutral solution
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In any aqueous solution:◦ [H+] [OH-1] = 1x10-14
◦ As [H+] goes up, [OH-1] must decrease.◦ As [OH-1] goes up, [H+] must decrease.
In other words, adding an acid to water causes the solution to become more acidic and less basic.
Adding a base to water causes the solution to become less acidic and more basic.
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If [H+] = 1x10-3 M, what is [OH-1]?◦ [H+][OH-1] = 1x10-14
◦ (1x10-3 M)[OH-1] = 1x10-14
◦ [OH-1] = (1x10-14) / (1x10-3)◦ [OH-1] = 1x10-11 M
If [OH-1] = 1x10-8 M, what is [H+]?◦ [H+][OH-1] = 1x10-14
◦ [H+](1x10-8 M) = 1x10-14
◦ [H+] = (1x10-14) / (1x10-8 M)◦ [H+] = 1x10-6 M
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pH = power of Hydrogen◦ negative logarithmic (powers of ten) scale.
pH = -log10[H+]◦ If [H+] = 1x10-1 M,
pH = -log(1x10-1 M) = 1◦ If [H+] = 1x10-2 M,
pH = -log(1x10-2 M) = 2◦ If [H+] = 1x10-3 M,
pH = -log(1x10-3 M) = 3
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Calculations Involving pH, pOH, [H+], and [OH-] of strong Acids and Bases
pH = -log [H+]
pOH = -log [OH-]
pOH + pH = 14
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Concentrations of Hydronium and Hydroxide Ions
1.00E-14
1.00E-121.00E-10
1.00E-081.00E-06
1.00E-041.00E-02
1.00E+00
1 2 3 4 5 6 7 8 9 10 11 12 13
pH
Mol
ar [H3O+1]
[OH-1]
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What are the pH values of the following solutions?◦ 1x10-1 M H+
pH = -log(1x10-1 M) = 1◦ 1x10-3 M H+
pH = -log(1x10-3 M) = 3◦ 1x10-5 M H+
pH = -log(1x10-5 M) = 5◦ 1x10-1 M OH-1
[H+] = (1x10-14) / (1x10-1 M) = 1x10-13 M pH = -log(1x10-13 M) = 13