acids and bases ph and poh. intro quiz: put these items in ph order from most acidic to least. blood...
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![Page 1: Acids and Bases pH and pOH. Intro Quiz: Put these items in pH order from most acidic to least. Blood Milk Water Lemon juice Baking soda Coffee Ammonia](https://reader036.vdocuments.us/reader036/viewer/2022081503/56649e395503460f94b2a2d5/html5/thumbnails/1.jpg)
Acids and BasesAcids and BasesAcids and BasesAcids and Bases
pH and pOHpH and pOH
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Intro Quiz:• Put these items in pH order from
most acidic to least.• Blood• Milk
• Water• Lemon juice• Baking soda
• Coffee• Ammonia
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Answer:• Lemon juice
• Coffee• Milk
• Water• Blood
• Ammonia• Baking Soda
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Defining & Using pH & pOH
Acid neutral Base
pH 0 1 2 3 4 5 6 7 8 9 10 11 12 13 14 pH
Examples
1M HCl
0.1M HCl
Gastric juice
ant venom
coca cola
lemon juice
vinegar
wine
coffeetomatoes
tap water
saliva
cow's milk
pure water
sea water
soapbaking soda
detergents
toothpaste
detergents
washing soda
household cleaner
0.1M NaOH
caustic oven cleaner
1M NaOH
+
pOH 14 13 12 11 10 9 8 7 6 5 4 3 2 1 0 pOH
most acidic
< ---- ----- ---- ---------
least acidic
neutral
least basic
----- -------- ----- ----- >
most basic
=14
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pH
• pH is a measure of the hydrogen ion concentration, [H+]
• pH is calculated using the following formula:pH = -log10[H+]
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pOH• pOH is a measure of
the hydroxide ion concentration, [OH-]
• pOH is calculated using the following formula:pOH = -log10[OH-]
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Solutions• Acidic solution: When the [H+] is
greater than [OH-]• Basic solution: When [OH-] is
greater than [H+]• Basic solutions are also known as
alkaline.
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Indicators
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Example 1:• Find the pH of a 0.2mol L-1
(0.2M) solution of HCl • Calculate pH: pH = -log10[H+]
pH = -log10[0.2] = 0.7
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Example 2:• Find the pOH of a 0.1mol L-
(0.1M) solution of NaOH • Calculate pOH: pOH = -
log10[OH-]pOH = -log10[0.1] = 1
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Example 3:• Find the pH of a 0.2 mol L-1
(0.2M) solution of H2SO4
• Calculate pH: pH = -log10[H+]pH = -log10[0.4] = 0.4
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Example 4:• Find the pOH of a 0.1mol L-1
(0.1M) solution of Ba(OH)2
• Calculate pOH: pOH = -log10[OH-]pH = -log10[0.2] = 0.7
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pH + pOH = 14 • And:• [H+] * [OH-] = 1 x 10-14
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OR:• [H+]*[OH-] = Kw = 1 X 10-14
• Take the -log of both sides of the equation
• - log [H+] +(- log [OH- ]) = - log [1 X 10-14 ]
• pH + pOH = 14
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About those H+’s• Water molecules are highly polar• A water molecule that loses H+
becomes the negatively charge hydroxide ion OH-
• The water molecule that gains a H+ (proton) becomes a hydronium ion, H30+
• H2O (l) H3O+(aq) + OH-(aq)
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Self Ionization• This is also known as the self
ionization reaction of water
• H2O (l) H3O+(aq) + OH-(aq)
• This is because water is amphoteric.
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Example (1): • Find the pH of a solution of sodium
hydroxide that has a pOH of 2 • pH = 14 - pOH
• pH = 14 - 2 = 12
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Example (2):• Find the [OH-] of a sulfuric acid
solution with a pH of 3 • Calculate the pOH • pOH = 14 - pH • pOH = 14 - 3 = 11 • Calculate [OH-]
[OH-] = 10-pOH
[OH-] = 10-11 = 10-11 mol L-1
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Example• pH [H+] [OH-]
pOH • 7 1.0 x 10-7M 1.0 x 10-7M 7• 6 1.0 x 10-6M 1.0 x 10-8M 8• 5 1.0 x 10-5M 1.0 x 10-9M 9• Etc.