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pH scale Logarithmic scale –expressing H +1 concentration, [H +1 ] If pH changes by factor of 1, [H +1 ] changes by factor of 10 pH = -log[H +1 ]pH = -log[H +1 ]
![pH scale Logarithmic scale –expressing H +1 concentration, [H +1 ] If pH changes by factor of 1, [H +1 ] changes by factor of 10 pH = -log[H +1 ]pH = -log[H +1 ]](http://images.slideplayer.com./39/10934315/slides/slide_3.jpg "pH scale Logarithmic scale –expressing H +1 concentration, [H +1 ] If pH changes by factor of 1, [H +1 ] changes by factor of 10 pH = -log[H +1 ]pH = -log[H +1 ]")
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Molarity to pH To determine pH: express [H +1 ] in scientific notation remember, [ ] means concentration of whatever is inside brackets log is the power of 10 log is the power of 10
![Molarity to pH To determine pH: express [H +1 ] in scientific notation remember, [ ] means concentration of whatever is inside brackets log is the power of 10 log is the power of 10](http://images.slideplayer.com./39/10934315/slides/slide_5.jpg "Molarity to pH To determine pH: express [H +1 ] in scientific notation remember, [ ] means concentration of whatever is inside brackets log is the power of 10 log is the power of 10")
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Molarity to pH for Pure water there ’ s a tiny bit of ionization: H 2 O H +1 + OH -1 -7[H +1 ] = [OH -1 ] = 1 X 10 -7 M log[H +1 ]-7pH = -log[H +1 ] = -(-7) = 7
![Molarity to pH for Pure water there ’ s a tiny bit of ionization: H 2 O H +1 + OH -1 -7[H +1 ] = [OH -1 ] = 1 X M log[H +1 ]-7pH = -log[H +1 ] = -(-7) = 7](http://images.slideplayer.com./39/10934315/slides/slide_6.jpg "Molarity to pH for Pure water there ’ s a tiny bit of ionization: H 2 O H +1 + OH -1 -7[H +1 ] = [OH -1 ] = 1 X M log[H +1 ]-7pH = -log[H +1 ] = -(-7) = 7")
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pH 3210.001 M or -3 1 X 10 -3 M 0.01 M or -2 1 X 10 -2 M 0.1 M or -1 1 X 10 -1 M 1 M or 0 1X10 0 M [H +1 ]
![pH M or -3 1 X M 0.01 M or -2 1 X M 0.1 M or -1 1 X M 1 M or 0 1X10 0 M [H +1 ]](http://images.slideplayer.com./39/10934315/slides/slide_7.jpg "pH M or -3 1 X M 0.01 M or -2 1 X M 0.1 M or -1 1 X M 1 M or 0 1X10 0 M [H +1 ]")
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pH to Molarity pH = -log[H +1 ], solve for [H +1 ] -pH = log[H +1 ] antilog(-pH) = [H +1 ] say pH = 5, then –pH = -5 antilog(-5) = 10 -5 the –pH becomes the power of 10!the –pH becomes the power of 10!
![pH to Molarity pH = -log[H +1 ], solve for [H +1 ] -pH = log[H +1 ] antilog(-pH) = [H +1 ] say pH = 5, then –pH = -5 antilog(-5) = the –pH becomes the power of 10!the –pH becomes the power of 10!](http://images.slideplayer.com./39/10934315/slides/slide_9.jpg "pH to Molarity pH = -log[H +1 ], solve for [H +1 ] -pH = log[H +1 ] antilog(-pH) = [H +1 ] say pH = 5, then –pH = -5 antilog(-5) = the –pH becomes the power of 10!the –pH becomes the power of 10!")
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pOH by analogy: pOH is defined as –log[OH -1 ] express [OH -1 ] in scientific notation if [OH -1 ] = 1.0 X 10 -3 M then pOH = -log(10 -3 ) = -(-3) = 3
![pOH by analogy: pOH is defined as –log[OH -1 ] express [OH -1 ] in scientific notation if [OH -1 ] = 1.0 X M then pOH = -log(10 -3 ) = -(-3) = 3](http://images.slideplayer.com./39/10934315/slides/slide_10.jpg "pOH by analogy: pOH is defined as –log[OH -1 ] express [OH -1 ] in scientific notation if [OH -1 ] = 1.0 X M then pOH = -log(10 -3 ) = -(-3) = 3")
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pH + pOH = 14 pH = 3, pOH = pH = 7, pOH = pH = 10, pOH = pH = 9, pOH = pH = 1, pOH =1174 5 13
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ACID or BASE? acids: [H +1 ] [OH -1 ] bases: [OH -1 ] [H +1 ]
![ACID or BASE acids: [H +1 ] [OH -1 ] bases: [OH -1 ] [H +1 ]](http://images.slideplayer.com./39/10934315/slides/slide_13.jpg "ACID or BASE acids: [H +1 ] [OH -1 ] bases: [OH -1 ] [H +1 ]")
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pH range 0 to 14 –with 7 being neutral pH = 0, strongly acidic pH = 14, strongly basic
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if pH = 4if pH = 4 [H +1 ] = ? pOH = ? [OH -1 ] = ?10 antilog(-pH) = [H +1 ] antilog(-4) = 1 x 10 -4 M antilog(-10) = [OH -1 ] 1x10 -10 M = [OH -1 ]
![if pH = 4if pH = 4 [H +1 ] = . pOH = .](http://images.slideplayer.com./39/10934315/slides/slide_16.jpg "[OH -1 ] = 10 antilog(-pH) = [H +1 ] antilog(-4) = 1 x M antilog(-10) = [OH -1 ] 1x M = [OH -1 ].")
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if the [OH -1 ] = 1 X 10 -3 pOH = ? pH = ? [H +1 ] = ? pOH = -log[OH -1 ] = -log(10 -3 ) = -(-3) = 3 14 – 3 = 11 antilog(-11) = 1x10 -11 M
![if the [OH -1 ] = 1 X pOH = . pH = . [H +1 ] = .](http://images.slideplayer.com./39/10934315/slides/slide_17.jpg "pOH = -log[OH -1 ] = -log(10 -3 ) = -(-3) = 3 14 – 3 = 11 antilog(-11) = 1x M.")
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i f the [H +1 ] = 1 x 10 -5 M pH = ? pOH = ? [OH - ] = ?5 14 – 5 = 9 antilog(-9) = 1x10 -9 M
![i f the [H +1 ] = 1 x M pH = pOH = [OH - ] = 5 14 – 5 = 9 antilog(-9) = 1x10 -9 M](http://images.slideplayer.com./39/10934315/slides/slide_18.jpg "i f the [H +1 ] = 1 x M pH = pOH = [OH - ] = 5 14 – 5 = 9 antilog(-9) = 1x10 -9 M")
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6 1x10 -2 1x10 -5 3 Acidic or Basic pOH[OH - ](M) pH[H + ](M) 11 1x10 -3 1x10 -11 A 5 9 1x10 -9 B 2 12 1x10 -12 A 8 1x10 -8 1x10 -6 B
 pH[H + ](M) 11 1x x A 5 9 1x10 -9 B x A 8 1x x10 -6 B](http://images.slideplayer.com./39/10934315/slides/slide_19.jpg "6 1x x Acidic or Basic pOH[OH - ](M) pH[H + ](M) 11 1x x A 5 9 1x10 -9 B x A 8 1x x10 -6 B")
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How to safely test pH instruments – use a pH meter indicators – use a series of indicators see if substance reacts with a metal other than Cu, Ag, or Au NEVER “ taste ”
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Indicator substance that changes color over narrow pH range use several indicators to narrow down pH range of substance
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