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Published byAdele Casey Modified over 9 years ago
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Acid-base indicators An acid base indicator is a special substance that exists in two forms ( colours) depending on it’s pH level. We have already talked about one of the most common indicators litmus (Lt)
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Acid-Base Indicators substances composed of a conjugate weak acid-base pair that changes color with changes in pH see table on pg 10 of Data Book or in the back cover of your text book.
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the general equation for the reaction occurring in indicators is: where “In” is the indicator formula HIn (aq) + H 2 O (aq) In - (aq) + H 3 O + (aq)
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Le Chatelier’s Principle is applied to determine the color change when an acid (H 3 O + (aq) ) is added, adding a product shifts the reaction left causing the corresponding color change adding a base will remove H 3 O + (aq)
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Predict the color of each for the specified pH: bromocresol green at 2.8 phenol red at 8.5 cresol red at 1.6 cresol red at 8.0 methyl violet at 1.0
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answers bromocresol green at 2.8=yellow phenol red at 8.5=red cresol red at 1.6=yellow cresol red at 8.0=orange ( red/yellow) methyl violet at 1.0=green ( yellow/blue)
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A solution was tested with several indicators to determine the pH. The following results were obtained. What is the pH of the solution? orange IV - yellow, bromoscresol green - blue, phenol red - yellow, and bromothymol blue - yellow.
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answer orange IV – yellow so pH>2.8 bromoscresol green – blue so pH>5.4 phenol red – yellow so pH<6.6 bromothymol blue – yellow so pH <6.0 So the 5.4<pH<6.0
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assignment Read page 245-247 Lab exercise 6.B on page 247 Do page 247 #1-4
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