pH and Indicators in Chemistry
Explore the concept of pH and indicators in chemistry to distinguish between acids and bases, understand pH scales, and safely test pH levels using indicators. Learn how indicators change color based on the pH of a solution and practice using indicators to determine pH ranges. Discover the properties of neutral, acidic, and basic solutions through engaging visuals and practical examples.
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Presentation Transcript
Topic: pH and Indicators 1. List the following as an acid or base a) HCl b) KOH c) CH3COOH d)HF 2. Which of the following would have a pH greater than 7 a) HCl b) CH3OH c) KOH d) NaCl
pH scale power (or potential) of Hydrogen Ranges from 0-14 measures H+concentration [H+] the more H+, the more acidic the solution
Acid, Base, or Neutral Neutral solution: pH = 7 [H+] = [OH-] H+1 > OH-1 OH-1 > H+1 Acidic solution: pH LESS THEN 7 Basic solution: pH GREATER THEN 7
How to safely test pH NEVER taste Instruments use a pH meter See if the substance reacts with a metal other than Cu, Ag, or Au Indicators use a series of indicators
Indicator substance that changes color over narrow pH range
What color would the following indicators be in a neutral solution? yellow green colorless purple blue yellow
Use several indicators to narrow down pH range of substance Ex: Three samples of the same solution are tested, each with a different indicator. All three indicators, bromthymol blue, bromcresol green and thymol blue, appear blue The pH of the solution must be greater than_____
Practice using table M 1. What indicator is yellow with a pH 9.8 2. Which indictor is blue with a pH of 5.6 0-3.0 4.5-14 3.1.-4.4 Orange Green Pink 7.7-14 8.4-14 Purple 3.8-5.4 0-3.7 5.5-14 Green 9.7-14 Green
