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Understanding Neutralization Reactions and Acid-Base Indicator Changes

This resource explores how chemists write and interpret neutralization reactions involving Arrhenius acids and bases. It emphasizes the reactions that lead to the formation of salt and water and details laboratory techniques such as titration to determine solution concentrations. Essential questions include identifying substances as Arrhenius acids or bases, recognizing pH-related properties of solutions, and understanding alternate acid-base theories like Bronsted-Lowry. By mastering these concepts, students will gain a comprehensive understanding of acid-base chemistry.

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Understanding Neutralization Reactions and Acid-Base Indicator Changes

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Presentation Transcript

  1. Aim: How do chemists write neutralization reactions and interpret changes in acid-base indicator color? In the process of neutralization, an Arrhenius acid and an Arrhenius base react to form a salt and water. Titration is a laboratory process in which a volume of a solution of known concentration is used to determine the concentration of another solution.

  2. Aim: How do chemists write neutralization reactions and interpret changes in acid-base indicator color? Essential Questions: •   Interpret changes in acid-base indicator color •   Write simple neutralization reactions when given the reactants •   Calculate the concentration or volume of a solution, using titration data

  3. Aim: How do chemists write neutralization reactions and interpret changes in acid-base indicator color? Essential Questions: • Given properties, identify substances as Arrhenius acids or Arrhenius bases. • Identify solutions as acid, base, or neutral based upon the pH. • There are alternate acid-base theories. One theory states that an acid is an H+ donor and a base is an H+ acceptor. (Bronsted-Lowry theory)

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