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Using balanced chemical equations, explain the observed conductivity at the point of faint pink indicator color for:

1) The addition of ammonia to acetic acid.

2) The addition of barium hydroxide to sulfuric acid

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Related questions

A student place 2 mL of a hydrochloric acid solution in an Erlenmeyer flask. She then added 23.3 mL DI water and 2 drops 0.2% phenolphthalein solution. During the titration, a faint, pale pink color was observed when 21.38 mL of 0.272 M barium hydroxide had been added. Calculate the concentration (in M) of the original hydrochloric acid solution.

  1. Write an equation for the chemical reaction that occurred between sulfuric acid and barium hydroxide.
  2. Explain in terms of the properties of the products formed why the light went out when barium hydroxide was added to the sulfuric acid solution, even though both of these reactants are electrolytes.  
  3. Explain why the light came on again when additional barium hydroxide was added.
  1. In the conductivity tests, what controlled the brightness of the light?
  2. Write an equation to show how acetic acid reacts with water to produce ions in solution.
  3. What classes of compounds tested are electrolytes?

 

Phenolphthalein indicator is added to a solution of sulfuric acid. The sulfuric acid solution is prepared by adding 836 uL of 1.00 M sulfuric acid stock solution to 19.16 mL of distilled water. You titrate this sulfuric acid solution using a potassium hydroxide solution. After addition of 35.44 mL of potassium hydroxide, the solution has a pale pink hue. What is the concentration of the potassium hydroxide solution?

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