All Waste can mix together and then go down the drain. Hot plates are located in the ends of each lab bench.You may use a transparent test tube holder for your buffer solutions if one is available. This allows you to more easily compare the colors of the unknown solutions to your knowns.Household chemicals are located at the back table with the cabbage. You can find a few different samples. You do not need to bring your own.https://wamaps3.s3.amazonaws.com/cfiles/23139/121_...Question 1:Data and Observations Part A: Cabbage IndicatorpHColor246781012Part B: Cabbage IndicatorSubstanceColorpHAcidic, Basic, or Neutraldish soapshampooglass cleanerQuestion 2:Data and Observations Part C: BuffersFor this section, you may upload an image of your data tables if you prefer. Files will be graded by hand, separately.Total Number of Drops of HCl(aq) AddedDI WaterBuffered SolutionsColorpHColorpH012345Total Number of Drops of NaOH(aq) AddedDI WaterBuffered SolutionsColorpHColorpH012345Question 3:To determine the pH of an unknown solution, a student uses adds 10 drops of red cabbage indicator to the solution, but the solution remains colorless.Can the student determine if the solution is acidic, basic, or neutral? Explain.Question 4:Consider other tests you have carried out on acids and bases during the quarter.Suggest another method for determining if the unknown solution is acidic, basic, or neutral.Question 5:What happened to the pH of DI water when the hydrochloric acid was added to it?A.)What happened to the pH of DI water when the sodium hydroxide was added to it?B.)What happened to the pH of the buffered solution when hydrochloric acid was added to it?C.)What happened to the pH of the buffered solution when sodium hydroxide was added to it?D.)Briefly describe any differences or similarities for any pH changes observed for DI water compared to a buffered solution when hydrochloric acid was added to each.E.)Briefly describe any differences or similarities for any pH changes observed for DI water compared to a buffered solution when sodium hydroxide was added to each.Question 6:Consider a buffer solution that consists of two separate components: the weak acid, HF(aq), and its conjugate base, F-(aq) (added as NaF).Which component will react with H+(aq) from a strong acid? Write the net ionic equation for the reaction that occurs when H+(aq) is added to the buffered solution.Which component will react with OH- (aq) from a strong base? Write the net ionic equation for the reaction that occurs when OH-(aq) is added to the buffered solution.

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