n Ruffar with Mifforant raneantratione nf Arid and Coniugate. Base: Show work for at least ane full set of dota. Label c
Posted: Fri Jul 15, 2022 5:01 pm
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Show work for at least ane full set of dota. Label calculations by their corresponding letter. Part 1: Determining the pH of Solutions using Acid-Base Indicators and pH Meters. Estimate the pH of each solution from Part 1 of the experiment and determine whether your findings with indicator dyes are consistent with measurements collected with a pH meter. Note, it is not uncommon for an indicator to provide unexpected results for extremely acidic or basic solutions. If a solution turns a color that makes no sense based on its range of colors shown in figure 1 , you may exclude that indicator's results when determining the pH of your solution. Write a net ionic equation showing the acid-base properties for each compound in aqueous solution. Note, ZnSO, has been omitted since highly-charged, small metal ions have unique acid properties. Part 2: Using a pH Meter to Observe Properties of a Buffer Use the Henderson-Hasselbalch equation to calculate the theoretical pH of each solution (originally...before adding any drops of acid or base) and compare this theoretical pH to the average pH measured with the pH meter. (Due to the log scale of pH, it is customary to report absolute error rather than relative (\%) error for pH measurements)