Introduction The objective of the experiment is to utilize acid-base indicators and determine the effect of adding a strong acid or strong base to a buffer solution, and adding a strong acid or strong base to water. For Part 1: Indicator Solutions and Their Colors, 6 indicators: thymol blue, methyl orange, methyl red, bromothymol blue, phenolphthalein, alizarin yellow, were each used to identify the pH of 0.1 M solution of FeSO4, NH4Cl, Na2HPO4, NaH2PO4, Na3PO4, NaCl, NaF, and Na2CO3. For Part 2: Buffer Systems and Their pH, part a, HCl or NaOH were added to an acetate buffer to observe the resistance of changes in pH when small quantities of a strong acid or a strong base are added, and in part b, where drops of NaOH and HCl were added to
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For example, during Part 1 of the experiment, 6 indicators: thymol blue, methyl orange, methyl red, bromothymol blue, phenolphthalein, and alizarin yellow were used along with its respective solution to determine the color change that was present with the addition of each indicator and the color change was used to identify if the solution was acidic or basic. Furthermore, several pH strips were also used during Part 2 of the experiment to approximate the pH value. The 3 - 5.5 pH paper was used to identify the solution 's pH within the 3.3-5.5 pH range. When the solution was outside of the 3-5.5, the Fisher brand 0-14 pH paper was utilized. Structural properties that affect the strengths of acids include the bond strength, which is affected by the ‘A’ atom. If the ‘A’ atom is smaller, the H-A bond is stronger. Going down the rows in the Periodic Table, the atoms increase and the bonds are weaker in terms of strength, and therefore, the acids are stronger. Another property includes bond polarity, which depends on the difference in the electronegativity of the bond of the two atoms. As the atom increases in electronegativity, the product is more stable, the O-H bond is weakened, and thus, a stronger
For example, during Part 1 of the experiment, 6 indicators: thymol blue, methyl orange, methyl red, bromothymol blue, phenolphthalein, and alizarin yellow were used along with its respective solution to determine the color change that was present with the addition of each indicator and the color change was used to identify if the solution was acidic or basic. Furthermore, several pH strips were also used during Part 2 of the experiment to approximate the pH value. The 3 - 5.5 pH paper was used to identify the solution 's pH within the 3.3-5.5 pH range. When the solution was outside of the 3-5.5, the Fisher brand 0-14 pH paper was utilized. Structural properties that affect the strengths of acids include the bond strength, which is affected by the ‘A’ atom. If the ‘A’ atom is smaller, the H-A bond is stronger. Going down the rows in the Periodic Table, the atoms increase and the bonds are weaker in terms of strength, and therefore, the acids are stronger. Another property includes bond polarity, which depends on the difference in the electronegativity of the bond of the two atoms. As the atom increases in electronegativity, the product is more stable, the O-H bond is weakened, and thus, a stronger