Weak/Strong Acid w/ Strong Base Titrations and pH Indicator Selection Help

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SUMMARY

This discussion focuses on the selection of pH indicators for weak/strong acid-base titrations, specifically using acetic acid and hydrochloric acid with sodium hydroxide. The appropriate indicator for the titration of 0.30 M acetic acid with 0.15 M sodium hydroxide is identified as Thymol Blue, while for the titration of 0.30 M hydrochloric acid with 0.15 M sodium hydroxide, Thymol Blue is also the correct choice. The calculations provided demonstrate the importance of understanding the pH range of indicators in relation to the expected pH at the equivalence point of the titration.

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Homework Statement



Use the information below to answer the following question(s).

methyl orange: red at pH < 3.1: orange at pH 3.1-4.4: yellow-orange above pH 4.4
litmus: red at pH < 4.5: purple at pH 4.5-8.3: blue above pH 8.3
thymol blue: yellow at pH < 8.0: green at pH 8.0-9.6: blue above pH 9.6
trinitrobenzene: colorless at pH < 12: yellow at pH 12.0-1: orange above pH 14.0

Q#1 Weak Acid with Strong Base Titration: Which of the pH indicators from the table would be most appropriate for the titration of 0.30 M acetic acid (Ka = 1.8 × 10-5) with 0.15 M sodium hydroxide?

a.) Litmus
b.) Trinitrobenzene
c.) Methyl Orange
d.) Thymol Blue
e.) None of These

Answer: D Thymol Blue

Q#2 Strong Acid with Strong Base Titration: Which of the pH indicators from the table would be most appropriate for the titration of 0.30 M hydrochloric acid with 0.15 M sodium hydroxide?

a.) Thymol Blue
b.) Methyl Orange
c.) Litmus
d.) Trinitrobenzene
e.) None of These

Answer: A Thymol Blue

I already have the answers as per the information above, I just don't know how to get that answer and I don't know where I'm going wrong. Any help is much appreciated.

Homework Equations



pH = pKa + log [conjugate/weak acid]

The Attempt at a Solution



Q#1 Weak Acid and Strong Base Titration:

HC2H3C2 + OH- ---> C2H3C2- + H2O
Initial 0.30 M HC2H3C2
add 0.15 M OH-
change -015 M HC2H3C2 -0.15 M OH- +0.15 M C2H3C2
Result (0.30-0.15=0.15 M HC2H3C2) ~0 M OH- 0.15 M C2H3C2

pH = pKa + log [conjugate/weak acid]
pH = -log(ka) + log[conjugate/weak acid]
pH = 4.75 + log [0.15/0.15]
pH = 4.75 + 0
pH = 4.75

If the above calculations are correct, I would have picked C "methyl orange" since it seems to somewhat cover the pH range of what I got (4.75) but obviously something is wrong since the answer is NOT methyl orange but rather thymol blue...?

Q#2 Strong Acid with Strong Base Titration

H30+ + OH- -----> 2 H2O
Initial 0.30 M H30+
add 0.15 M OH-
change -0.15 M H30+ -0.15 M OH-
Result (0.30-0.15=0.15 M H30+) ~0 M OH-

pH = -log[H30]
pH = -log[0.15]
pH = 0.82390874

Again, I would have picked Methyl Orange...what am I doing wrong? Help please... :(
 
Last edited:
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