Which indicator would be the best to use for a titration between 0.20 m hi with 0.10 m ba(oh)2? you will probably need to consul

Question

Licemer1

1 month ago

5

Which indicator would be the best to use for a titration between 0.20 m hi with 0.10 m ba(oh)2? you will probably need to consul

t the appropriate table in the book?

Chemistry

2 answers:

alisha [2.8K] · Answer 1 · 2026-03-08T23:48:17+03:00

1. alizarin yellow R, changes color at pH 10-12
2. thymol blue, changes color at pH 2-4
3. methyl red, changes color at pH 3-5
4. phenolphthalein, changes color at pH 8-10
<span>5. bromothymol blue, changes color at pH 6-8

These are the indicators we can choose from, and the best choice is 5) Bromothymol blue, which changes color at pH 6-8.
Since both HI is a strong acid and Ba(OH)₂ is a strong base, the resulting salt BaI₂ will have a pH of 7, placing it within the effective range of Bromothymol blue.</span>

Tems11 [2.6K] · Answer 2 · 2026-03-08T23:43:51+03:00

For the endpoint at ${\text{pH}}$ 7, the indicator is $\boxed{{\text{bromothymol blue}}}$ .

More Details:

Neutralization reaction:

This describes the reaction between an acid and a base that generates salt and water. It serves to neutralize any excess hydrogen or hydroxide ions in the solution. Applications include decreasing stomach acidity, wastewater treatment, antacids, and managing soil pH. An example of such a reaction is shown in:

${\text{HCl}}+{\text{NaOH}}\to{\text{NaCl}}+{{\text{H}}_2}{\text{O}}$

An indicator is typically a weak acid or weak base used to detect the ${\text{pH}}$ changes in a solution. When dissolved, an indicator splits into ions and imparts color. Acid-base indicators are employed during neutralization reactions.

The titration involving HI and ${\text{Ba}}{\left({{\text{OH}}}\right)_{\text{2}}}$ leads to the following neutralization reaction.

$2{\text{HI}}+{\text{Ba}}{\left( {{\text{OH}}}\right)_2}\to{\text{Ba}}{{\text{I}}_2}+2{{\text{H}}_{\text{2}}}{\text{O}}$

Based on the balanced equation, 2 moles of HI are required to fully neutralize 1 mole of ${\text{Ba}}{\left({{\text{OH}}}\right)_{\text{2}}}$ .

If we consider a volume of 1 L, the moles of HI in a 0.20 M solution equal 0.20 mol. Furthermore, the moles of ${\text{Ba}}{\left({{\text{OH}}}\right)_{\text{2}}}$ in a 0.10 M solution equal 0.10 mol.

Since 1 mole of ${\text{Ba}}{\left({{\text{OH}}}\right)_{\text{2}}}$ can neutralize 2 moles of HI yielding 1 mole of ${\text{Ba}}{{\text{I}}_2}$ , thus for 0.10 moles of ${\text{Ba}}{\left({{\text{OH}}}\right)_{\text{2}}}$ , it completely neutralizes 0.20 moles of HI resulting in 0.10 moles of ${\text{Ba}}{{\text{I}}_2}$ . As this is a neutralization reaction, the final ${\text{pH}}$ of the solution becomes 7.

The appropriate indicator for the endpoint at ${\text{pH}}$ 7 is bromothymol blue, featuring a ${\text{pH}}$ range from pH 6.0 to 7.6.

Further Learning:

1. Why are some amino acids classified as having "acids" in their name yet are basic in water?:

2. Calculate how many moles of water are produced:

Details:

Grade: Senior school

Subject: Chemistry

Chapter: Acid-base reactions

Keywords: Acids, bases, titrations, pH, moles, neutralization reactions, HI, ba(oh)2, 2 moles and 1 mole.