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Chapter 17: Problem 23

The amount of indicator used in an acid-base titration must be small. Why?

Short Answer

Expert verified
In an acid-base titration, the amount of indicator must be small to minimize its interference with the reaction while still providing a clear, observable signal of when the titration has reached its equivalence point.

Step by step solution

01

Understand the role of the indicator

An indicator is used in a titration to signal the point at which the reaction has reached its equivalence point, that is, when the moles of acid equal the moles of base. This is typically shown by a change in color. Since its role is primarily as a signal, only a small amount is required.
02

Discuss the behavior of an indicator

Indicators are weak acids or bases themselves and they can momentarily affect the pH of the solution when added. This deviation could affect the accuracy of the titration, but, given the minute quantities of the indicator used, this influence is negligible.
03

Conclude

Therefore, only a small amount of indicator is used in an acid-base titration to minimize the interference of the indicator with the reaction while still providing a clear, observable signal of when the titration has reached its equivalence point.

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Most popular questions from this chapter

Explain, with balanced ionic equations, why (a) \(\mathrm{CuI}_{2}\) dissolves in ammonia solution, (b) AgBr dissolves in NaCN solution, (c) \(\mathrm{Hg}_{2} \mathrm{Cl}_{2}\) dissolves in \(\mathrm{KCl}\) solution.

A student carried out an acid-base titration by adding \(\mathrm{NaOH}\) solution from a buret to an Erlenmeyer flask containing HCl solution and using phenolphthalein as indicator. At the equivalence point, he observed a faint reddish-pink color. However, after a few minutes, the solution gradually turned colorless. What do you suppose happened?

How can we predict whether a precipitate will form when two solutions are mixed?

Solid NaI is slowly added to a solution that is \(0.010 M\) in \(\mathrm{Cu}^{+}\) and \(0.010 \mathrm{M}\) in \(\mathrm{Ag}^{+}\). (a) Which compound will begin to precipitate first? (b) Calculate \(\left[\mathrm{Ag}^{+}\right]\) when CuI just begins to precipitate. (c) What percentage of \(\mathrm{Ag}^{+}\) remains in solution at this point?

Both \(\mathrm{KCl}\) and \(\mathrm{NH}_{4} \mathrm{Cl}\) are white solids. Suggest one reagent that would enable you to distinguish between these two compounds.
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