/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 23 The amount of indicator used in ... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

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.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Over 30 million students worldwide already upgrade their learning with 91影视!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

The \(\mathrm{p} K_{\mathrm{b}}\) s for the bases \(\mathrm{X}^{-}, \mathrm{Y}^{-},\) and \(Z^{-}\) are 2.72 \(8.66,\) and \(4.57,\) respectively. Arrange the following acids in order of increasing strength: HX, HY, HZ.

Specify which of these systems can be classified as a buffer system: (a) \(\mathrm{KNO}_{2} / \mathrm{HNO}_{2}\) (b) \(\mathrm{KHSO}_{4} / \mathrm{H}_{2} \mathrm{SO}_{4}\) (c) HCOOK/HCOOH.

Define buffer solution.

Both \(\mathrm{Ag}^{+}\) and \(\mathrm{Zn}^{2+}\) form complex ions with \(\mathrm{NH}_{3}\). Write balanced equations for the reactions. However, \(\mathrm{Zn}(\mathrm{OH})_{2}\) is soluble in \(6 \mathrm{M} \mathrm{NaOH},\) and \(\mathrm{AgOH}\) is not. Explain.

What is the \(\mathrm{pH}\) of the buffer \(0.10 \mathrm{M} \mathrm{Na}_{2} \mathrm{HPO}_{4} / 0.15 \mathrm{M}\) \(\mathrm{KH}_{2} \mathrm{PO}_{4} ?\)
See all solutions

Recommended explanations on Chemistry Textbooks

Making Measurements

Read Explanation

Organic Chemistry

Read Explanation

Chemistry Branches

Read Explanation

Kinetics

Read Explanation

Inorganic Chemistry

Read Explanation

Nuclear Chemistry

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.