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Chapter 4: Problem 75

Describe the basic steps involved in an acid-base titration. Why is this technique of great practical value?

Short Answer

Expert verified
The basic steps in an acid-base titration involve choosing an indicator, placing the unknown solution in a flask, gradually adding a known solution until the neutralization point is reached, and then calculating the concentration of the unknown solution. This technique is of great practical value as it's used widely in areas like water testing, medical testing and food quality assurance.

Step by step solution

01

Introduction to Acid-Base Titration

An acid-base titration is a quantitative chemical analysis used to determine the concentration of an unknown acid or base solution by neutralizing it with a known concentration of the other.
02

Preparation - Step 1

First, choose an appropriate indicator that would show the end point of the reaction. An indicator is a substance that changes color at or near the neutralization point.
03

Setup - Step 2

Place a known volume of the solution with an unknown concentration in a flask. Add a few drops of the chosen indicator.
04

Titration - Step 3

Gradually add the other solution with a known concentration from a burette into the flask and mix them together. The solution from the burette is added slowly until the indicator changes color, indicating that the reaction has reached the neutralization point, or equivalence point.
05

Result Calculation - Step 4

By using the known volume of the added solution and its known concentration, calculate the concentration of the unknown solution using the equation: \(M_1V_1 = M_2V_2\), where \(M_1\) and \(M_2\) are the molarities of the two solutions and \(V_1\) and \(V_2\) are their volumes.
06

Practical Value of Acid-Base Titration

Acid-base titration is of great practical value because it allows scientists and researchers to determine unknown concentrations of acids or bases in a variety of settings. These include testing the quality of water, determining blood pH in medical testing, and assessing acidity in food and beverages. It is also an essential technique taught in many chemistry laboratories.

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Most popular questions from this chapter

How many grams of \(\mathrm{KOH}\) are present in \(35.0 \mathrm{~mL}\) of a \(5.50 \mathrm{M}\) solution?

A \(3.664-\mathrm{g}\) sample of a monoprotic acid was dissolved in water and required \(20.27 \mathrm{~mL}\) of a \(0.1578 \mathrm{M}\) \(\mathrm{NaOH}\) solution for neutralization. Calculate the molar mass of the acid.

A \(1.00-\mathrm{g}\) sample of a metal \(\mathrm{X}\) (that is known to form \(\mathrm{X}^{2+}\) ions) was added to a \(0.100 \mathrm{~L}\) of \(0.500 \mathrm{M}\) \(\mathrm{H}_{2} \mathrm{SO}_{4}\). After all the metal had reacted, the remaining acid required \(0.0334 \mathrm{~L}\) of \(0.500 \mathrm{M} \mathrm{NaOH}\) solution for neutralization. Calculate the molar mass of the metal and identify the element.

Ammonium nitrate \(\left(\mathrm{NH}_{4} \mathrm{NO}_{3}\right)\) is one of the most important nitrogen-containing fertilizers. Its purity can be analyzed by titrating a solution of \(\mathrm{NH}_{4} \mathrm{NO}_{3}\) with a standard \(\mathrm{NaOH}\) solution. In one experiment a \(0.2041-\mathrm{g}\) sample of industrially prepared \(\mathrm{NH}_{4} \mathrm{NO}_{3}\) required \(24.42 \mathrm{~mL}\) of \(0.1023 \mathrm{M} \mathrm{NaOH}\) for neutralization. (a) Write a net ionic equation for the reaction. (b) What is the percent purity of the sample?

Identify the following as a weak or strong acid or base: (a) \(\mathrm{NH}_{3},\) (b) \(\mathrm{H}_{3} \mathrm{PO}_{4},\) (c) \(\mathrm{LiOH},\) d) \(\mathrm{HCOOH}\) (formic acid), (e) \(\mathrm{H}_{2} \mathrm{SO}_{4},\) (f) \(\mathrm{HF},(\mathrm{g}) \mathrm{Ba}(\mathrm{OH})_{2}\)
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