   Chapter 4, Problem 54PS

Chapter
Section
Textbook Problem

Suppose you have 100.00 mL of a solution of a dye and transfer 2.00 mL of the solution to a 100.00-mL volumetric flask. After adding water to the 100.00 mL mark, you take 5.00 mL of that solution and again dilute to 100.00 Ml. If you find the dye concentration in the final diluted sample is 0.000158 M, what was the dye concentration in the original solution?

Interpretation Introduction

Interpretation:

The concentration of dye in the original solution after a series of dilution process should be determined.  The final concentration of dye is 0.000158M

Concept Introduction:

• Concentration of solutions can be expressed in various terms; molarity is one such concentration expressing term.
• Molarity (M) of a solution is the number of gram moles of a solute present in one liter of the solution.

Molarity=MassperlitreMolecular mass

• A solution containing one gram mole or 0.1 gram of solute per litre of solution is called molar solution.
• Concentrationofsubstance=Amountof substancevolumeofthesubstance
• Amountof substance=Concentrationofsubstance×volumeofthesubstance
Explanation

We have dye with 0.000158M concentration.

Amount of dye in the 100mL solution can be calculated as follows,

Amountofdye = Cdye×Vdye =0.000158moldyeL×0.1L =0.0000158moldye

The concentration of the solution in 5mL will be,

Concentrationofdye =Amountof dyevolumeofthedye =0

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