   Chapter 4, Problem 53PS

Chapter
Section
Textbook Problem

You have 250. mL of 0.136 M HCl. Using a volumetric pipet, you take 25.00 mL of that solution and dilute it to 100.00 mL in a volumetric flask. Now you take 10.00 mL of that solution, using a volumetric pipet, and dilute it to 100.00 mL in a volumetric flask. What is the concentration of hydrochloric acid in the final solution?

Interpretation Introduction

Interpretation:

The final concentration of HCl after a series of dilution process has to be determined given the initial concentration of 250mLofHCl is 0.136M

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 250mLof0.136MHCl.  Amount of HCl in the 25.0mL solution can be calculated as follows,

AmountofHCl = CHCl×VHCl = 0.136molHClL×0.025L = 0.0034molHCl

0.0034molHCl is in 25.0mL, when it is diluted to 100.00mL the concentration will be,

ConcentrationofHCl =Amountof HClvolumeoftheHCl =0

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