Chapter 4, Problem 53PS

### Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074

Chapter
Section

### Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074
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 250â€‰mLâ€‰ofâ€‰0.136â€‰Mâ€‰â€‰HClâ€‰.Â  Amount of HCl in the 25.0â€‰mL solution can be calculated as follows,

â€‚Â Amountâ€‰ofâ€‰HCl = CHClÃ—â€‰VHCl = 0.136â€‰â€‰molâ€‰HClLâ€‰Ã—â€‰0.025â€‰L = 0.0034â€‰â€‰molâ€‰HCl

0.0034â€‰â€‰molâ€‰HCl is in 25.0â€‰mL, when it is diluted to 100.00â€‰mL the concentration will be,

â€‚Â Concentrationâ€‰ofâ€‰HCl =Amountâ€‰ofÂ HClvolumeâ€‰ofâ€‰theâ€‰HCl =0

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