Chapter 4, Problem 71PS

### 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

# If 38.55 mL of HCI is required to titrate 2.150 g of Na2CO3 according to the following equation, what is the concentration (mol/L) of the HCl solution?Na2CO3(aq) + 2HCl(aq) → 2 NaCI(aq) + CO2(g) + H2O(l)

Interpretation Introduction

Interpretation:

The concentration (mol/L) of HCl required to titrate 2.150g of Na2CO3 has to be determined.

Concept introduction:

Numberofmole=GivenmassofthesubstanceMolarmass

• The molar mass of an element or compound is the mass in grams of 1 mole of that substance, and it is expressed in the unit of grams per mol (g/mol).
• For chemical reaction balanced chemical reaction equation written in accordance with the Law of conservation of mass.
• Law of conservation of mass states that for a reaction total mass of the reactant and product must be equal.
• Stoichiometric factor is a relationship between reactant and product which is obtained from the balanced chemical equation for a particular reaction.
• Concentrationofsubstance=Amountof substancevolumeofthesubstance
Explanation

Balanced chemical equation for the given reaction is,

â€‚Â Na2CO3(aq)â€‰+â€‰2HCl(aq)â€‰â†’â€‰H2O(l)â€‰+â€‰CO2(g)+â€‰2â€‰NaCl(aq)

The amount (moles) of Na2CO3 available can be calculated as follows,

â€‚Â 2.150â€‰gâ€‰Na2CO3â€‰Ã—1â€‰molâ€‰Na2CO3106â€‰gâ€‰â€‰=â€‰0.02028â€‰molâ€‰Na2CO3

The balanced equation for the reaction shows that 1â€‰mol of Na2CO3 requires 2â€‰mol of HCl. Â This is the required stoichiometric factor to obtain the amount of HCl present.

Thus the amount of HCl can be calculated as follows,

â€‚Â 0

### Still sussing out bartleby?

Check out a sample textbook solution.

See a sample solution

#### The Solution to Your Study Problems

Bartleby provides explanations to thousands of textbook problems written by our experts, many with advanced degrees!

Get Started