Homework Help is Here – Start Your Trial Now!
Science
Chemistry
5. In another titration, a student uses 1.023 M HCl solution to standardize a sodium hydroxide solution. Perform the following calculations, assuming there is 1.000 L of HCl solution, and its density is 1.019 g/mL. Show all of your work on this page or on a separate sheet of paper. a. Beginning with the molarity of HCl, calculate the mass percent of HCl in the HCl solution. This calculation should be done all in one string. You should use the density of the solution and the molar mass of HCl in your calculation string. Record your answer to the appropriate number of sf. Mass percent: b. Use the following process to calculate the molality of HCl in the solution. This calculation should be performed in multiple steps, illustrated below. i. Beginning with the volume of HCl solution (1.000 L HC1), determine the grams of total solution. You will need the density of HCl to calculate this. Track the sf in your work below. Example: 2039,56 g solution ii. Beginning with the volume of HCl solution, use the molarity and the molar mass of HCl to determine the mass of HCl (solute). Track the sf in your work below. Example: 12.2256 g iii. Use the unrounded and tracked values from parts į and ii to determine the mass of solvent in grams. Pay close attention to the sig figs for the subtraction! Track the sf in your work below. Example: 335.678 g/ iv. Beginning with the volume of HCl solution, use the molarity and the unrounded and tracked mass of solvent from iii (converted to kg) to determine the molality. This calculation should be done all in one string (including the conversion to kg.)

5. In another titration, a student uses 1.023 M HCl solution to standardize a sodium hydroxide solution. Perform the following calculations, assuming there is 1.000 L of HCl solution, and its density is 1.019 g/mL. Show all of your work on this page or on a separate sheet of paper. a. Beginning with the molarity of HCl, calculate the mass percent of HCl in the HCl solution. This calculation should be done all in one string. You should use the density of the solution and the molar mass of HCl in your calculation string. Record your answer to the appropriate number of sf. Mass percent: b. Use the following process to calculate the molality of HCl in the solution. This calculation should be performed in multiple steps, illustrated below. i. Beginning with the volume of HCl solution (1.000 L HC1), determine the grams of total solution. You will need the density of HCl to calculate this. Track the sf in your work below. Example: 2039,56 g solution ii. Beginning with the volume of HCl solution, use the molarity and the molar mass of HCl to determine the mass of HCl (solute). Track the sf in your work below. Example: 12.2256 g iii. Use the unrounded and tracked values from parts į and ii to determine the mass of solvent in grams. Pay close attention to the sig figs for the subtraction! Track the sf in your work below. Example: 335.678 g/ iv. Beginning with the volume of HCl solution, use the molarity and the unrounded and tracked mass of solvent from iii (converted to kg) to determine the molality. This calculation should be done all in one string (including the conversion to kg.)

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
See similar textbooks
icon
Related questions
Question
5. In another titration, a student uses 1.023 M HCl solution to standardize a sodium hydroxide solution. Perform the following calculations, assuming there is 1.000 L of HCl solution, and its density is 1.019 g/mL. Show all of your work on this page or on a separate sheet of paper. a. Beginning with the molarity of HCl, calculate the mass percent of HCl in the HCl solution. This calculation should be done all in one string. You should use the density of the solution and the molar mass of HCl in your calculation string. Record your answer to the appropriate number of sf. Mass percent: b. Use the following process be performed in multiple steps, illustrated below. i. Beginning with the volume of HCl solution (1.000 L HCI), determine the grams of total solution. You will need the density of HCl to calculate this. Track the sf in your work below. Example: 2039.56 g solution calculate the molality of HCl in the solution. This calculation should ii. Beginning with the volume of HCl solution, use the molarity and the molar mass of HCl to determine the mass of HCl (solute). Track the sf in your work below. Example: 12.2256 g iii. Use the unrounded and tracked values from parts į and ii to determine the mass of solvent in grams. Pay close attention to the sig figs for the subtraction! Track the sf in your work below. Example: 335.678 g/ iv. Beginning with the volume of HCl solution, use the molarity and the unrounded and tracked mass of solvent from iii (converted to kg) to determine the molality. This calculation should be done all in one string (including the conversion to kg.)
Transcribed Image Text:5. In another titration, a student uses 1.023 M HCl solution to standardize a sodium hydroxide solution. Perform the following calculations, assuming there is 1.000 L of HCl solution, and its density is 1.019 g/mL. Show all of your work on this page or on a separate sheet of paper. a. Beginning with the molarity of HCl, calculate the mass percent of HCl in the HCl solution. This calculation should be done all in one string. You should use the density of the solution and the molar mass of HCl in your calculation string. Record your answer to the appropriate number of sf. Mass percent: b. Use the following process be performed in multiple steps, illustrated below. i. Beginning with the volume of HCl solution (1.000 L HCI), determine the grams of total solution. You will need the density of HCl to calculate this. Track the sf in your work below. Example: 2039.56 g solution calculate the molality of HCl in the solution. This calculation should ii. Beginning with the volume of HCl solution, use the molarity and the molar mass of HCl to determine the mass of HCl (solute). Track the sf in your work below. Example: 12.2256 g iii. Use the unrounded and tracked values from parts į and ii to determine the mass of solvent in grams. Pay close attention to the sig figs for the subtraction! Track the sf in your work below. Example: 335.678 g/ iv. Beginning with the volume of HCl solution, use the molarity and the unrounded and tracked mass of solvent from iii (converted to kg) to determine the molality. This calculation should be done all in one string (including the conversion to kg.)
Expert Solution
Step 1

a) Mass percent = ?

 

Moles of HCl are,

Moles = molarity × volume

Moles = 1.023 M × 1.0 L

Moles = 1.023 mol

 

Now the mass of HCl is,

Moles = mass ÷ molar mass

Mass = moles × molar mass

Mass = 1.023 mol × 36.458 g/mol

Mass = 37.30 g

 

Now, the mass of 1.0 L HCl solution is,

Mass = density × volume

Mass = 1.019 g/mL × 1000 mL

Mass = 1019 g 

 Now, the mass percent of HCl in HCl solution is,

Mass percent = (mass of solute ÷ mass of solution) × 100%

Mass percent = (37.30 g ÷ 1019 g) × 100%

Mass percent = 3.66%

Therefore, the mass percent of HCl in the HCl solution is 3.66%.

 

 

 

 

trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 2 steps

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Acid-Base Titrations
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Similar questions
Recommended textbooks for you
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY
SEE MORE TEXTBOOKS