Homework Help is Here – Start Your Trial Now!
Science
Chemistry
6. Calculate the moles of NAHCO; in the sample and record the data in the data table. Data Table mass NaHCO; moles NaHCO; liters NaHCO; 7. The molarity is calculated using the formula: mass solute/ moles solute molarity = 1. solution molar mass solute I. solution

6. Calculate the moles of NAHCO; in the sample and record the data in the data table. Data Table mass NaHCO; moles NaHCO; liters NaHCO; 7. The molarity is calculated using the formula: mass solute/ moles solute molarity = 1. solution molar mass solute I. solution

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
100%
Week 11: Converting Concentrations to Different Units Occasionally, when making solutions in the laboratory, it is convenient to make a solution with a certain concentration unit, such as molarity, and then convert the concentration to a different unit. In this assignment, you will make a sodium bicarbonate (baking soda) solution of a certain molarity and then convert that concentration to molality, mass percent, and mole fraction. 1. Start Virtual ChemLab, select Reactions and Stoichiometry, and then select Converting Concentrations to Different Units from the list of assignments. The lab will open in the Titration laboratory. 2. In the laboratory, a bottle of baking soda (sodium bicarbonate, NaHCO;) will be next to the balance, and an empty beaker will be on the stir plate. Drag the empty beaker to the spotlight next to the balance, click in the Balance area to zoom in, place a weigh paper on the balance, and tare the balance. 3. Open the bottle by clicking on the lid (Remove Lid). Pick up the Scoop and scoop out some sample by first dragging the scoop to the mouth of the bottle and then pulling the scoop down the face of the bottle. As the scoop is dragged down the face of the bottle, it will pick up different quantities of solid. Select the largest sample possible and drag the scoop to the weighing paper on the balance until it snaps in place and then let go. This will put approximately 1 g of sample on the balance. Repeat this process six additional times so there is approximately 7.0 g of sample. Record the mass of the NAHCO; in the data table. 4. Drag the weigh paper to the beaker and add the NaHCO; sample to the beaker. Click on the green Zoom Out arrow to return to the laboratory. 5. Drag the beaker to the 50 mL graduated cylinder (the largest one) by the sink and empty the sample into the cylinder. Hold the cylinder under the tap until it fills with water to make an aqueous solution of NAHCO;. (When the graduated cylinder is full, it will automatically snap back into place.) Note that the solid is added and dissolved before the volume is measured when making a molar solution. Chemists normally use a volumetric flask for making molar solutions, but this is not available in the simulation. Record the volume of the solution, in L, in the data table. 6. Calculate the moles of NAHCO; in the sample and record the data in the data table. Data Table mass NaHCO; moles NAHCO; liters NaHCO; 7. The molarity is calculated using the formula: mass solute/ moles solute /molar mass solute I. solution molarity = I. solution
Transcribed Image Text:Week 11: Converting Concentrations to Different Units Occasionally, when making solutions in the laboratory, it is convenient to make a solution with a certain concentration unit, such as molarity, and then convert the concentration to a different unit. In this assignment, you will make a sodium bicarbonate (baking soda) solution of a certain molarity and then convert that concentration to molality, mass percent, and mole fraction. 1. Start Virtual ChemLab, select Reactions and Stoichiometry, and then select Converting Concentrations to Different Units from the list of assignments. The lab will open in the Titration laboratory. 2. In the laboratory, a bottle of baking soda (sodium bicarbonate, NaHCO;) will be next to the balance, and an empty beaker will be on the stir plate. Drag the empty beaker to the spotlight next to the balance, click in the Balance area to zoom in, place a weigh paper on the balance, and tare the balance. 3. Open the bottle by clicking on the lid (Remove Lid). Pick up the Scoop and scoop out some sample by first dragging the scoop to the mouth of the bottle and then pulling the scoop down the face of the bottle. As the scoop is dragged down the face of the bottle, it will pick up different quantities of solid. Select the largest sample possible and drag the scoop to the weighing paper on the balance until it snaps in place and then let go. This will put approximately 1 g of sample on the balance. Repeat this process six additional times so there is approximately 7.0 g of sample. Record the mass of the NAHCO; in the data table. 4. Drag the weigh paper to the beaker and add the NaHCO; sample to the beaker. Click on the green Zoom Out arrow to return to the laboratory. 5. Drag the beaker to the 50 mL graduated cylinder (the largest one) by the sink and empty the sample into the cylinder. Hold the cylinder under the tap until it fills with water to make an aqueous solution of NAHCO;. (When the graduated cylinder is full, it will automatically snap back into place.) Note that the solid is added and dissolved before the volume is measured when making a molar solution. Chemists normally use a volumetric flask for making molar solutions, but this is not available in the simulation. Record the volume of the solution, in L, in the data table. 6. Calculate the moles of NAHCO; in the sample and record the data in the data table. Data Table mass NaHCO; moles NAHCO; liters NaHCO; 7. The molarity is calculated using the formula: mass solute/ moles solute /molar mass solute I. solution molarity = I. solution
7. The molarity is calculated using the formula: moles solute mass solute/ L solution molar mass solute L solution molarity = Beyond Labz, all rights reserved Calculate the molarity of the NaHCO; solution in units of molL. 8. If the density of the solution is 1.047 giml, calculate the molality of the solution in units of molkg. 9. Calculate the mass percent of sodium bicarbonate in the solution. 10. Calculate the mole fraction of sodium bicarbonate in the solution.
Transcribed Image Text:7. The molarity is calculated using the formula: moles solute mass solute/ L solution molar mass solute L solution molarity = Beyond Labz, all rights reserved Calculate the molarity of the NaHCO; solution in units of molL. 8. If the density of the solution is 1.047 giml, calculate the molality of the solution in units of molkg. 9. Calculate the mass percent of sodium bicarbonate in the solution. 10. Calculate the mole fraction of sodium bicarbonate in the solution.
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 4 steps

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Solutions
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.
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