Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Concept explainers
Question
part 1
Which of the following is a best practice in weighing solid samples?
-
Use weighing paper, a watch glass, a beaker, or some other container to measure mass of your solid samples.
-
Do not return the mass settings to zero mark; let the next user tare it for you.
-
Place chemicals directly on the balance pan.
-
For different trials of an experiment, use multiple balances for your measurements
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution
Trending nowThis is a popular solution!
Step by stepSolved in 2 steps
Knowledge Booster
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
- Super fine 40-gauge copper wire has a diameter of only 0.080 mm and weighs only 44.5 g/km. Suppose a spool of 40-gauge wire weighs 624. g less after some wire is pulled off to wind a magnet. How could you calculate how much wire was used? Set the math up. But don't do any of it. Just leave your answer as a math expression. Also, be sure your answer includes all the correct unit symbols. length of wire x10arrow_forward3. When a piece of metal weighing 108 g is submerged in water the volume changes from 36.9 mL to 49.2 mL. Calculate the density of this metal. 4. The accepted value for the density of a certain metal is 6.81 g/cm³ . Calculate the percent error in a laboratory measurement that gives a density value of 6.6 g/cm³ . Express this result in the proper number of significant figures.arrow_forwardPART 3 A Volumetric Flask + A С — ALI50 SOA A 50-mL volumetric flask measures a volume of 50.00 mL. In this experiment, we want to show that this is true. 50.00 mL is the actual volume measured by this volumetric flask. EXPERIMENT: The mass of an empty volumetric flask is measured. Then water is added to the volumetric flask and the meniscus is adjusted to be at the correct level. Then the mass of the volumetric flask and the water is measured. Finally, the temperature of the water in the volumetric flask is measured. RESULTS: Mass of empty volumetric flask = 37.04 g Mass of volumetric flask and water = 86.83 g Temperature of the water in the volumetric flask = 23°C 4 Densities of water at different temperatures: Density of Water at Different Temperatures (g/cm) Temp, °C Density Temp, °C Density Temp, °C Density 18 0.99862 21 0.99802 24 0.99733 19 0.99844 22 0.99780 25 0.99708 20 0.99823 23 0.99757 26 0.99681 (a) Using the mass of the water measured and the density of the water,…arrow_forward
- Measurement and Matter Adding or subtracting and multiplying or dividing measurements 0/3 B A chemistry student must write down in her lab notebook the concentration of a solution of potassium chloride. The concentration of a solution equals the mass of what's dissolved divided by the total volume of the solution. Here's how the student prepared the solution: The label on the graduated cylinder says: empty weight: 1.500 g She put some solid potassium chloride into the graduated cylinder and weighed it. With the potassium chloride added, the cylinder weighed 40.22 g. She added water to the graduated cylinder and dissolved the potassium chloride completely. Then she read the total volume of the solution from the markings on the graduated cylinder. The total volume of the solution was 172.08 mL. What concentration should the student write down in her lab notebook? Be sure your answer has the correct number of significant digits. A Om g·mL -1 □×1 x10 x 5arrow_forwardA student find an irregular metal object. Student wanted to know the identity of this metal. As a chemistry student, you learnt that finding density of the object would be cheap, easy, and reliable method to find the identity. Explain in detail, how would you find the identity of this metal using density? When you explain the method, you show all the steps you will follow (measuring, recording, calculations,.etc) in the laboratory. For example, if you are using a measuring cylinder for taking volume, you must draw diagrams to show every aspects including scale on the cylinder, meniscus, reading,.etcarrow_forward✓ 13 water. 14 A chemist makes 920. mL of zinc nitrate ✓ 15 mol L ✓ 16 0 17 x10 ✓ 18 Calculate the concentration of the chemist's working solution. Round your answer to 3 significant digits. X ✓ 19 ✓ 20 ✓ 21 mol (Zn (NO3)₂) working solution by adding distilled water to 160. mL of a 3.87 stock solution of zinc nitrate in L 22 23 ✓ 24arrow_forward
- please help with all the parts in this question, it is practice so I want to have all the parts to studyarrow_forwardIn the lab you weigh 12.54 g of NaCl to make a stock solution of 5.12 M. To further dilute the solution to 100.0 mL of 0.125 M, how much of the stock solution do you need? Give your answer in mL. Use correct number of significant figures.arrow_forward1. A student overheats their beaker during the dehydration of the copper salt, creating black CuO(s) and Cl2 (g). How will this error change the mass of water calculated? Explain. 2. A student overheats their beaker during the dehydration of the copper salt, creating black CuO(s) and Cl2 (g). How will this error change the mass of copper calculated? Explain. You may assume that the student is able to react all of the CuO with the aluminum wire. 3. A student reports an erroneously-high waters of hydration mass but the correct copper mass for their sample. How will this change the mass of chloride calculated? Explain.arrow_forward
- In a similar experiment, a pair of students was asked to measure out 10.00 mL of water using a 25-mL buret. The data they collected is shown in the table below: Trial Student 1 Student 2 1 9.98 mL 9.97 mL 2 10.00 mL 9.99 mL 3 9.99 mL 10.01 mL Which of the following statements best describes the set of data collected by each student? Student 1 both accurate and precise Student 2 only accurate [ Choose] only accurate both accurate and precise only precisearrow_forwardDuring the experiment, the mass of original sample was 2.226 g, and the mass of copper obtained was 1.239 g. Based on these numbers, calculate the mass of chlorine in the original sample in grams. Include the unit and the three decimal places in your answer.arrow_forwardWhat are your sub-dilutions and what is your total dilution if you made the following serial dilution: 0.4/20 x 0.4/20 x 0.2/20? Provide your answer as a decimal number, not in scientific notation. d1 = Round to 2 decimal points. d2 = Round to 2 decimal points. d3 = Round to 2 decimal points. d(total) = Round to 6 decimal points.arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill EducationPrinciples of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning
- Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill EducationChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningElementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781259911156
Author:Raymond Chang Dr., Jason Overby Professor
Publisher:McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Cengage Learning
Organic Chemistry
Chemistry
ISBN:9780078021558
Author:Janice Gorzynski Smith Dr.
Publisher:McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Elementary Principles of Chemical Processes, Bind...
Chemistry
ISBN:9781118431221
Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:WILEY