Can you plz help me and thankyou so much 4. Can 1.75 L of water dissolve 4.6 moles of Copper Sulfate CusO.?(please show work)Why?/Why not?5. What is the solution concentration formed from 3.6 moles of solute dissolved into 1.3 L of water?(please show work)近

Formula used : Molarity = no. of moles/ volume

Answered: 4. Can 1.75 L of water dissolve 4.6…

Living By Chemistry: First Edition Textbook

1st Edition

ISBN:9781559539418

Author:Angelica Stacy

Publisher:Angelica Stacy

ChapterU4: Toxins: Stoichiometry, Solution Chemistry, And Acids And Bases

Section: Chapter Questions

Problem SIII7RE

See similar textbooks

Similar questions

What mass of a 4.00% NaOH solution by mass contains 15.0 g of NaOH?
Addition of water to concentrated sulfuric acid is dangerous because it generates enough heat to boil the water, causing it to spatter out of the container. For this reason, chemists remember to add acid to water. In a dilution experiment, we calculate the amount of the more concentrated solution that must be measured out. If we place this concentrated solution (Figure 4.7) in the volumetric flask first, then dilute with water, we violate the caution Add acid to water. Describe a safer variation on the method shown in Figure 4.7 that allows the quantitative dilution of concentrated sulfuric acid. Figure 4.7 Preparing a dilute solution from a concentrated solution. (a) Draw the concentrated solution into a pipet to a level just above the calibration mark. (b) Allow the liquid to settle down to the calibration line. Touch the tip of the pipet to the side of the container to remove any extra liquid. (c) Transfer this solution to a volumetric flask. Again touch the pipet to the wall of the flask to ensure complete transfer, but do not blow out the pipet because it is calibrated for a small amount of liquid to remain in the tip. (d) Dilute to the mark with solvent. Frequently, especially with concentrated acids, it is best to have some solvent present in the volumetric flask before you add the concentrated sample.
What happens if you add a very small amount of solid salt (NaCl) to each beaker described below? Include a statement comparing the amount of solid eventually found in the beaker with the amount you added: a a beaker containing saturated NaCl solution, b a beaker with unsaturated NaCl solution, c a beaker containing supersaturated NaCl solution. A saturated sodium chloride solution.

Recommended textbooks for you

Living By Chemistry: First Edition Textbook

Chemistry

ISBN:

9781559539418

Author:

Angelica Stacy

Publisher:

MAC HIGHER

Introductory Chemistry For Today

Chemistry

ISBN:

9781285644561

Author:

Seager

Publisher:

Cengage

World of Chemistry, 3rd edition

Chemistry

ISBN:

9781133109655

Author:

Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Publisher:

Brooks / Cole / Cengage Learning

Living By Chemistry: First Edition Textbook

Chemistry

ISBN:

9781559539418

Author:

Angelica Stacy

Publisher:

MAC HIGHER

Introductory Chemistry For Today

Chemistry

ISBN:

9781285644561

Author:

Seager

Publisher:

Cengage

World of Chemistry, 3rd edition

Chemistry

ISBN:

9781133109655

Author:

Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Publisher:

Brooks / Cole / Cengage Learning

Chemistry: Matter and Change

Chemistry

ISBN:

9780078746376

Author:

Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Publisher:

Glencoe/McGraw-Hill School Pub Co

Chemistry: The Molecular Science

Chemistry

ISBN:

9781285199047

Author:

John W. Moore, Conrad L. Stanitski

Publisher:

Cengage Learning

Fundamentals Of Analytical Chemistry

Chemistry

ISBN:

9781285640686

Author:

Skoog

Publisher:

Cengage

SEE MORE TEXTBOOKS

4. Can 1.75 L of water dissolve 4.6 moles of Copper Sulfate CuSOa? Why?/Why not? (please show work) 5. What is the solution concentration formed from 3.6 moles of solute dissolved into 1.3 L of water? (please show work)