For questions #24 - #26 A student dissolves 1.30g H2SO4 in 700mL solution. 24. What is the molar mass of H2SO4? A.) 98.1g/mol 25. How many moles does the solute contain? A.) 0.0133 mole 26. What is the molarity of the solution? A.) 0.0484 mol/L B.) 48.0g/mol C.) 23.8g/mol C.) 31.4g/mol B.) 0.0357 mole C.) 0.0950 mole D.) 0.0499 mole B.) 0.0190 mol/L C.) 0.0202 mol/L C.) 0.0653 mol/L

For questions #24 - #26 A student dissolves 1.30g H2SO4 in 700mL solution. 24. What is the molar mass of H2SO4? A.) 98.1g/mol 25. How many moles does the solute contain? A.) 0.0133 mole 26. What is the molarity of the solution? A.) 0.0484 mol/L B.) 48.0g/mol C.) 23.8g/mol C.) 31.4g/mol B.) 0.0357 mole C.) 0.0950 mole D.) 0.0499 mole B.) 0.0190 mol/L C.) 0.0202 mol/L C.) 0.0653 mol/L

Introductory Chemistry For Today

8th Edition

ISBN:9781285644561

Author:Seager

Publisher:Seager

Chapter7: Solutions And Colloids

Section: Chapter Questions

Problem 7.105E

See similar textbooks

Similar questions

What kinds of solute particles are present in a solution of an ionic compound? Of a molecular compound?
. Why does the amount of excess solid solute present in a solution not affect the amount of solute that ultimately dissolves in a given amount of solvent?
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.
An experiment calls for 100. mL of 1.25 M HC1. All that is available in the lab is a bottle of concentrated HC1, whose label indicates that it is 12.1 M. How much of the concentrated HC1 would be needed to prepare the desired solution?
What volume of a 0.20MK2SO4 solution contains 57 g of K2SO4?
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.