A student needs to prepare 250 mL of a 0.500 M aqueous solution of sucrose, C,,H,,0, (aq), which is used frequently in biological experiments. 200 mL 250 mL 150 200 100 150 50 100 250 mL B Which type of glassware should be used to make this How should the correct amount of solute be obtained? solution (assuming that the accuracy of the concentration is important)? O Measure out x mo! of solid sucrose on a molemeter. O Measure out x g of solid sucrose on a balance. Measure out x cm of sucrose with a ruler. OC Based on the selected correct unit, what is the value of x? X3D

A student needs to prepare 250 mL of a 0.500 M aqueous solution of sucrose, C,,H,,0, (aq), which is used frequently in biological experiments. 200 mL 250 mL 150 200 100 150 50 100 250 mL B Which type of glassware should be used to make this How should the correct amount of solute be obtained? solution (assuming that the accuracy of the concentration is important)? O Measure out x mo! of solid sucrose on a molemeter. O Measure out x g of solid sucrose on a balance. Measure out x cm of sucrose with a ruler. OC Based on the selected correct unit, what is the value of x? X3D

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

Chapter4: Types Of Chemical Reactions And Solution Stoichiometry

Section: Chapter Questions

Problem 101AE: You wish to prepare 1 L of a 0.02-M potassium iodate solution. You require that the final...

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When a solution is diluted by adding additional solvent, the concentration of solute changes hut the amount of solute present does not change. Explain. Suppose 250. mL of water is added to 125 mL of 0.55 1 M NaCl solution. Explain how you would calculate the concentration of the solution after dilution.
The units of parts per million (ppm) and parts per billion (ppb) are commonly used by environmental chemists. In general, 1 ppm means 1 part of solute for every 106 parts of solution. Mathematically, by mass: ppm=gsolutegsolution=mgsolutekgsolution In the case of very dilute aqueous solutions, a concentration of 1.0 ppm is equal to 1.0 g of solute per 1.0 mL, which equals 1.0 g solution. Parts per billion is defined in a similar fashion. Calculate the molarity of each of the following aqueous solutions. a. 5.0 ppb Hg in H2O b. 1.0 ppb CHCl3 in H2O c. 10.0 ppm As in H2O d. 0.10 ppm DDT (C14H9Cl5) in H2O
A student tries to determine experimentally the molar mass of aspirin (HAsp). She takes 1.00 g of aspirin, dissolves it in water, and neutralizes it with 17.6 mL of 0.315 M KOH. The equation for the reaction is HAsp(aq)+OH(aq)Asp(aq)+H2OWhat is the molar mass of aspirin?
You wish to prepare 1 L of a 0.02-M potassium iodate solution. You require that the final concentration be within 1% of 0.02 M and that the concentration must be known accurately to the fourth decimal place. How would you prepare this solution? Specify the glassware you would use, the accuracy needed for the balance, and the ranges of acceptable masses of KIO3 that can be used.
When 10. L of water is added to 3.0 L of 6.0 M H2SO4, what is the molarity of the resulting solution? Assume the volumes are additive.
How do we define the mass percent composition of a solution? Give an example of a solution, and explain the relative amounts of solute and solvent present in the solution in terms of the mass percent composition.
A 10.00-mL sample of a 24.00% solution of ammonium bromide (NH4Br) requires 23.41 mL of 1.200 molar silver nitrate (AgNO3) to react with all of the bromide ion present. (a) Calculate the molarity of the ammonium bromide solution. (b) Use the molarity of the solution to find the mass of ammonium bromide in 1.000 L of this solution. (c) From the percentage concentration and the answer to part b, find the mass of 1.000 L ammonium bromide solution. (d) Combine the answer to part c with the volume of 1.000 L to express the density of the ammonium bromide solution (in g/mL).
Twenty-five milliliters of a solution (d=1.107g/mL)containing 15.25% by mass of sulfuric acid is added to 50.0 mL of 2.45 M barium chloride. (a) What is the expected precipitate? (b) How many grams of precipitate are obtained? (c) What is the chloride concentration after precipitation is complete?
One mole of CaCl2 is represented as where represents Ca and represents Cl. Complete the picture showing only the calcium and chloride ions. The water molecules need not be shown. What is the molarity of Ca2+? of Cl-?
A cough syrup contains 5.0% ethyl alcohol, C2H5OH, by mass. If the density of the solution is 0.9928 g/mL, determine the molarity of the alcohol in the cough syrup.

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