(Incorrect) In order to prepare very dilute solutions, a lab technician chooses to perform a series of dilutions instead of measuring a very small mass. A solution was prepared by dissolving 0.360 g of KNO3 in enough water to make 500. mL of solution. A 10.0 mL sample of this solution was transferred to a 500.0-mL volumetric flask and diluted to the mark with water. Then 10.0 mL of the diluted solution was transferred to a 250.0-ml flask and diluted to the mark with water. What is the final concentration of the KNO3 solution? 7.12 × 103 M (Your answer) 2.85 x 10-6 M 7.91 × 10-⁹ M 5.70 x 10-6 M (Correct answer) 1.42 × 10-¹4 M

(Incorrect) In order to prepare very dilute solutions, a lab technician chooses to perform a series of dilutions instead of measuring a very small mass. A solution was prepared by dissolving 0.360 g of KNO3 in enough water to make 500. mL of solution. A 10.0 mL sample of this solution was transferred to a 500.0-mL volumetric flask and diluted to the mark with water. Then 10.0 mL of the diluted solution was transferred to a 250.0-ml flask and diluted to the mark with water. What is the final concentration of the KNO3 solution? 7.12 × 103 M (Your answer) 2.85 x 10-6 M 7.91 × 10-⁹ M 5.70 x 10-6 M (Correct answer) 1.42 × 10-¹4 M

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

Similar questions

Calculate the molarity (to at least three significant digits) of a solution created when 108 mL of a 1.3-M NaCl solution is added to 100. mL of a 2.2-M NaCl solution.
A student has 480.0 mL of a 0.1217 M aqueous solution of LiCl to use in an experiment. He accidentally leaves the container uncovered and comes back the next week to find only a solid residue. The mass of the residue is 3.529 g. Determine the chemical formula of this residue. If the substance is a hydrate, use a period instead of a dot in its formula.
4.67 g of cobalt(II) sulfate are dissolved in water to make 2600. mL of solution. Calculate the molarity. Isa molar mass needed for this calculation? Enter either yes or no, If so, calculate the molar mass using our periodic table and enter with the proper s.f. If not, enter 0. Do not include units. g/mol In the three blanks, enter the results of the calculation: value (decimal notation with proper s.f.)., units, and substance (in this order).
Calculate the molarity of a solution prepared by dissolving 12.50 grams of NaNO3 in 250. mL of solution? The molar mass of NaNO3 is 85.00 g/mol. Write your answer with the correct units on the blank below.
The solution was prepared by adding 150 g of sodium hydroxide to 150 g of water, giving a total weight of 300 g. Density of the solution is 1.53 g/mL What is the molarity of the solution? 2. Pause the Student Protocol video at 1 minute 39 seconds. Now use your molarity in the dilution equation to calculate the number of mL you will need to dilute to make 500 mL of a 0.10 M sodium hydroxide solution.
A diluted NaCl solution is made by mixing 110.5 mL of 1.26 M NaCl with 201.3 mL of water. What is the final concentration of NaCl in the newly diluted solution?
Suppose 20.4 g of ammonium sulfate is dissolved in 150. mL of a 0.70 M aqueous solution of sodium chromate. Calculate the final molarity of ammonium cation in the solution. You can assume the volume of the solution doesn't change when the ammonium sulfate is dissolved in it. Be sure your answer has the correct number of significant digits.
1. A 4.24 g sample of a laboratory solution contains 1.42 g of acid. What is the concentration of the solution as a mass percentage? 2. Isopropyl alcohol is mixed with water to produce a solution that is 35.0% alcohol by volume. How many milliliters of each component are present in 645 mL of this solution?
Sodium carbonate is used in toothpaste where it acts as a foaming agent and an abrasive. Calculate the mass (in grams) of solute needed to prepare 53 mL of a 0.443 mol/L solution of Na2CO3 Record only your numerical answer with the correct number of significant digits. You do not need to include units as the units appear for you beside the answer box already.
A potassium iodide solution is made by mixing 3.241 grams of potassium iodide and mixing it into 248.2 mL of water. Calculate the molarity of this solution.
Suppose 2.33g of zinc chloride is dissolved of zinc chloride is dissolved in 300. mL of a 51.0 mM aqueous solution of potassium carbonate. Calculate the final molarity of zinc cation in the solution. You can assume the volume of the solution doesn’t change when the zinc chloride is dissolved in it.
You are given a solid that is a mixture of Na2SO4 and K₂SO4. A 0.205g sample of the mixture is dissolved in water. An excess of an aqueous solution of BaCl₂ is added. The BaSO4 that is formed is filtered, dried, and weighed. Its mass is 0.298g. What are the percent compositions by mass of Na₂SO4 and K₂SO4 in the sample?