5. 8. 9. 10 11 12 13 An analytical chemist weighs out 0.033 g of an unknown monoprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. She then titrates this solution with 0.0700 M NAOH solution. When the titration reaches the equivalence point, the chemist finds she has added 10.2 mL of NaOH solution. Calculate the molar mass of the unknown acid. Round your answer to 2 significant digits. mol Continue Submit As

5. 8. 9. 10 11 12 13 An analytical chemist weighs out 0.033 g of an unknown monoprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. She then titrates this solution with 0.0700 M NAOH solution. When the titration reaches the equivalence point, the chemist finds she has added 10.2 mL of NaOH solution. Calculate the molar mass of the unknown acid. Round your answer to 2 significant digits. mol Continue Submit As

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.102QE

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A bottle of concentrated hydroiodic acid is 57% HI by weight and has a density of 1.70 g/mL. A solution of this strong and corrosive acid is made by adding exactly 10.0 mL to some water and diluting to 250.0 mL. If the information on the label is correct, what volume of 0.988 M NaOH is needed to neutralize the HI solution? Suggest an indicator for the titration.
A titration of 25.00 mL of an unknown HCl solution with 0.1550 M NaOH starts at a buret reading of NaOH of 0.33 mL. The phenolphthalein indicator turns light pink in the acid solution over 30 seconds at a buret reading of 24.19 mL. Write the balanced equation for the neutralization reaction. What is the molarity of the HCl solution?
A chemistry student needs to standardize a fresh solution of sodium hydroxide. She carefully weighs out 350.mg of oxalic acid H2C2O4 , a diprotic acid that can be purchased inexpensively in high purity, and dissolves it in 250.mL of distilled water. The student then titrates the oxalic acid solution with her sodium hydroxide solution. When the titration reaches the equivalence point, the student finds she has used 119.0mL of sodium hydroxide solution. Calculate the molarity of the student's sodium hydroxide solution. Be sure your answer has the correct number of significant digits.
A chemistry student needs to standardize a fresh solution of sodium hydroxide. She carefully weighs out 303 mg of oxalic acid, a diprotic acid that can be purchased inexpensively in high purity, and dissolves it in 250mL of distilled water. The student then titrates the oxalic acid solution with her sodium hydroxide solution. When the titration reaches the equivalence point, the student finds she has used 104.5 mL of sodium hydroxidesolution. Calculate the molarity of the student's sodium hydroxide solution. Round your answer to 3 significant digits.
Oxalic acid dihydrate (H2C2O4 2H2O) can be used to standardize NaOH solution through acid-base titration. To determine the molarity of an unknown NaOH solution, a student weighed out 0.56 g of solid oxalic acid dihydrate and dissolved the solid in 32.8 mL of DI water. The resulting solution was used in a titration with the unknown NaOH solution (3 drops of phenolphthalein was used as an indicator). The balance chemical equation is given below. If the student used 21.21 mL of the unknown NaOH solution in the titration, what is the molarity of the NaOH solution? Keep the correct number of significant figures. H2C2O4 (aq) + 2NaOH (aq) --> Na2C2O4 (aq) + 2H2O (l)
Oxalic acid dihydrate (H2C2O4 2H2O) can be used to standardize NaOH solution through acid-base titration. To determine the molarity of an unknown NaOH solution, a student weighed out 0.56 g of solid oxalic acid dihydrate and dissolved the solid in 32.8 mL of DI water. The resulting solution was used in a titration with the unknown NaOH solution (3 drops of phenolphthalein was used as an indicator). The balanced chemical equation is given below. If the student used 25.71 mL of the unknown NaOH solution in the titration, what is the molarity of the NaOH solution? Keep the correct number of significant figures. H2C2O4 (aq) + 2NaOH (aq) --> Na2C2O4 (aq) + 2H2O (l)
A chemistry student needs to standardize a fresh solution of sodium hydroxide. She carefully weighs out 13.mg of oxalic acid H2C2O4, a diprotic acid that can be purchased inexpensively in high purity, and dissolves it in 250.mL of distilled water. The student then titrates the oxalic acid solution with her sodium hydroxide solution. When the titration reaches the equivalence point, the student finds she has used 11.9mL of sodium hydroxide solution. Calculate the molarity of the student's sodium hydroxide solution. Round your answer to 2 significant digits.
A titration of 25.00 mL of an unknown HCl solution with 0.1240 M NaOH starts at a buret reading for NaOH of 0.53 mL. The phenolphthalein indicator turns light pink in the acid solution for over 30 seconds at a buret reading of 27.30 mL. 5. What was the volume of NaOH dispensed? 6. How many moles of NaOH were dispensed? 7. Write the balanced molecular equation for the neutralization reaction: 8. How many moles of HCl are present in the acid solution? 9. What is the molarity of the unknown HCl solution?
A solution of tartaric acid (H2C4H6O6) with a known concentration of 0.155 M H2C4H4O6 is titrated with a 0.425 M NaOH solution. How many mL of NaOH are required to reach the second equivalence point with a starting volume of 70.0 mL H2C4H4O6, according to the following balanced chemical equation : H2C4H4O6 + 2 NaOH --> Na2C4H4O6 + 2H2O
A chemistry student needs to standardize a fresh solution of sodium hydroxide. She carefully weighs out 51 mg of oxalic acid (H2C2O4), a diprotic acid that can be purchased inexpensively in high purity, and dissolves it in 250 mL of distilled water. The student then titrates the oxalic acid solution with her sodium hydroxide solution. When the titration reaches the equivalence point, the student finds she has used 19.2 mL of sodium hydroxide solution. Calculate the molarity of the student's sodium hydroxide solution.
You are to determine the molarity of an unknown monoprotic acid, acetic acid (HC2H3O3). You prepared a 0.1 M NaOH solution from a 6 M NaOH stock solution. You standardized this solution using KHP (C8H5KO4) and you used this standardized solution to titrate your unknown. The following is the data you collected: Data for standardization of NaOH:Mass of KHP: 0.5000 gThe volume of NaOH solution used: 24.67 mLData for unknown determination:The volume of HC2H3O3 solution used: 30.00 mLThe volume of NaOH solution used: 36.78 mLWhat is the molarity of NaOH? What is the molarity of the unknown acetic acid solution?
0.3456 g of a solid acid is dissolved in 50 mL of water in a flask and a few drops of phenolphthalein are added to the solution. A buret containing 0.2545 M NaOH is prepared with an initial volume of 10.50 mL. The acid is accidentally titrated with the base beyond the end point, so 1.52 mL of 0.187 M HCl are added to the flask. The titration with the base is continued to a final volume reading of 40.55 mL. Calculate the molar mass of the solid acid.