An analytical chemist weighs out 0.120 g of an unknown diprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. She then titrates this solution with 0.0500 M NaOH solution. When the titration reaches the equivalence point, the chemist finds she has added 35.8 mL of NaOH solution. Calculate the molar mass of the unknown acid. Be sure your answer has the correct number of significant digits. mol

An analytical chemist weighs out 0.120 g of an unknown diprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. She then titrates this solution with 0.0500 M NaOH solution. When the titration reaches the equivalence point, the chemist finds she has added 35.8 mL of NaOH solution. Calculate the molar mass of the unknown acid. Be sure your answer has the correct number of significant digits. mol

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

An analytical chemist weighs out 0.087 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 0.1100 M NaOH solution. When the titration reaches the equivalence point, the chemist finds she has added 11.0 mL of NaOH solution. Calculate the molar mass of the unknown acid. Be sure your answer has the correct number of significant digits. g mol Explanation JAYE A @@ W Recheck > # 3 E 80 F3 $ 4 X 8.88 F4 R S C % 5 F5 T 6 MacBook Air Y & 7 4 F7 U * © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility 8 DII ( 9 DD O O F10 P ?圖 □ 留 m F11 olo Ar (9)
An analytical chemist weighs out 0.112 g of an unknown monoprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. He then titrates this solution with 0.1300M NaOH solution. When the titration reaches the equivalence point, the chemist finds he has added 9.6 mL of NaOH solution. Calculate the molar mass of the unknown acid. Be sure your answer has the correct number of significant digits. mol
You determine the molarity of an unknown acid by titrating it with 0.38 M KOH. You use a 73.08 mL sample of the acid and it requires 24.57 mL of base to reach the endpoint. What is the molarity of the acid? (Only enter the number, do not enter units)
An unknown potassium hydroxide solution is titrated with a standardized solution of hydrochloric acid. It takes 37.4 mL of the base to reach the endpoint when reacting with 25.0 mL of 0.138 M HCl. What is the molarity of the KOH solution?
A student is given 1.52 g of an unknown acid, which can be either oxalic acid, H2C2O4, or citric acid, H3C6H5O7. To determine which acid she has, she titrates the unknown acid with 0.650 M NaOH. The equivalence point is reached when 52.0 mL are added. Answer the following questions to determine the identity of the unknown acid. 1. How many moles of NaOH are consumed? Moles of NaOH = _____ mol 2. How many moles of H+ acid are available to react if the acid is H2C2O4? 0.0403 mol NaOH Moles of H+ from H2C2O4 = ___ mol 3. How many moles of H+ are available to react if the acid is H3C6H5O7? 0.0403 mol NaOH 0.0573 mol H+ from H2C2O4 Moles of H+ from H3C6H5O7 = ___ mol
An analytical chemist weighs out 0.115 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 17.0 mL of NaOH solution. Calculate the molar mass of the unknown acid. Be sure your answer has the correct number of significant digits. g mol
A 4.80 mL sample of an H3PO4 solution of unknown concentration is titrated with a 1.100×10−2 M NaOH solution. A volume of 7.32 mL of the NaOH solution was required to reach the equivalence point. What is the concentration of the unknown H3PO4 solution? Express your answer with the appropriate units.
An analytical chemist weighs out 0.065 of an unknown monoprotic acid into a 250mL volumetric flask and dilutes to the mark with distilled water. She then titrates this solution with 0.1700 M NaOH solution. When the titration reaches the equivalence point, the chemist finds she has added 6.4mL of NaOH solution. Calculate the molar mass of the unknown acid. Round your answer to 2
The iodine contained in every one mL of the 0.010 M iodine solution in the buret will react with 1.76 mg of vitamin C. (In other words, every mL of iodine solution needed for the titration indicates the presence of 1.76 mg of vitamin C in the juice sample.) If your titration used 5.86 mL of iodine solution, what mass of vitamin C is in your fruit juice sample (in milligrams, mg)?
An analytical chemist weighs out 0.191 g of an unknown monoprotic acid into a 250 ml. volumetric flask and dilutes to the mark with distilled water. He then titrates this solution with 0.0600 M NaOH solution. When the titration reaches the equivalence point, the chemist finds he has added 33.7 ml. of NaOH solution. Calculate the molar mass of the unknown acid. Be sure your answer has the correct number of significant digits. e mol D 5
A 34.99 mL sample of an unknown phosphoric acid solution is titrated with a 0.115 M calcium hydroxide solution. The equivalence point is reached when 27.62 mL of calcium hydroxide solution is added. What is the concentration of the unknown phosphoric acid solution? Enter a numerical answer only, in terms of M.
A chemistry student needs to standardize a fresh solution of sodium hydroxide. She carefully weighs out 17. mg of oxalic acid (H,C,0,), 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 16.4 mL of sodium hydroxide solution. Calculate the molarity of the student's sodium hydroxide solution. Round your answer to 2 significant digits. Submit Ass Continue O 2021 McGraw Hill LLC. Al Rights Reserved. Terms of Use I Privacy Center LL