An analytical chemist weighs out 0.170 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 0.1200M NaOH solution. When the titration reaches the equivalence point, the chemist finds she has added 21.1 mL of NaOH solution. Calculate the molar mass of the unknown acid. Round your answer to 3 significant digits. g mol X S

An analytical chemist weighs out 0.170 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 0.1200M NaOH solution. When the titration reaches the equivalence point, the chemist finds she has added 21.1 mL of NaOH solution. Calculate the molar mass of the unknown acid. Round your answer to 3 significant digits. g mol X S

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter3: Mass Relations In Chemistry; Stoichiometry

Section: Chapter Questions

Problem 23QAP

See similar textbooks

Similar questions

Two beakers sit on a balance; the total mass is 167.170 g. One beaker contains a solution of KI; the other contains a solution of Pb(NO3)2. When the solution in one beaker is poured completely into the other, the following reaction occurs: 2 KI(aq) + Pb(NO3)2(aq) 2 KNO3(aq) + PbI2(s) What is the total mass of the beakers and solutions after reaction? Explain completely.
What mass of solid NaOH (97.0% NaOH by mass) is required to prepare 1.00 L of a 10.0% solution of NaOH by mass? The density of the 10.0% solution is 1.109 g/mL.
94. Baking soda (sodium hydrogen carbonate. NaHCO3) is often used to neutralize spills of acids on the benchtop in the laboratory. What mass of NaHCO3 would be needed to neutralize a spill consisting of 25.2 mL of 6.01 M hydrochloric acid solution?
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.
An analytical chemist weighs out 0.167 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 0.0800M NaOH solution. When the titration reaches the equivalence point, the chemist finds she has added 23.2 mL of NaOH solution. Calculate the molar mass of the unknown acid. Round your answer to 3 significant digits. 0 g mol x10 X S
An analytical chemist weighs out 0.182 g of an unknown triprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. She then titrates this solution with 0.0600 M NaOH solution. When the titration reaches the equivalence point, the chemist finds she has added 47.4 mL of NaOH solution. Calculate the molar mass of the unknown acid. Round your answer to 3 significant digits. 0 mol x10 X S
Chemistry An analytical chemist weighs out 0.410g of an unknown triprotic acid into a 250mL volumetric flask and dilutes to the mark with distilled water. She then titrates this solution with 0.0700M NaOH solution. When the titration reaches the equivalence point, the chemist finds she has added 91.5mL of NaOH solution. Calculate the molar mass of the unknown acid. Round your answer to 3 significant digits.
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 0.1700 M NaOH solution. When the titration reaches the equivalence point, the chemist finds she has added 5.4 mL of NaOH solution. Calculate the molar mass of the unknown acid. Round your answer to 2 significant digits.
An analytical chemist weighs out 0.138 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 0.0600M NaOH solution. When the titration reaches the equivalence point, the chemist finds he has added 25.5 mL of NaOH solution. Calculate the molar mass of the unknown acid. Round your answer to 3 significant digits. 0 mol X S 629 OL A
An analytical chemist weighs out 0.192 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 0.0600 M NaOH solution. When the titration reaches the equivalence point, the chemist finds she has added 37.2 mL of NaOH solution. Calculate the molar mass of the unknown acid. Round your answer to 3 significant digits. mol
A chemistry student weighs out 0.425 g of citric acid (H,C,H,O,), a triprotic acid, into a 250. mL volumetric flask and dilutes to the mark with distilled water. He plans to titrate the acid with 0.1400M NaOH solution. Calculate the volume of NaOH solution the student will need to add to reach the final equivalence point. Round your answer to 3 significant digits. 0mL I Don't Know tab Submit esc 2. ! 1 ← X 2 W 5 © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility #3 E ✿ S4 $ 4 R % 5 MacBook Pro T 6 & Y 7
An analytical chemist weighs out 0.101g of an unknown diprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. He then titrates this solution with 0.1400 M NaOH solution. When the titration reaches the equivalence point, the chemist finds he has added 10.8 mL of NaOH solution. Calculate the molar mass of the unknown acid. Round your answer to 3 significant digits.