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.

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.

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 molar mass of the unknown acid. Be sure your answer has the correct number of significant digits.
A chemistry student weighs out 0.379 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 0.2000 M NaOH solution. Calculate the volume of NaOH solution the student will need to add to reach the final equivalence point. Be sure your answer has the correct number of significant digits.
Part 1 of 2 To a flask, 15.0 mL of 1.25 M HF is added. Then, 3.05 M NaOH is used to titrate the acid sample. Write the balanced net ionic equation for the acid- base reaction. Be sure to include states of matter. Part 2 of 2 00 X 00 ローロ X 3 To determine the concentration of a sample of Ca(OH)2, 1.45 M HCl is added drop-wise using a buret. Write the balanced net ionic equation for the acid- base reaction. Be sure to include states of matter. 0-0 h S
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)
A chemistry student weighs out 0.0570 g of citric acid (H,C,H,0,), a triprotic acid, into a 250. mL volumetric flask and dilutes to the mark with distilled water. He plans to titrate the acid with 0.1900 M NaOH solution. Calculate the volume of NaOH solution the student will need to add to reach the final equivalence point. Be sure your answer has the correct number of significant digits. O mL x10
6. A student titrated 30.00 mL of a hydrochloric acid solution with 1.00 M sodium hydroxide. The sodium hydroxide was initially tilled to the 2.30 mL mark on the burette. Once the level in the burette reached 50.00 mL, the student was forced to refill the burette and did so to the 5.06 mL mark. The endpoint was finally reached when the sodium hydroxide level dropped to 32.09 mL on the burette. What is the molarity of the acid solution? Show work.
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 0.159 g of an unknown monoprotic acid into a 250 mL volumetric flask and dilutes to the mark titrates this solution with 0.0700 M NaOH solution. When the titration reaches the equivalence point, the chemist finds she has added 25.2 mL of NaOH solution. Calculate the molar mass of the unknown acid. Round your answer to 3 significant digits. mol
Calculate the molar mass of the unknown acid. Be sure your answer has the correct number of significant digits.
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)?
Determining the volume of base needed to titrate a given mass of acid.
You titrate a 2.00 mL sample of sulfuric acid with 8.43 mL 0.150 M KOH. Calculate the molarity of the sulfuric acid sample.