An analytical chemist weighs out 0.118 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 0.1100M NAOH solution. When the titration reaches the equivalence point, the chemist finds she has added 32.8 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 0.118 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 0.1100M NAOH solution. When the titration reaches the equivalence point, the chemist finds she has added 32.8 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...

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An analytical chemist weighs out 0.278 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 0.1800M NaOH solution. When the titration reaches the equivalence point, the chemist finds she has added 23.0 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 chemistry student needs to standardize a fresh solution of sodium hydroxide. She carefully weighs out 233. 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 63.2 mL 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.
in a titration to determine the concentration of hydronium ions in a test solution, the test solution was titrated with a 0.250 mol/L sodium hydroxide solution. during several titrations using 55.0 mL of test solution each time, an average of 85.0 mL of sodium hydroxide was used to reach the endpoint. Calculate the molar concentration of the hydronium ions in the test solution.
An analytical chemist weighs out 0.066 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 0.1700M NaOH solution. When the titration reaches the equivalence point, the chemist finds she has added 8.4 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 x10 X S
In a laboratory experiment, a student is conducting a titration. In this titration, a 0.250 M solution of Sodium Hydroxide (NaOH) is added to 30.0 mL of an HCl solution with an unknown concentration. After adding the sodium hydroxide, the student determined that 15.0 mL of NaOH was needed to reach the equivalence point. Based on this information, what was the original concentration of the HCl solution? (Please provide your answer to 3 decimal places.)
To a 25.00 mL volumetric flask, a lab technician adds a 0.100 g sample of a weak monoprotic acid, HA, and dilutes to the mark with distilled water. The technician then titrates this weak acid solution with 0.0841 M KOH. She reaches the endpoint after adding 44.65 mL of the KOH solution. Determine the number of moles of the weak acid in the solution. moles of weak acid: Determine the molar mass of the weak acid. molar mass= pKa mol After the technician adds 16.63 mL of the KOH solution, the pH of the mixture is 5.79. Determine the pK₁ of the weak acid. = g/mol
A titration is a procedure for determining the concentration of a solution by allowing it to react with another solution of known concentration (called a standard solution). Acid-base reactions and oxidation- reduction reactions are used in titrations. For example, to find the concentration of an HCl solution (an acid), a standard solution of NaOH (a base) is added to a measured volume of HCI from a calibrated tube called a buret. An indicator is also present and it will change color when all the acid has reacted. Using the concentration of the standard solution and the volume dispensed, we can calculate molarity of the HCl solution. A volume of 90.0 mL of aqueous potassium hydroxide (KOH) was titrated against a standard solution of sulfuric acid (H₂SO4). What was the molarity of the KOH solution if 13.2 mL of 1.50 M H₂SO4 was needed? The equation is 2KOH(aq) + H₂SO4 (aq)→K₂SO4 (aq) + 2H₂O(1) Express your answer with the appropriate units. ► View Available Hint(s) molarity = Submit…
An analytical chemist weighs out 0.406 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 0.1400M NaOH solution. When the titration reaches the equivalence point, the chemist finds she has added 34.9 mL of NaOH solution. Calculate the molar mass of the unknown acid. Be sure your answer has the correct number of significant digits. C mol Explanation Recheck JAHE B! F2 # 3 80 F3 X $ 4 888 F4 S % LO 5 F5 MacBook Air A 2 F6 & 7 F7 Ⓒ2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Acc * ∞ DII F8 9 FO A F10 4 F11
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
A strong acid-strong base titration was performed as follows: 10.00 mL of 0.10M HCl were collected in an Erlenmeyer flask, and then diluted to 100 mL with distilled water. After that, two drops of indicator were added. Then, the buret was filled with 0.100 M NaOH. The titration was started by slowly adding NaOH to HCl. (Note: The volume of two drops indicator is ignored as it is so tiny compared with 100 mL.) What is the pH of the solution in the Erlenmeyer flask after adding 10.20 ml of 0.100M NaOH? Select one:a. 9.80b. 10.26c. 9.90d. 11.08
To determine the concentration of a solution of sulfurous acid, a 50.00-mL sample is placed in a flask and titrated with a 0.1090 M solution of potassium hydroxide. A volume of 42.82 mL is required to reach the phenolphthalein endpoint. Calculate the concentration of sulfurous acid in the original sample.
A chemistry student weighs out 0.159 g of ascorbic acid (H,C,H,0), a diprotic acid, into a 250. mL volumetric flask and dilutes to the mark with distilled water. He plans to titrate the acid with 0.0800M 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. mL