1 A student carries out a titration to determine the molar mass and structure of a weak acid A. The student follows the method below. Dissolve a weighed mass of A in 100 cm3 of distilled water and make the solution up to 250 cm in a beaker. Add the solution of A to a burette. Titrate the solution of A with a standard solution of sodium hydroxide, NAOH. (a) What is meant by the tem standard solution? .*** ......................... .**** (b) Sodium hydroxide is an alkali. What is meant by the term alkali? (c) The student carries out a trial, followed by three further titrations. The diagram shows the initial and final burette readings for the three further titrations. The student measures all burette readings to the nearest 0.05cm3. Titration 1 Titration 2 Titration 3 Initial reading Final reading Initial reading Final reading Initial reading Final reading F27 27 27 28 28 28 29 29 29

1 A student carries out a titration to determine the molar mass and structure of a weak acid A. The student follows the method below. Dissolve a weighed mass of A in 100 cm3 of distilled water and make the solution up to 250 cm in a beaker. Add the solution of A to a burette. Titrate the solution of A with a standard solution of sodium hydroxide, NAOH. (a) What is meant by the tem standard solution? .* ......................... .** (b) Sodium hydroxide is an alkali. What is meant by the term alkali? (c) The student carries out a trial, followed by three further titrations. The diagram shows the initial and final burette readings for the three further titrations. The student measures all burette readings to the nearest 0.05cm3. Titration 1 Titration 2 Titration 3 Initial reading Final reading Initial reading Final reading Initial reading Final reading F27 27 27 28 28 28 29 29 29

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.
In this assignment, you will determine the mass % of an unknown sample of baking soda (NaHCO3) by titrating it with an HCl solution of known concentration. The laboratory will open with a beaker on the stir plate with 1.5000 g of impure solid NaHCO3 and with sufficient water added to make the total volume 25.00 mL. The buret will be filled with 0.3015 M HCl. Pouring HCI until pH is 2. The volume in the buret went from 0 mL to 43 mL Question 1: Calculate the moles of HCl transferred during the titration. (number and unit) (Keep four significant digits in all of the calculations.) Question 2: How many moles of NaHCO3 are present in the sample? Question 3: What mass of NaHCO3 is present in the sample? Question 4: What percent of the original sample mass was NaHCO3?
Explain the difference between pH value of distilled water and the theoretical pH expected.
Sodium benzoate, NaC6H5COO (molar mass 144.1 g mol-1) is a common food preservative. The Ka of benzoic acid, C6H5COOH, is 1.6 X 10-5. A chemist titrates 25.00 mL of a stock solution of sodium benzoate, NaC6H5COO, with 1.20 M HCl solution using a pH meter and an indicator (d) Calculate the pH at the half-equivalence point.
A tablet contains 0.5 g of magnesium hydroxide as the only basic ingredient . The tablet is analysed by dissolving it and titrating with a standard hydrochloric acid solution .The hydrochloric acid solution used in this titration is made by diluting 200 ml of 2M standardised solution to 500 ml 1.Calculate the volume of the HCl solution required to neutralize two of these indigestion tablets dissolved in water to make 35ml solution and calculate the concentration of Cl- in the final solution in mol.dm-3
A weak acid- strong base titration was performed as follows: 10.00 mL of 0.10 M acetic acid 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 acetic acid. (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 10.00 ml of 0.100M NaOH? Select one:a. 8.35b. 6.9c. 7.22d. 7.00
A weak acid- strong base titration was performed as follows: 10.00 mL of 0.10 M acetic acid 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 acetic acid. (Note: The volume of two drops indicator is ignored as it is so tiny compared with 100 mL.) What is the pH of the diluted acid in the flask before adding NaOH? Select one:a. All options are incorrectb. 4.90c. 5.30d. 3.1e. 5.15
calculate molarity of acetic acid in vinegar: (volume of NaOH 3ml, cincentration of NaOH 24.215, titrate average use of NaOH 3.44mL). then convert your M concentration of acetic acid to %w/w, given the density of vinegar is 1.005 g/mL.
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 10.00 ml of 0.100M NaOH? Select one:a. 7.1b. 7.00c. 6.9d. 6.00
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 2.00 ml of 0.100M NaOH? Select one:a. All options are incorrectb. 1.22c. 3.2d. 2.11
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 diluted acid in the flask before adding NaOH? Select one:a. 5.00b. 5.0c. All options are incorrectd. 4.90e. 3.1
Answer questions a through c: a. A CHEM 1215L student prepares a dilute solution of sodium hydroxide, NaOH(aq), starting with 6 M sodium hydroxide. She then titrates a 1.372 g sample of KHP with the dilute sodium hydroxide solution, NaOH (aq), to a phenolphthalein end point. If the titration required 21.84 mL of sodium hydroxide, NaOH(aq), calculate the molar concentration of the sodium hydroxide solution, NaOH (aq). (Remember that KHP is potassium hydrogen phthalate KHC8H4O4, NOT potassium hydrogen phosphorus!) b. The student uses the same sodium hydroxide to titrate 10.00 mL of vinegar to a phe- nolphthalein end point. If the titration required 27.48 mL of sodium hydroxide, NaOH (aq), calculate the molar concentration of acetic acid, HC2H3O2 (aq), in the vinegar. c. Calculate the mass percent of acetic acid, HC2H3O2 (aq), in the vinegar using the mo- lar concentration for acetic acid, HC2H3O2 (aq), determined in part band assuming the density of the solution is 1.01 g/mL.