The following table shows data from the titration of four 10.0 mL samples of a solution containing hydrochloric acid, HCI(aq), using a 0.231 mol/L sodium hydroxide standard solution. Bromothymol blue is used as an indicator to detect when the endpoint is reached. Titration of 10.0 mL HCl(aq) with 0.231 mol/L NaOH(aq) Trial #1 # 2 #3 # 4 final burette reading (mL) 17.9 35.0 22.9 40.1 initial burette reading (mL) 0.3 17.9 5.9 22.9 volume of NaOH(aq) added (mL) colour at endpoint blue green green green a) Select the most consistent trials and calculate the average volume of titrant added. b) Calculate the concentration of the hydrochloric acid solution.

The following table shows data from the titration of four 10.0 mL samples of a solution containing hydrochloric acid, HCI(aq), using a 0.231 mol/L sodium hydroxide standard solution. Bromothymol blue is used as an indicator to detect when the endpoint is reached. Titration of 10.0 mL HCl(aq) with 0.231 mol/L NaOH(aq) Trial #1 # 2 #3 # 4 final burette reading (mL) 17.9 35.0 22.9 40.1 initial burette reading (mL) 0.3 17.9 5.9 22.9 volume of NaOH(aq) added (mL) colour at endpoint blue green green green a) Select the most consistent trials and calculate the average volume of titrant added. b) Calculate the concentration of the hydrochloric acid solution.

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

See similar textbooks

Similar questions

The table has data from the titration of four 10.0 mL samples of a solution containing hydrochloric acid, HCl(aq), using a 0.299 mol/L sodium hydroxide standard solution. Titration of 10.0 mL HCl(aq) with 0.299 mol/L NaOH(aq) Trial #1 #2 #3 #4 final burette reading (mL) 17.9 35.0 22.9 40.1 initial burette reading (mL) 0.3 17.9 5.9 22.9 volume of NaOH(aq) added (mL) colour at endpoint blue green green green a) Select the most consistent trials and calculate the average volume of titrantadded.b) Calculate the concentration of the hydrochloric acid solution.
An analytical chemist weighs out 0.097g of an unknown triprotic acid into a 250mL 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 49.5mL of NaOH solution. Calculate the molar mass of the unknown acid. Be sure your answer has the correct number of significant digits.
Students Mola and Rity were tasked to analyze the acidity of a 10.0-mL fermented milk sample diluted with water in a 250-mL volumetric flask. Mola obtained a 15.0-mL aliquot of this solution, diluted it to 50.0 mL, and then titrated this diluted sample. Titration data were given to Rity and she found out that the 50.0-mL diluted sample contains 0.21 mmol of lactic acid. MW: Lactic Acid (90.08) a. What is the lactic acid concentration (in M) of the titrated sample? b. Determine the lactic acid content (in M) of the 10.0-mL fermented milk sample. c. What is the lactic acid concentration (in %w/v) of the 10.0-mL fermented milk sample?
Calculate the concentration of the following, aqueous solutions. Give your final answer to two decimal places. Hydroxonium ions, H3O+, in a solution of pH 6.4 Calcium hydroxide, Ca(OH)2 in a solution of pH 11.5 Use the ‘oxidation number method’ and balance the unfinished, ionic equation below. SO2 (aq) + IO3- (aq) → SO42- (aq) + I- (aq) Describe how a mixture of pentanoic acid (CH3CH2CH2CH2COOH) and potassium pentanoate (CH3CH2CH2CH2COOK) in solution can act as a buffer solution.
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
A student is trying to determine the concentration of an acetic acid (HC2H3O2) solution. They place 10.00 mL of the solution in a flask and titrate it with a 0.250 M NaOH solution. At the endpoint of the titration, they find that they have used 22.31 mL of the NaOH solution. Based on this information answer the following questions in the answer box provided. a) How many moles of NaOH are used to reach the endpoint? b) How many moles of acetic acid were neutralized by the NaOH added? c) What is the molar concentration (M) of the original acetic acid solution?
A titration of 25.00 mL of an unknown HCl solution with 0.1550 M NaOH starts at a buret reading of NaOH of 0.33 mL. The phenolphthalein indicator turns light pink in the acid solution over 30 seconds at a buret reading of 24.19 mL. Write the balanced equation for the neutralization reaction. What is the molarity of the HCl solution?
A 44.6 mL of 0.103 M HCI is added to an antacid sample. The solution is titrated to a bromophenol blue endpoint using 19.8 mL of 0.0998M NaOH. How many moles and how many grams of the base are in the antacid sample? Assume the active ingredient is MgCO3. Moles of NaOH? Moles of HCl? Moles of MgCO3? Mass of MgCO3?
A 0.7500 g sample of a phosphoric acid (H3PO4) solution with unknown concentration requires 30.00 mL of 0.3375 M NaOH to reach the end point. Calculate the %(m/m) concentration of the phosphoric acid in the unknown solution. H3PO4(aq) + 3NaOH(aq)---> K3PO4(aq) + 3H2O(l)
Calculate the initial concentration of Fe ion in the solution below. Fe3+ (aq) + SCN– (aq) ⇌ FeSCN2+ (aq) Beaker number 0.200 M Fe(NO3)3(mL) 0.00200 M SCN–(mL) H2O(mL) 1 9.54 6.26 33.9
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