A solution of an unknown weak base (0.495 g in 100 mL of water) was prepared andtitrated with standardized 0.113 M HCÌi and the pH of the solution was plotted as afunction of titrant added (shown below).Titration of a Weak Base With 0.113 M HCI1210102030405060708090Volume of HCl added (ml)Possible identities for the three liquid bases are shown in the table below.Basepyrolepyrimidinepyridinetriethylamine2.51 x 10-141.25 x 10-131.70 x 10-95.30 x 104Density (g/mL)0.9671.020.9820.762Based on the data above, identify the weak base and explain your selection. Thebest explanations will account for all relevant experimental data. Additionally,suggest an indicator to use for this titration if it were to be done without a pHmeter.Hd

Here we have to select which of the following bases is weak based on the given data. Data: Molarity…

A solution of an unknown weak base (0.495 g in 100 mL of water) was prepared and titrated with standardized 0.113 M HCİ and the pH of the solution was plotted as a function of titrant added (shown below). Titration of a Weak Base With 0.113 M HCI 12 10 2 10 20 30 40 50 60 70 80 90 Volume of HCl added (mL) Possible identities for the three liquid bases are shown in the table below. Base рyrole pyrimidine pyridine triethylamine K 2.51 x 10-14 1.25 x 10-13 1.70 x 109 5.30 x 104 Density (g/mL) 0.967 1.02 0.982 0.762 Based on the data above, identify the weak base and explain your selection. The best explanations will account for all relevant experimental data. Additionally, suggest an indicator to use for this titration if it were to be done without a pH meter.

A solution of an unknown weak base (0.495 g in 100 mL of water) was prepared and titrated with standardized 0.113 M HCİ and the pH of the solution was plotted as a function of titrant added (shown below). Titration of a Weak Base With 0.113 M HCI 12 10 2 10 20 30 40 50 60 70 80 90 Volume of HCl added (mL) Possible identities for the three liquid bases are shown in the table below. Base рyrole pyrimidine pyridine triethylamine K 2.51 x 10-14 1.25 x 10-13 1.70 x 109 5.30 x 104 Density (g/mL) 0.967 1.02 0.982 0.762 Based on the data above, identify the weak base and explain your selection. The best explanations will account for all relevant experimental data. Additionally, suggest an indicator to use for this titration if it were to be done without a pH meter.

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

(Answer highlighted questions please) A 50.050.0 mL solution of 0.1390.139 M KOHKOH is titrated with 0.2780.278 M HClHCl. Calculate the pH of the solution after the addition of each of the given amounts of HClHCl. 20.0 mLpH=20.0 mLpH= 24.0 mLpH=24.0 mLpH= 25.0 mLpH=25.0 mLpH=
Select ALL of the following that can be determined from the titration of a strong, monoprotic acid with a standardized solution of sodium hydroxide? moles of acid in the titration moles of hydroxide ions used in the titration mass of acid titrated | volume of sodium hydroxide used in the titration Select ALL of the following quantities that must be used in a titration calculation to find the identity of an unknown strong acid: concentration of the standardized base solution stoichiometric ratio of acid to base volume of the acid solution used in the titration volume of the base used in the titration at the equivalence point Need Help?
A student obtains the following data from the Determining the pKa of an Acid-Base Indicator experiment. Using this data, calculate the pKa of the indicator in the fourth solution. Solution Abs. pH 3.4 + HCI 0.054 pH 4.6 + NaOH 0.564 Sample # actual pH Abs. 1 3.48 0.130 2345 3.77 0.217 3.99 0.296 4.37 0.388 4.54 0.468 Your Answer: Answer (2 points) After creating a graph of pH versus log([HIn]/[In-]), the following trendline is obtained. = -1.0291× + 3.721 y=-1 Calculate the pKa of bromophenol blue from this data to three decimal places. Your Answer: Answer MacBook Pro
Question Completion Status: For Solution A, approximately how many mL of HCI were needed to exceed the buffering capacity of this solution? Enter the number only. Don't enter units as part of your answer and don't use commas or scientific notation. Titration curve of Solution A 14 13 12 11- 10 9 8 pH 7 6 5 4 3 2 1 5 4 3 2 1 HCI added (mL) 0 1 2 3 4 5 NaOH added (mL) 14 13 12- 11 10 9 8 pH 7 6.8 2 65 4 3 2 1 Titration curve of Solution B Click Save and Submit to save and submit. Click Save All Answers to save all answers. 54 32 1 HCI added (mL) 0123 NaOH added (mL)
A 29.83 mL aliquot of weak base that has a concentration of 0.542 M will be titrated with 0.712 M HCl. Calculate the pH of of the solution upon the addition of 33.32 mL of HCl. The Kb of the weak base is 4.4 × 10-7
Determine the pH during the titration of 20.0 mL of 0.110 M perchloric acid by 7.69x10-2 M barium hydroxide at the following points: (1) Before the addition of any barium hydroxide (2) After the addition of 7.15 mL of barium hydroxide (3) At the equivalence point (4) After adding 18.3 mL of barium hydroxide
Regarding titrations, which of the following is TRUE? A plot of pH vs. the [base]/[acid] ratio is known as a titration curve. The equivalence point is when the moles of base equals the moles of acid during any acid–base titration. Indicators do not respond to changes in pH. The pH is always 7 once the equivalence volume has been delivered. None of the answers are true.
The volume required to reach the equivalence point of an acid– base titration depends on the volume and concentration of the acid or base to be titrated and on the concentration of the acid or base used to do the titration. It does not, however, depend on the whether or not the acid or base being titrated is strong or weak. Explain.
You have an unknown solution whose initial pH is 2.90. Addition of 10 ml of the titrant increased the pH to 4.15. Adding small-volume increments of the titrant causes the pH to increase very slightly. At equivalence point, the pH of the solution is at 8.70. Abrupt increase in pH to 10.00 was observed when 0.1 ml of titrant was added after equivalence point. Addition of few more drops of the titrant just increase the pH even more with no buffering region. Which among the choices best describes the analyte? The analyte is a strong monoprotic acid. The analyte is a weak monoprotic acid. The analyte is a weak monoprotic base. O The analyte is a weak diprotic acid. O The analyte is a weak diprotic base.
For an aqueous solution formed by mixing 4.50mL of 0.15M LIOH with 25.0mL of 0.100M C2H5CO2H (propanoic acid), a) determine whether this forms a buffer solution. b) determine the pH of this combined solution. c) state whether the addition of 6.75mL of 0.100M HCl to the solution will have a large or small effect on the pH of the solution. Explain your reasoning (using 1-2 sentences).
A 50.0-ml sample of 0.20 M hydrochloric acid (HCI) is titrated with 0.5 M LIOH. Determine the pH of the solution after the following volumes of LIOH titrant are added. Express your answers to two decimal places. a) pH after 10 mL of LIOH added: b) pH after 20 mL of LIOH added: c) pH after 30 mL of LIOH added: Check
An aqueous solution of an unknown solid salt was placed into five different test tubes. Into each test tube a couple of drops of different indicators were then added to each test tube and the color of the indicator in the solution was recorded as shown below. What is the approximate pH of the solution? Test pH Acid Base Color in Unknown Indicator tube Range Color Color Solution 3.0 - 1 Methyl orange 4.4 Red Yellow Yellow 3.0 - Congo Red Purple Red Red 5.0 Bromcresol 3.8 - Yellow Blue Blue Green 5.4 Bromthymol 6.0 - 7.6 4 Yellow Blue Yellow Blue 8.2 - Phenolphthalein Colorless Blue Colorless 10.0 4.3 O 8.4 O 5.2 6.7