Experiment 1. Find the Molarity of NaOH (mol/L) for each trial. Then calculate the average Molarity. See attached table.Experiment 2. Find the Molarity of the unknown solution using the titration data in the experiment 2 table and using the average molarity of NaOH calculated in Experiment#1. See attached table. Experiment 2AcidTrial#1 Trial #2 Trial #325 mLvolume of acid (mL)25 mL 25 mL9.0 mLvolume of NaOH dispensed in the titration at the 9.0 mL 9.0 mLcolor change (mL)Calculations:Molarity of the unknown solution using titration data and standardized NaOHmolarity from Experiment#1. Experiment 1MeasurementsTrial#1Trial#2mass of benzoic acid used (g)pH of benzoic acid solution before titrationinitial volume reading on the burette before titration 0.0 mL 0.0 mL(mL)volume of NaOH dispensed in the titration at thecolor change (mL)Determined Molarity of NaOH (mol/L)0.244 g 0.244 g2.972.97Trial#10.2442.970.0 mLvolume reading on the burette at the color change 20.0 mL 20.0 mL 20.0 mL(mL)20.0 mL 20.0 mL 20.0 mL

The question is based on the titrations. we are titrating a weak acid with a strong base. we need…

Experiment 1 Measurements Trial #1 Trial #2 volume of NaOH dispensed in the titration at the color change (mL) Determined Molarity of NaOH (mol/L) mass of benzoic acid used (g) pH of benzoic acid solution before titration initial volume reading on the burette before titration 0.0 mL 0.0 mL (mL) 0.244 g 0.244 g 2.97 2.97 Trial #1 0.244 2.97 0.0 mL volume reading on the burette at the color change 20.0 mL 20.0 mL 20.0 mL (mL) 20.0 mL 20.0 mL 20.0 mL

Experiment 1 Measurements Trial #1 Trial #2 volume of NaOH dispensed in the titration at the color change (mL) Determined Molarity of NaOH (mol/L) mass of benzoic acid used (g) pH of benzoic acid solution before titration initial volume reading on the burette before titration 0.0 mL 0.0 mL (mL) 0.244 g 0.244 g 2.97 2.97 Trial #1 0.244 2.97 0.0 mL volume reading on the burette at the color change 20.0 mL 20.0 mL 20.0 mL (mL) 20.0 mL 20.0 mL 20.0 mL

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 16.55QE

See similar textbooks

Similar questions

54. According to the titration curve to the right, acid A is 품 9 8 7 6 5 4 3 2 1 Titration Curve of Acid A 0 0 01 02 03 04 05 06 07 08 09 1 OH added (equivalents) A) weak: resists change when 50% titrated. B) strong: resists change when 50% titrated. C) weak; changes dramatically when 100% titrated. D) strong: changes dramatically when 100% titrated. E) It cannot be determined from the information given. because the pH, 55. According to the titration curve to the right, acid A has a pk, of A) 0.2. B) 0.5. C) 3.2. D) 3.8. E) 4.8. 56. According to the titration curve above, acid A has a buffering range of A) 0.3 M to 0.8 MOH. B) 0.9 to 1.0 MOH. C) pH 3.5 to pH 4.2. D) pH 2.8 to pH 3.8. E) pH 2.8 to pH 4.8.
ANSWER BI AND ANY OTHER THREE QUESTIONS SECTION D Question B1 One way to delermine the pKa value is by use ofa pli curve. One student used thie pH curve to determine thc pka value of the weak monoprotic acid. She transferred 25.0 cm' of 0.100 M solution of the acid into a conical flask and measured the pll of the acid solution using a pH mcter accurate to one decimal place. A solution of sodium hydroxide of concentration 0.100 mol dni was added from the burette in small portions until the alkali was present in excess. The pH of the mixture was recorded after each addition of the sodium hydroxide solution. Then she plotted the pH of the solution versus volume of alkali added from the burette and used this graph to determine the acid dissociation constant. 14 12 10- 10 20 30 40 50 VNaOH (ml) a) Calculate mass of the acid required to prepare 100 cm' of 0.1 solution of this acid.(Molar mass of the acid 150 g mol) b) What is the volume of sodium hydroxide added at cquivalence point? c) What…
Question 15 An unknown student takes 25.0 ml sample of an unknown weak base solution with a an unknown concentration and titrates it with H,SO, solution. At half- equivalence point the pH is 11.20, It takes 17ml of HSO, to reach an equivalence point. What would be the concentration of the unknown weak base sample Mit the pOH at equivalence point is 8.03. Must show all your work for any credit and keep you answer to3 decimal places
M of NaOH: 0.100 Volume of HCI 25mL = 0.025L Moles of HCI = 2.5 mol What is the Volume of NaOH equivalence point: What is Moles of NaOH equaivalence point: What is pH at equivalence point? What is calculated pH and experimental pH of NaOH at 0.00 mL , 12.50 mL, 25mL, and 30 mL. Also what is the Error percentage for each one?
Testbank, Question 7 Two buffer solutions of the same pH are prepared. After adding 15 millimoles of acid to 250 mL of one solution, the pH changes by 0.02 pH unit. Adding 15 millimoles of acid to 250 mL of the second solution results in a 0.05 pH unit change. Which statement most accurately describes the differences between the two buffer solutions? OThe second solution has a lower concentration of conjugate base that the first solution. O The first solution has a higher concentration of conjugate acid than conjugate base. OThe second solution has a higher acid to conjugate base ratio than the first solution. OThe first solution has a higher capacity than the second solution. O The first solution has a lower capacity than the second solution.
Part A Find the mass of sodium formate that must be dissolved in 430.0 cm of a 20 M solution of formic acid to prepare a buffer solution with pH 3.40 Express your answer to two signiticant figures and include the appropriate units. Value Units Submit Reguest Answer Nest> Provide Feedback
Calculate the pH at the following points on the titration curve where 50.00 mL of 0.10 M nitric acid is being titrated with 0.15 M NaOH . (0, 10, 25, 50, 75, 100,, 125% titrated) Please answer
v Question Completion Status: QUESTION 13 Consider an acid-base titration in which the base is dispenssd from a burette into a flask containing an acid. If any drops of the base adhere to the inner walls of the flask, but do not ackially mix with the solution, the calculated acid concentration would be O the same as the actual value. O lower than the actual value. O higher than the actual value. O Need more information QUESTION 14 What is the BEST numerical value for the quantity of liquid in the graduated cylinder? Save A Click Save and Submit to save and submit. Click Save All Answers to save all answers.
In the titration today, you will have reached the _______________ when the indicator phenolphthalein has just changed color to pale pink, which signals the reaction is complete. (Actually phenolphthalein only turns pink when a little bit of extra base has been added. ) Group of answer choices: a) titrant b) titration c) indicator d) endpoint e) buffer zone
PLEASE ANSWER ALL PARTS THANK YOU Given:Kb for ammonia of 1.8 X 10-5 Volume of NH3 in flask (mL): 10.00 Average Volume of HCl it took to get to equivalence point (mL): 20.50 Concentration of HCl (M): 0.100Volume of HCl added to calculate “beyond equivalence pH”(mL): 10.50 a) Calculate the concentration of the ammonia.b) Calculate the pH of the contents of the flask (NH3) before the titration begins.c) Calculate the pH of the contents of the flask in the titration at ¼ way to equivalence. This means use your volume added to get to eq point (mL) value but multiply it by ¼ (so you are not yet at equivalence).d) Calculate the pH of the contents of the flask in the titration at ½ way to equivalence (so also not yet at equivalence)e) Calculate the pH of the contents of the flask in the titration at the equivalence point.f) Calculate the pH of the contents of the flask in the titration beyond the equivalence point. Use your given amount
During the titration of 50.0mL of 0.1098M HCl using a standardized 0.0750M NaOH solution, what would be the pH of the solution (round off to 2 decimal points) after the addition of: a.) 0.00mL NaOH total volume? b.) 50.0mL NaOH total volume? c.) 75.0mL NaOH total volume? d.) 100.mL NaOH total volume?
Which of the following is not standardized against sodium carbonate? a) H2SO4 b) NaOH c) HCl Which of the following is not standardized against KHP? a) H2SO4 b) NaOH c) HCl