Titus titrates 45 mL of 0.750 M lactic acid (HC₂H₂O₂, Ka NaOH. = 1.5 x 10 4) using 0.250 M Calculate the pH of the resulting solution at each of the following points in the titration. After adding 24.750000000000004 mL of the NaOH solution: At the equivalence point: After adding 191 mL of the NaOH solution:

Titus titrates 45 mL of 0.750 M lactic acid (HC₂H₂O₂, Ka NaOH. = 1.5 x 10 4) using 0.250 M Calculate the pH of the resulting solution at each of the following points in the titration. After adding 24.750000000000004 mL of the NaOH solution: At the equivalence point: After adding 191 mL of the NaOH solution:

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

A 25.31 ml solution of a weak acid, 0.211M, is titrated with 0.338M. The ka of the acid is 1.3 x 10^-7. Calculate the pH after these volumes of NaOH have been added. Round all answers to two decimal places a. 0.00ml added (a) b. 3.16ml added c. at the equivalence point d. 15.96ml
A student is titrating a 100 mL of 0.50 M solution of hydrofluoric acid (HF) with 1.0 M strong base (NaOH). a) at the equivalence point, what ions/compounds will be present in the solution? A complete answer will also be specific as to what ions/compounds are not present in solution. b) calculate the pH at the equivalence point.
Can you please do A and B thank you!
Determine the mass of solid NaCH₃COO that must be dissolved in an existing 500.0 mL solution of 0.200 M CH₃COOH to form a buffer with a pH equal to 5.00. The value of Ka for CH₃COOH is 1.8 × 10⁻⁵. Need help especially with the setup of the ice table to make sure, to double check, appreciate all the help.
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.
Please don't provide handwritten solution... A 1.0 L solution contains 0.100 mol HC2H3O2 and 0.100 mol NaC2H3O2. The value for Ka HC2H3O2 is 1.8 X 10-5. What is the pH of the buffer after adding 0.010 mol NaOH to the buffer.
Determine the pH during the titration of 11.4 mL of 0.231 M nitric acid by 4.23x10-² barium hydroxide at the following points: (1) Before the addition of any barium hydroxide (2) After the addition of 15.6 mL of barium hydroxide (3) At the equivalence point (4) After adding 39.2 mL of barium hydroxide 4
Do 2
Determine the pH at the point in the titration of 40.0 mL of 0.200 M HNNH2 with 0.100 M HNO: after 10.0 mL of the strong acid has been added. The value of Kb for H2NNH2 is 3.0 x 10-6. PREV 1 2 4 NEXT > Based on your ICE table and definition of Kb, set up the expression for Kb in order to determine the unknown. Do not combine or simplify terms. = 3.0 x 10-6 RESET [0] [0.200] [0.0200] [0.100] [0.140] [0.175] [x] [2x] [0.200 + x] [0.200 - x] [0.0200 + x] [0.0200 - x] [0.100 + x] [0.100 - x] [0.140 + x] [0.140 - x] [0.175 + x] [0.175 - x]
Calculate the pH of the buffers prepared in the following ways: a. by mixing 50.00 mL of 0.200 M ammonium nitrate, NH,NO,, with 25.00 mL 0.200 M NaOH b. by neutralizing half of the acid in 100.00 mL of 0.200 M ammonium nitrate solution with 1.0 M NaOH c. by mixing 60.00 mL of 0.400 M sodium formate (NaCHOO) with 40.00 mL 0.360 M HCI d. by mixing 80.00 mL of 1.00 M NH, with 40.00 mL of 1.00 M HCI e. by mixing equal volumes of 1.00 M NH, and 0.50 M HCI
When pH titrations occur, more data points become necessary at the vertical deflection near the equivalence point which is accomplished by adding smaller volumes of base from the pipers before taking the pH of the solution. Why are more points needed at this point in the titration curve? Why can larger volumes be used in the area outside of this region?
titration of acetic acid: what is the pH after 10.00mL sodium hydroxide solution are added? the mL base needed to reach equivalence point: 25.5 mL