Use the References to access important values if needed for this question. A 21.4 ml sample of 0.263 M triethylamine, (C,H5)3N, is titrated with 0.253 M perchloric acid. After adding 34.5 mL of perchloric acid, the pH is Use the Tables link in the References for any equilibrium constants that are required. Submit Answer Retry Entire Group 1 more group attempt remaining

Use the References to access important values if needed for this question. A 21.4 ml sample of 0.263 M triethylamine, (C,H5)3N, is titrated with 0.253 M perchloric acid. After adding 34.5 mL of perchloric acid, the pH is Use the Tables link in the References for any equilibrium constants that are required. Submit Answer Retry Entire Group 1 more group attempt remaining

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

please complete all 3 question to complete for 1. Use ICE table neatly and clean
Can you confidently determine if the molarities are accurate? Explain why or why not.
Determine the pH of a buffer solution by constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. Complete Parts 1-3 before submitting your answer. 3 > A solution is prepared with 0.55 M HNO2 and 0.75 M KNO2. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products. Initial (M) Change (M) Equilibrium (M) -2x 0.75 -2x 0 1 HNO₂(aq) 0.55 + x 0.55 -X 0.55-x 0.55 0.55 - x 0.75 2 H₂O(l) III 0.55 + 2x 6.8 x 104 0.55 - 2x 1L +x H3O+(aq) 0.75 + x +x -X 0.75-x + NO₂ (aq) RESET +2x NEXT 0.75 + 2x +x
just tell me the answer option
Do the 2nd and 3rd questions according to the table below. Indicator Acid color Color change, pH range Base color Methyl orange Red 3.1-4.5 Yellow Brome tymol blue Yellow 6.0-7.6 Blue 2) When the above-mentioned indicators are dropped into the two separate 10* M HCI solution, what will the color of solutions be respectively? A. Red, blue B. Red, yellow C. Yellow, yellow D. Yellow, blue E. Orange, green 3) When the above-mentioned indicators are dropped into the two separate 10 M NAOH solution, what will the color of solutions be respectively? A. Red, blue B. Red, yellow C. Yellow, yellow D. Yellow, blue E. Orange, green В. When the above-mentioned indicators are dropped into the 0.1 M NH3, what will the color of solution be? K, for NH3: 1x105
A 28.6 mL sample of 0.378 M dimethylamine, (CH3)2NH, is titrated with 0.202 M hydrochloric acid. After adding 21.5 mL of hydrochloric acid, the pH is Use the Tables link in the References for any equilibrium constants that are required. Submit Answer Retry Entire Group 8 more group attempts remaining
Acetic Acid = 0.1033 M Ka = 1.8 x 10-5 Sodium hydroxide = 0.1104 M The first picture are the data, if needed second picture are the ones needs to be solved
1.00g of acetylsalicylic acid is mixed with 120 mL of water. Then, 25.00 mL of the solution is transferred to 3 flasks each. Assuming the pH is 3.00, calculate the initial concentration of , the Ka and pKa.
Use the References to access important values if needed for this question. An aqueous solution contains 0.367 M hypochlorous acid. How many mL of 0.224 M potassium hydroxide would have to be added to 125 mL of this solution in order to prepare a buffer with a pH of 7.300? Submit Answer Retry Entire Group mL 8 more group attempts remaining Pravious Email Instructor Next> Save and Exit
How much of each solution is needed to prepare 1 L of buffer solution with a pH value of 9.45 using 0.3 M Na2CO3 and 0.2 M HCl. You need to take, calculate (Ka1 = 4.3 × 10-7, Ka2 = 4.69x10-11).
Give typed explanation not a single word hand written otherwise leave it
All one question plz anwser neatly? thanks ?