Picture this: A burette used for the titration of p-methylbenzoic acid (p- MBA) was washed with distilled water only; the analyst filled the burette with a previously standardized NaOH without drying. The concentration of the actual concentration p-MBA calculated in this titration will be of p-MBA. higher than lower than O equal to O indeterminate to

Picture this: A burette used for the titration of p-methylbenzoic acid (p- MBA) was washed with distilled water only; the analyst filled the burette with a previously standardized NaOH without drying. The concentration of the actual concentration p-MBA calculated in this titration will be of p-MBA. higher than lower than O equal to O indeterminate to

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

50.0 mL of 0.31 M acrylic acid (C2H3COOH, Ka = 1.71 x 10 ) solution is titrated with 0.31 M NaOH to the equivalence point. The %3D reactants are completely transformed into sodium acrylate C2H3COONA at this point. What is the pH of the titration solution at equivalence point? Please keep your answer to two decimal places.
Based on the results obtained in the table, What is the color of acid-base indicator B when the pH of the medium is equal to its pKa?
use the titration curve below. 14 12 10 8 4 2 60 70 10 20 30 40 50 80 Volume of Titrant (mL) What is the possible identity of the titrant? a. Strong base b. Strong acid Which of the following stoichiometrically represents the titration curve? а. НА +3 X-Он — Х;А +3 Н,О b. НА +X-ОН — ХА+Н:0 с. Н.А +2X-Он — Х,А + 2 H,0 d. 2 H;A + 3 X(0H), → X;A2 + 6 H,0 Which of the following statement is NOT FALSE regarding the titration curve? a. There are three equivalence points located near pH 2.00, 6.00 and 12.00. b. There are three equivalence points that approximately requires 15.00, 40.00 and 60.00 mL of titrant. c. There are two equivalence points located near pH 6.00 and 12.00. d. There are two equivalence points that approximately requires 25.00 and 50.00 mL of titrant. c. Weak base d. Weak acid Hd
What is the pH at 90.00 mL of titrant in the titration of 50.00 mL of 0.400 M B (a generic base with Kp = (4.45x10^-10)) with 0.200 M HNO3? Enter your answer in scientific notation with 3 sig figs. Do not include any units in your answer. Do not round any intermediate calculations. Note: Your answer is assumed to be reduced to the highest power possible. Your Answer: x10 Answer
If a 300 mg sample of Sodium Bicarbonate (98% NaHCO3) is titrated with 0.922 N sulfuric acid, what volume of the acid should be required to produce an end point? Atomic Weights :Sodium - 22.99Oxygen - 15.999Hydrogen - 1.008Sulfur - 32.06 Enter numerical value only; round off to 4 decimal places
HA+KOH → NaA + H₂O Nia titrates half of a weak acid solution with KOH until she observes the endpoint. She measures the pH of the half-titrated weak acid solution as 1.23. What is the Ka for the acid? K₂ = [? ] × 10¹²] a Coefficient (green) Exponent (yellow) Enter
The pK, values for the dibasic base B are pKpi = 2.10 and pK2 = 7.62. %3D %3D Calculate the pH at each of the points in the titration of 50.0 mL of a 0.50 M B(aq) solution with 0.50M HCI(aq). What is the pH before addition of any HCI? pH = What is the pH after addition of 25.0 mL HC1? pH = What is the pH after addition of 50.0 mL HCI? pH What is the pH after addition of 75.0 mL HCI? pH = What is the pH after addition of 100,0 mL HCI? pH =
What is the pH of 3.00 L of a buffer made of (2.840x10^-1) M HBrO and (7.16x10^-1) M KBrO AFTER the addition of 250.00 mL of 0.800 M HNO3? Enter your answer in scientific notation with 3 sig figs. Do not include any units in your answer. Do not round any intermediate calculations. Note: Your answer is assumed to be reduced to the highest power possible. Your Answer: х10
Calculate the pH for each of the cases in the titration of 25.0 mL of 0.110 M pyridine, C₁H₁N(aq) with 0.110 M HBr(aq). The Kb of pyridine is 1.7 x 10-⁹. before addition of any HBr pH = after addition of 12.5 mL of HBr after addition of 16.0 mL of HBr after addition of 25.0 mL of HBr after addition of 35.0 mL of HBr 9.31 pH = pH = pH = pH = 5.23 4.63 Incorrect 11.65 Incorrect 1.33 Incorrect
Please answer; they were all the same choices.
What is the pH at 0.00 mL of titrant in the titration of 50.00 mL of 0.400 M B (a generic base with Kp = (4.28x10^-10)) with 0.200 M HNO3? Enter your answer in scientific notation with 3 sig figs. Do not include any units in your answer. Do not round any intermediate calculations. Note: Your answer is assumed to be reduced to the highest power possible. Your Answer: x10 Answer
QUESTION 30 Below is a titration curve of a sample of monoprotic acid (HA) by NaOH. Which is most likely the acid? 15 Hd 12 10 6 2 0 0 10 20 volume of strong base (mL) O H-CIO₂ (pKa = 1.96) OH-CN (pKa = 9.2) O H-C₂H302 (pKa = 4.7) O HCO2-H (pKa = 3.7) OH-NO3 30 40 50 60 70 Click Save and Submit to save and submit. Click Save All Answers to save all answers. f4 H a 7 f7 f8 $ www S