1. What is the effect on the computed molarity of KMNO4 if you stop titrating when the titrate solution turns dark pink? 1. A student was inquiring about the molarity of his KMN04 solution. As an analyte, ten milliliters of 0.1 M oxalic acid were used. The 50-mL burette reading towards the endpoint revealed a remaining capacity of 48.6 mL. What is the molarity of KMNO4? Note that the entire ionic equation for the interaction of KMNO4 with oxalic acid is depicted.

1. What is the effect on the computed molarity of KMNO4 if you stop titrating when the titrate solution turns dark pink? 1. A student was inquiring about the molarity of his KMN04 solution. As an analyte, ten milliliters of 0.1 M oxalic acid were used. The 50-mL burette reading towards the endpoint revealed a remaining capacity of 48.6 mL. What is the molarity of KMNO4? Note that the entire ionic equation for the interaction of KMNO4 with oxalic acid is depicted.

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

You measure 0.210 gram of unknown diprotic acid into a beaker. You add distilled water and a chemical indicator. You slowly add titrant 0.100M NaOH acid solution. Your first equivalence point is reached after 15mL NaOH has been added. The second equivalence point is reached after 30.0mL. WHat is the molar mass of the unkown diprotic acid?
A 25.0 mL sample of 0.150 M NH3 is titrated with 0.180 M HCI. Kb of NH3 = 1.76 x 10-5 Show your calculations. a) Write the neutralization reaction. b) What volume of 0.180 M HCI is required to reach the equivalence point? c) What is the pH at the equivalence point? d) Explain why the pH is not equal to 7 at the equivalence point. e) What is pH at the midpoint? f) What is the pH after 30.0 mL of 0.180 M HCI has been added. g) Draw a reasonable titration curve label the equivalence point and the midpoint. A
You are titrating 30 mL of 0.100M H3PO4 with 0.200 M KOH. For H3PO4: Ka1=1.1X 10-², Ka2 = 7.5 X 10-8, and Ka3 = 4.8 X 10-¹3. What is the pH after you add 35.00 mL of KOH?
Consider the titration of a weak monoprotic acid with a strong base. The titration starts with 80mL of a weak acid solution with a concentration of 0.160 M. The Ka of the weak acid is 2.9*10^-8. The solution of the weak acid is titrated by adding a 0.290 M NaOH solution. (NaOH is a strong base) A. What is the pH of the solution after 15mL of the base is added?
The following graph shows the pH curve for the titration of 25 mL of a 0.1 M monoprotic acid solution with a 0.1 M solution of a monoprotic base. 14 pH 12 10 8 6 4 2 0 0 5 10 15 20 25 30 35 40 45 50 mL of 0.1 M base added (1) The pH curve represents the titration of a (2) Choose a suitable indicator for the endpoint of the titration from the following pulldown list. 0 Malachite green Thymol blue Methyl orange Bromocresol green Methyl red Bromothymol blue Cresol red Phenolphthalein Thymolphthalein Alizarin yellow 0.2 1.8 pH 0 1 1.2 2 2.8 3 3.2 4.4 3.8 5.4 4 4.8 6.0 5 6.0 6 25 7.0 71 7 8.0 9.6 7.6 8.2 8 8.8 10.0 94 10.6 10.1 9 10 11 acid with a 12.0 12 13 14 base.
Questions 15-20 refer to the same weak base/strong acid (WB/SA) titration. The K of pyridine is 1.7 x 10-⁹. A 40.00 mL solution of 0.700 M pyridine (C5H5N) is being titrated with 1.05 M hydrochloric acid (HCI). What is the solution pH before the titration begins? (Two decimal places) Type your answer...
How is activity related to the 1/2 equivalence point in a titration? activity=activity coefficient x Molarity
For humans to maintain the pH of their blood close to 7.4, the body uses three buffer systems: carbonate, phosphate and proteins. If the pH of the blood goes below 6.8 or above 7.8, death may result. Imagine you want to make a phosphate buffer in the lab that resembles the bloods phosphate buffer. You start by mixing 0.95 M NaH2PO4 and 0.68 M Na2HPO4. H2PO4- + H2O ⇌ HPO42- + H+ pKa= 7.21 (5 marks total) a. From the reaction above indicate the weak acid and the conjugate base involved in making this buffer. (2 marks) b. Calculate the pH of the phosphate buffer solution. Provide your answer with 2 decimal places (2 marks) c. If the pH calculated in b. was the blood pH of an actual patient, would you say this patient’s blood pH is in the normal range or are they suffering from alkalosis or acidosis? (1 mark)
Two 25.0-mL. samples of unknown monoprotic weak acids, A and B, are titrated with 0.100 M NAOH solutions. The titration curve for each acid is shown below ACID A ACID B 14 14 12 12 10 10 10 15 20 25 30 35 40 45 30 5 10 15 20 25 30 33 40 45 30 Vohume of NaOH added (ml) Volume of NaOH added (ml ) Part A Which of the two weak acid solutions is less concentrated? B A. Submit Bequest Answer
Answer Questions #27 through #31 about the titration curves below (labeled a and b) for two different bases. The titrant acid used in both cases was 0.100 M HCl and the volume of the base solutions in both cases was 75.0 mL mL. 14 14 12 12 - 10- 10 8- 6. 4. 2- 2- 20 40 60 80 100 20 40 60 80 100 Volume of acid added (mL) (a) (b) Volume of acid added (mL) 2014 Pearson Education Inc P Type here to search 11:17 AM (? 3/18/2021 -> ort sc 80 6. ece num ER/TY || на 0 04 2C Hd
3
The half‑equivalence point of a titration occurs half way to the equivalence point, where half of the analyte has reacted to form its conjugate, and the other half still remains unreacted. If 0.500 moles of a monoprotic weak acid (?a=8.9×10−5) is titrated with NaOH, what is the pH of the solution at the half‑equivalence point? pH= ( Please type answer note write by hend )