* The use of indicators must follow the properties listed below. Chose the correct property.3 Indicators must be used according to pH at end point Indicators must be used according to the chemical reaction Indicators must be used according to the products of reaction Indicators must be used according to the type of titration reaction

* The use of indicators must follow the properties listed below. Chose the correct property.3 Indicators must be used according to pH at end point Indicators must be used according to the chemical reaction Indicators must be used according to the products of reaction Indicators must be used according to the type of titration reaction

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...

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Please answer the 3 boxes for ph
Consider the reaction of a 20.0 mL of 0.220 M CSH&NHCI (Ka = 5.9 x 10-6) with 12.0 mL of 0.241 M CSOH.
1. A substance that shows the endpoint of titration 2. Type of error in which the volume delivered differ slightly from those indicated by their graduations 3. Procedure to eliminate personal error.
What are the properties of a buffer solution? Explain clearly and write it on text. (Not handwritten)
When titrating a strong acid with a strong base, the equivalence point is reached when: Select one: a. The pH indicator changes color. b. The amount of base added is exactly enough to react away all of the acid. c. The pH is determined solely by the amount of acid originally present. d. The pH is determined solely by excess base after all the acid has been neutralized.
The experimental procedure above was used to generate the data in the tables below. Data Collection Table Titration Mass of Sample Initial Buret Reading (mL) Final Buret Reading (mL) 1 1.234 1.05 19.95 2 1.213 4.00 23.50 3 1.273 0.30 20.05 4 1.292 5.95 25.65 - For each titration, calculate: - The number of moles of potassium permanganate used in the titration (H x L of KMnO4) - The number of moles of iron present in the sample (stoichiometry in balanced equation) - The percentage by mass of iron in the solid sample (Equation 1) - The average mass % of iron in your unknown - The standard deviation in your % Fe results:
II. Titrating HCI Solution with NaOH Solution 1. Prepare a titration curve. Plot pH (on the y-axis) versus volume of NaOH solution added (on the x-axis). If your initial buret reading was not 0.00 mL, remember to subtract your actual initial reading from each of your subsequent buret readings before plotting the titration data.
Describe the information necessary (and why) to choose a good indicator for a weak acid/strong base titration. Answer:
Solution : Acetic Buffer NaCl Original pH : 4.2 7.2 pH after adding 5 drops of HCl : 4.2 2.7 pH after adding 5 drops of NaOH : 4.2 11.1 Which sample showed little or no change in pH upon the addition of acid and base? Please write an equation and explain briefly.
Question Completion Status: For Solution A, approximately how many mL of HCI were needed to exceed the buffering capacity of this solution? Enter the number only. Don't enter units as part of your answer and don't use commas or scientific notation. Titration curve of Solution A 14 13 12 11- 10 9 8 pH 7 6 5 4 3 2 1 5 4 3 2 1 HCI added (mL) 0 1 2 3 4 5 NaOH added (mL) 14 13 12- 11 10 9 8 pH 7 6.8 2 65 4 3 2 1 Titration curve of Solution B Click Save and Submit to save and submit. Click Save All Answers to save all answers. 54 32 1 HCI added (mL) 0123 NaOH added (mL)
A standard solution is a solution of accurately known concentration. What is a standard solution for titrating sulfuric acid in acid-alkali titration? a) Alkali such as sodium hydroxide b) Any alkali and acids c) Salt such as sodium chloride d) Acid such as hydrochloric acid
Which of the following is true In an acid-base titration A. Water is never formed B. You are trying to make a precipitate C. Moles acid = moles base at the point of neutralization D. The pH will always be = to 7.0 at the neutralization point