QUESTION 9 Acid-Base Titration In this experiment, an indicator called phenolphthalein is used to signal the endpoint of the titration (when the acid has been fully neutralized by the base). The indicator is colorless in acidic solution and pink in basic solution. During the titration, the pink color will appear and then disappear quickly with each addition of base (titrant). If a student is having trouble seeing the pink color in the sample flask, what can be done to help them see the color more clearly? Experiment - Acid-Base Titration.pdf O Remove safety goggles to get them out of the way. O Add several more drops of indicator - the more the better! O Place a piece of white paper or a white paper towel beneath the sample flask. O Place something dark beneath the sample flask.

QUESTION 9 Acid-Base Titration In this experiment, an indicator called phenolphthalein is used to signal the endpoint of the titration (when the acid has been fully neutralized by the base). The indicator is colorless in acidic solution and pink in basic solution. During the titration, the pink color will appear and then disappear quickly with each addition of base (titrant). If a student is having trouble seeing the pink color in the sample flask, what can be done to help them see the color more clearly? Experiment - Acid-Base Titration.pdf O Remove safety goggles to get them out of the way. O Add several more drops of indicator - the more the better! O Place a piece of white paper or a white paper towel beneath the sample flask. O Place something dark beneath the sample flask.

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

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
||| ctrl lacc shift ↑ tab caps lock VILION Mc ALE Graw HI esc K →1 Pavilion x360 fn O CHEMICAL REACTIONS Determining the molar mass of an acid by titration McCA X Eplanation g mol V An analytical chemist weighs out 0.188 g of an unknown triprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. She then titrates this solution with 0.1500M NaOH solution. When the titration reaches the equivalence point, the chemist finds she has added 38.4 mL of NaOH solution. Calculate the molar mass of the unknown acid. Be sure your answer has the correct number of significant digits. f1 Type here to search A https://www-awu.aleks.com/alekscgi/x/Isl.exe/1o_u-IgNslkr7j8P3jH-IvUrTNdLZh5A8CnG03PBGuXr8iCPa7ZMmym f2 @ Z Check 2 L M W hp S ALE MCCA ALER f3 # Mc Graw 3 X alt D 4 $ 4 с x10 X R O f5 Me Graw MI % F 5 at 40 MCCA ALE ALE ● V T S f6 4- G 6 ■ T f7 B Y ♫+ & Mc 7 H raw fg MCCA ALER *. N KAA © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center |…
A 50.0-ml sample of 0.20 M hydrochloric acid (HCI) is titrated with 0.5 M LIOH. Determine the pH of the solution after the following volumes of LIOH titrant are added. Express your answers to two decimal places. a) pH after 10 mL of LIOH added: b) pH after 20 mL of LIOH added: c) pH after 30 mL of LIOH added: Check
Help me answer this one question:
Determine the Ka value Solution 1 3.98 X 10-3 M Solution 2 6.03 X 10-4 M Solution 3 1.07 X 10-5 M Solution 4 1.05 X 10-5 M Solution 5 4.68 X 10-10 M
You are asked to make the 4.5 pH buffer from question the previous question. a. From the list of Acids and conjugate bases attached which pair would you pick. b. You are asked to make a 2M stock solution of the Buffer, how many grams of each acid and base would you need to make a 1000mL stock. c. For the experiment, the final concentration of the buffer should be 50mM. How many mL of your stock would you need to make 2L. Hint: M1V1=M2V2
the solution has to be acidified before testing for Ag+ ions. To make sure that the solution is acidic, what should be done? Apply a drop of the solution to red litmus paper to see if it turns blue. Apply a drop of the solution to blue litmus paper to see if it turns red. Apply a drop of the solution to pH paper to see if the pH is above 7. Apply a drop of the solution to your tongue to see if it tastes sour.
A solution of weak base is titrated to the equivalence point with a strong acid. a Which one of the following statements is most likely to be correct? The pH of the solution is greater than 13.0. The pH of the solution at the equivalence point is 7.0. The pH of the solution is between 2.0 and 7.0. The pH of the solution is between 7.0 and 13.0. The pH of the solution is less than 2.0. D The reason that best supports the answer above is OBecause the solution contains a weak base and the acid (titrant) is used up at the equivalence point, the solution will be basic. Whenever a solution is titrated with a strong acid, the solution will be very acidic. Because the solution contains the conjugate acid of the weak base at the equivalence point, the solution will be acidie
Calculate the pH for each case in the titration of 50.0 mL of 0.140 M HCIO(aq) with 0.140 M KOH(aq). Use the ionization constant for HC1O. What is the pH before addition of any KOH? pH = What is the pH after addition of 25.0 mL KOH? pH = What is the pH after addition of 30.0 mL KOH? pH