During the course of a titration experiment, you notice that no matter how much base you add to the sample of acid, the color of the solution does not change. In fact, you have added three times the amount of base you expected to add! What is the next thing you should do to troubleshoot this problem? Select the single best answer. O Redo your calculation to make sure you are expecting the correct amount of base. O Add a few drops of indicator to your flask. Perhaps you forgot to add them. O Try the titration with another base. Maybe this one doesn't react with your acid. O Put everything into the waste container and start over. X S

During the course of a titration experiment, you notice that no matter how much base you add to the sample of acid, the color of the solution does not change. In fact, you have added three times the amount of base you expected to add! What is the next thing you should do to troubleshoot this problem? Select the single best answer. O Redo your calculation to make sure you are expecting the correct amount of base. O Add a few drops of indicator to your flask. Perhaps you forgot to add them. O Try the titration with another base. Maybe this one doesn't react with your acid. O Put everything into the waste container and start over. X S

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

it is time for the titration. You measure 15.0 mL of the H2C2O4 solution with a 100-mL graduated cylinder and add it to a 125-mL Erlenmeyer flask. Then you add two drops of the indicator, phenolphthalein, to the oxalic acid solution in the flask. You dispense the NaOH solution from the buret into the flask (while swirling the flask) until you reach the endpoint. At the endpoint, the solution in the flask turns light pink. You repeat the titration two additional times for a total of three trials. H2C2O4 (aq) + 2 NaOH (aq) --> Na2C2O4 (aq) + 2 H2O (l) (I) (II) (III) Volume of H2C2O4 used 15.00 mL 15.00 mL 15.00 mL Initial Buret Reading 0.00 mL 0.05 mL 0.10 mL Final Buret Reading 14.45 mL 14.38 mL 15.40 mL Volume NaOH used ________mL ________mL ______mL Moles NaOH _______M ________M _________M…
Determining the volume of base needed to titrate a given mas... A chemistry student weighs out 0.348 g of ascorbic acid (H,C,H,0), a diprotic acid, into a 250. mL volumetric flask and dilutes to the mark with distilled water. He plans to titrate the acid with 0.1800M NaOH solution. Calculate the volume of NaOH solution the student will need to add to reach the final equivalence point. Round your answer to 3 significant digits. mL dla Explanation Check O 2021 McGraw-Hill Education. All Rights Reserved Terms of Use Privacy Accessibility MacBook Air
CHEMISTRY (Please write the complete solution legibly. No long explanation needed. Answer in 2 decimal places. Box the final answer.) 25.00 mL of a solution of phosphoric acid, H3PO4, was titrated with 0.500 M NaOH. a) Write the balanced chemical equation for this reaction.b) If 35.92 mL of NaOH solution were needed to reach the end point in the titration, what is the molarity of the H3PO4 solution?c) How many grams of H3PO4 were present?
An analytical chemist weighs out 0.280g of an unknown diprotic acid into a 250mL volumetric flask and dilutes to the mark with distilled water. She then titrates this solution with 0.1400M NaOH solution. When the titration reaches the equivalence point, the chemist finds she has added 26.7mL of NaOH solution. Calculate the molar mass of the unknown acid. Round your answer to 3 significant digits.
The solubility product constant for a certain metal phosphate, M3(PO4)2 is Ksp = 2.1 × 10−27. Its molar mass is ℳ = 279.04 g/mol. What is its solubility in g/L? Report your answer to TWO significant figures. Enter your answer in scientific notation using the appropriate boxes. Remember, a number like 1.6, in scientific notation is 1.6 × 100.
Titration of a 11.0 mLmL solution of HClHCl requires 32.4 mLmL of 0.11 MM NaOHNaOH. What is the molarity of the HClHCl solution? Express your answer using two significant figures.
I have 28.63 mL of an unknown-concentration Mg(OH)2 (aq) solution. I find that, when I add 23.33 mL of 0.1060 molar HCl(aq) to this solution, the acid and base exactly neutralize each other. What was the original concentration of the Mg(OH)2 solution? a. 3.151 molar O b. 0.1728 molar c. 0.04319 molar d. 0.06504 molar e. 0.08638 molar Clear my choice Previous page Z 3 $ 4 n 5 80 MacBook Pro 6 & 11 8 Next page
Calculate the molar mass of the unknown acid. Be sure your answer has the correct number of significant digits.
Consider the titration of 25.00 mL of Sprite with 0.050 M NaOH. Using the following data, determine the citric acid concentration in Sprite (g/L). Take the molar mass of citric acid to be 192.124 g/mol. Give your answer to one decimal place. initial volume (mL) final volume (mL) Buret reading (mL) 1.75 14.32
A chemist needs to determine the concentration of a sulfuric acid solution by titration with a standard sodium hydroxide solution. He has a 0.1886 M0.1886 M standard sodium hydroxide solution. He takes a 25.00 mL25.00 mL sample of the original acid solution and dilutes it to 250.0 mL.250.0 mL. Then, he takes a 10.00 mL10.00 mL sample of the dilute acid solution and titrates it with the standard solution. The endpoint was reached after the addition of 12.42 mL12.42 mL of the standard solution. What is the concentration of the original sulfuric acid solution?
Paolo added 6.5 mL of 3.5 M NaOH to 3.6 mL of 0.62 M HCI. Calculate the concentration, in units of M, of excess OH in the resulting solution. Note: Do not use scientific notation or units in your response. Sig figs will not be graded in this question, enter the unrounded value to four decimal places. Carmen may add or remove zeros from your response, your submission will still be graded correctly if this happens.
An analytical chemist weighs out 0.185 g of an unknown monoprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. She then titrates this solution with 0.2000 M NAOH solution. When the titration reaches the equivalence point, the chemist finds she has added 9.5 mL of NaOH solution. Calculate the molar mass of the unknown acid. Be sure your answer has the correct number of significant digits. g x10 mol