During 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? a. Try the titration with another base. Maybe this one doesn't react with your acid. b. Put everything into the waste container and start over. c. Redo your calculation to make sure you are expecting the correct amount of base. d. Add a few drops of indicator to your flask. Perhaps you forgot to add them.

During 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? a. Try the titration with another base. Maybe this one doesn't react with your acid. b. Put everything into the waste container and start over. c. Redo your calculation to make sure you are expecting the correct amount of base. d. Add a few drops of indicator to your flask. Perhaps you forgot to add them.

Living By Chemistry: First Edition Textbook

1st Edition

ISBN:9781559539418

Author:Angelica Stacy

Publisher:Angelica Stacy

ChapterU4: Toxins: Stoichiometry, Solution Chemistry, And Acids And Bases

Section: Chapter Questions

Problem SIV3RE

See similar textbooks

Similar questions

Determine the volume of 0.205 MM KOHKOH solution required to neutralize each sample of sulfuric acid. The neutralization reaction is:H2SO4(aq)+2KOH(aq)→H2SO4(aq)+2KOH(aq)→ K2SO4(aq)+2H2O(l) Sample A: 30 mLmL of 0.205 MM H2SO4 Sample B: 200 mLmL of 0.140 MM H2SO4 Sample C: 65 mLmL of 0.110 MM H2SO4
In titration, what solution is placed inside the Erlenmeyer flask? Group of answer choices diluted solution titrant analyte stock solution
Which is NOT TRUE about titration?A. Slow addition of one solution of unknown concentration to a known volume of anothernsolution of known concentration.B. Reactions will end up to neutralization.C. A technique which is carried out to obtain the unknown concentrations.D. It is often indicated by a change in color.
This series demonstrates a drop-by-drop addition of 0.5 M barium chloride solution (???? ) to 0.5 M sodium carbonate solution (?? ?? 1. 1. What observations indicate that a chemical reaction has occurred? 2. Break up the reactants into ions. Switch the cations. Use the “criss-cross” method to get the balanced formulas for the products. Write the balanced molecular equation for this reaction, including phase labels. 3. Write the complete ionic equation for this reaction. 4. Write the net ionic equation for this reaction. 5. What is the precipitate?
What are "reference solutions" for in an experiment/lab?
Report your results in the table below. How do you know when a solution is saturated? When a solution is saturated and additional solid solute is added, what happens? Why do you think this is? How does adding this additional solute change the concentration of this saturated solution? How does evaporation change the concentration of a saturated solution?
A student did not read the directions to the experiment properly and mixed up where to place the NaOH solution and the vinegar. He put the vinegar in the titrator and the measured amount of NaOH in the beaker. He then added a drop of the phenolphthalein to the solution in the beaker. Does the student need to empty out all of the solutions and start over again or can he go ahead and run the titration? If he runs the titration using the solutions as given above, what should he expect to see happen for results?
Why is having a wash bottle useful for titrations?
given a diluted acid solution that was tested by another student. They were supposed to make a solution with a certain concentration. If your experimental data matched the test but not the target concentration, what does that tell you about the data? For example, the student was supposed to make a 0.87 M solution. When they tested it, they got 0.6113 M. When we tested it,we got 0.6144 M.
explain why the volume of water did not need to be exactly measure or recorded in Titration?
A chemist needs to determine the concentration of a sulfuric acid solution by titration with a standard sodium hydroxide solution. He has a 0.1834 M0.1834 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 13.96 mL13.96 mL of the standard solution. What is the concentration of the original sulfuric acid solution?
Initial Volume of Vinegar: 0.01 mL Final Volume of Vinegar: 15.18mL Initial Volume of NaOH: 0.21 mL Final Volume of NaOH: 24.30mL Molarity of NaOH: 0.50M Using this data, for this trial what was the molarity of acetic acid in vinegar?

SEE MORE QUESTIONS

Recommended textbooks for you

Living By Chemistry: First Edition Textbook

Chemistry

ISBN:

9781559539418

Author:

Angelica Stacy

Publisher:

MAC HIGHER

Living By Chemistry: First Edition Textbook

Chemistry

ISBN:

9781559539418

Author:

Angelica Stacy

Publisher:

MAC HIGHER

SEE MORE TEXTBOOKS

GET THE APP

About FAQ Academic Integrity Sitemap Document Sitemap

Contact Bartleby Contact Research (Essays)High School Textbooks Literature Guides Concept Explainers by Subject Essay Help Mobile App

GET THE APP

Privacy

Your CA Privacy Rights

Your NV Privacy Rights

About Ads

Manage My Data

bartleby, a Learneo, Inc. business

a.	Try the titration with another base. Maybe this one doesn't react with your acid.
b.	Put everything into the waste container and start over.
c.	Redo your calculation to make sure you are expecting the correct amount of base.
d.	Add a few drops of indicator to your flask. Perhaps you forgot to add them.