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...

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4. A student did not read the directions to the experiment properly and mixed up where to put the NaOH and the HCl solutions. He put the HCl in the buret and the NaOH in the flask. He then added a drop of the phenolphthalein to the solution in the flask. Does the student need to empty out all of the solutions and start over again or can he go ahead and run the titration? Explain qalb ribidw qid edini olddud ris ogrel s znisimos tund entd nousu 5. How many liters of 3.4 M HI will be required to reach the equivalence point with 2.1 L of 2.0 M KOH? 9no vino to beateni nolusius to alsid sigulum ob of insttoqmi ti al VW S
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.
A lab technician finds an old bottle of NaOH stock solution but the concentration label is smudged. They take 12.5 mL of the unknown solution and dilute it to make a new solution of 50.0 mL. Through a titration experiment they find the concentration of the new solution to be 23.1 M. What was the concentration of the original KOH stock solution? Enter your answer with three significant figures.
O Microsoft O shift V A chemistry student weighs out 0.0608 g of formic acid (HCHO₂) into a 250. mL volumetric flask and dilutes to the mark with distilled water. He plans to titrate the acid with 0.1400M NaOH solution. OCHEMICAL REACTIONS Determining the volume of base needed to titrate a given mass... Calculate the volume of NaOH solution the student will need to add to reach the equivalence point. Be sure your answer has the correct number of significant digits. W Microsoft Microsoft 6.52.210... tab esc caps lock mL control Explanation ! 1 (8) Q A Check N © 2 W S #3 X T option command E x10 X D NOV 14 $ 4 C R S F do L % 5 V T G tv ♫ 6 MacBook Pro 9 Y & 7 H Ⓒ2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility U 8 1 9 BN M A O J K O O JOD 05 L H W P > { I command option DOCX + 11 ? | 1 9 OC
SIMPLE REACTIONS Shamma V Determining the volume of base neede... A chem student weighs out 0.0999 g of acetic acid (HCH,CO,) into a 250. mL volumetric flask and dilutes to the mark with distilled water. He plans to titrate the acid with 0.1100 M NAOH solution. Calculate the volume of NaOH solution the student will need to add to reach the equivalence point. Round your answer to 3 significant digits. ||mL O ml. x10 dlo 18 Ar Explanation Check O 2021 Mcolaw- LUutatioI. All RightS RESEIVEU. Privacy Accessibility
A student titrating a sample of a powdered aspirin tablet to find out how much acetylsalicylic acid is in the sample finds that it requires 30.4 mL of a 0.0902M sodium hydroxide solution to neutralize the acid in the sample. How many milligrams of acetylsalicylic acid did the sample contain? Use the correct number of significant figures. Do not include units or your answer will be counted wrong.
Calculate the molarity of an NaOH solution from the following titration data. Be sure the answer has the correct amount of significant figures. The chemical equation for this titration is as follows: NaOH + KHP → NaKP + H₂O NaOH buret reading, inital: 15.27 mL NaOH buret reading, final: 8.32 mL Mass of KHP (204.22 g/mol): 1.1592 g
A sample with a mass of 1.340 g was dissolved in water, releasing chlorine ions. The aqueous solution was treated with access AgNO3(aq), the AgCl precipitate collected and weighted. Its mass was 2.709 g. What percentage by mass was the original sample? Make sure to use the correct number of significant figures in your answer.
An analytical chemist weighs out 0.159 g of an unknown monoprotic acid into a 250 mL volumetric flask and dilutes to the mark titrates this solution with 0.0700 M NaOH solution. When the titration reaches the equivalence point, the chemist finds she has added 25.2 mL of NaOH solution. Calculate the molar mass of the unknown acid. Round your answer to 3 significant digits. mol
A chemist needs to determine the concentration of a sulfuric acid solution by titration with a standard sodium hydroxide solution. He has a 0.1166 M standard sodium hydroxide solution. He takes a 25.00mL sample of the original acid solution and diluted it to a 250.0mL. Then, he takes a 10.00mL sample of the dilute acid solution and titrates it with the standard solution. The endpoint was reached after the addition of 12.52mL of the standard solution. What is the concentration of the original sulfuric acid solution? concentration:_____M
A quantity of 19.68 mL of a KOH solution is needed to neutralize 0.3528 g of the monoprotic, weak acid KHP. What is the concentration (in molarity) of the KOH solution? (The molar mass of KHP is 204.21). Round your answer mol 4 significant digits.
A chemist needs to determine the concentration of a sulfuric acid solution by titration with a standard sodium hydroxide solution. He has a 0.1840 M standard sodium hydroxide solution. He takes a 25.00 mL sample of the original acid solution and dilutes it to 250.0 mL. Then, he takes a 10.00 mL sample of the dilute acid solution and titrates it with the standard solution. The endpoint was reached after the addition of 13.34 mL of the standard solution. What is the concentration of the original sulfuric acid solution? concentration: M