In this experiment you were given the concentration of NaOH(aq). That concentration wasdetermined in part A. by using a solid acid, potassium hydrogen phthalate. Suppose that in part A.6.during the standardization of the sodium hydroxide solution a drop of the NaOH titrant adheres onthe side of the buret (because of a dirty buret) between the initial and final readings for the titration,and therefore does not make it down to the flask containing the acid potassium hydrogen phthalate.This technique error will result in the reported concentration of NaOH(aq) to beO too lowO too highO unaffected

Standardization is the process of determining the exact concentration (molarity ) of a solution .…

In this experiment you were given the concentration of NaOH(aq). That concentration was determined in part A. by using a solid acid, potassium hydrogen phthalate. Suppose that in part during the standardization of the sodium hydroxide solution a drop of the NAOH titrant adheres the side of the buret (because of a dirty buret) between the initial and final readings for the titrat and therefore does not make it down to the flask containing the acid potassium hydrogen phthal This technique error will result in the reported concentration of NaOH(aq) to be. O too low O too high O unaffected

In this experiment you were given the concentration of NaOH(aq). That concentration was determined in part A. by using a solid acid, potassium hydrogen phthalate. Suppose that in part during the standardization of the sodium hydroxide solution a drop of the NAOH titrant adheres the side of the buret (because of a dirty buret) between the initial and final readings for the titrat and therefore does not make it down to the flask containing the acid potassium hydrogen phthal This technique error will result in the reported concentration of NaOH(aq) to be. O too low O too high O unaffected

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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A 27.56 mL portion of a 0.337 M solution of hydrochloric acid, a monoprotic acid, is to be titrated with a standarized 0.411 M solution of KOH. What is the expected volume in milliliters of the KOH solution needed to reach the phenolphthalein end point? Report your answer with a precision of two decimal places.
A chemistry student needs to standardize a fresh solution of sodium hydroxide. She carefully weighs out 316.mg of oxalic acid H2C2O4 , a diprotic acid that can be purchased inexpensively in high purity, and dissolves it in 250.mL of distilled water. The student then titrates the oxalic acid solution with her sodium hydroxide solution. When the titration reaches the equivalence point, the student finds she has used 93.2mL of sodium hydroxide solution. Calculate the molarity of the student's sodium hydroxide solution. Be sure your answer has the correct number of significant digits.
An analytical chemist weighs out 0.087 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 0.1100 M NaOH solution. When the titration reaches the equivalence point, the chemist finds she has added 11.0 mL of NaOH solution. Calculate the molar mass of the unknown acid. Be sure your answer has the correct number of significant digits. g mol Explanation JAYE A @@ W Recheck > # 3 E 80 F3 $ 4 X 8.88 F4 R S C % 5 F5 T 6 MacBook Air Y & 7 4 F7 U * © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility 8 DII ( 9 DD O O F10 P ?圖 □ 留 m F11 olo Ar (9)
A solution of sodium hydroxide is standardized against potassium hydrogen phthalate (molecular mass = 204.224 g mol-1). From the following data, calculate the molarity of the NaOH solution. The mass of the KHP is 0.7840 g. Before the titration the buret reading was 0.8400 mL and afterwards it was 39.20 mL. A 85.12 mL sample of a solution of sulfuric acid, H2SO4, is neutralized by 59.82 mL of the NaOH solution from the problem above. Calculate the molarity of the sulfuric acid solution.
You are running an acid-base titration with hydrochloric acid and calcium hydroxide. The calcium hydroxide is your titrant; it has a known concentration of 0.0891 M. You have added 25.0 mL of the hydrochloric acid solution to an Erlenmeyer flask along with 2 drops of phenolphthalein (fee’-nol-thay-leen) indicator. To begin your first trial, you fill a clean 50 mL buret with the calcium hydroxide solution. Your starting volume is 0.25 mL. After the addition of solution from the buret, you see a color change in the flask, and the end point of the reaction is reached. You note the final volume in the buret to be 18.75 mL. You begin again for your second titration trial. You add 24.8 mL of the hydrochloric acid solution to a clean flask along with 2 drops of indicator. You refill the buret to an initial volume of 1.42 mL. When the reaction is complete, you note the final volume in the buret at 16.74 mL. Then you complete a third trial. You add 25.6 mL of hydrochloric acid solution…
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A titration of 25.00 mL of an unknown HCl solution with 0.1550 M NaOH starts at a buret reading of NaOH of 0.33 mL. The phenolphthalein indicator turns light pink in the acid solution over 30 seconds at a buret reading of 24.19 mL. Write the balanced equation for the neutralization reaction. What is the molarity of the HCl solution?
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A student measures that it takes 7.21mL of 0.326 M NaOH (aq) solution to reach the first equivalence point of a titration of 100.0 mL of phosphoric acid solution. He also notes that it takes a total of 14.40 mL of 0.326 M NaOH (aq) solution to reach the second equivalence point. What is the concentration of the phosphoric acid solution?
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A student weighs a sample of potassium hydrogen phthalate (KHP) to prepare a primary standard for a titration. She later discovers that the KHP was contaminated with sugar. To determine the amount of KHP in the mixture, she takes 4.678 g4.678 g of the mixture and make a 100.0 mL100.0 mL solution. The student then titrates 10.00 mL10.00 mL of this solution with a 0.1030 M0.1030 M sodium hydroxide solution. She finds that 15.15 mL15.15 mL of the NaOHNaOH solution is needed to reach the end point.
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