4.Suppose you run a titration of an acid yourself. You do it three times be- tween an acid and sodium hydroxide solution. Here is some data: Average volume of sodium hydroxide solution delivered: 9.10 mL Concentration of sodium hydroxide standard solution: 0.1010 M Average mass of acid solution: 9.555 g The average volume of sodium hydroxide solution is the average of three titra- tions. In other words, you did the experiment three times and took an average. The same goes for the average mass of the acid. You ran the experiment three times and the average mass of the acid solution is given for those three titra- tions. The sodium hydroxide solution was standardized and the concentration is given. Show your step-by-step calculations for this experiment to find the mass per- cent of acid in the solution. Show each step explicitly.

4.Suppose you run a titration of an acid yourself. You do it three times be- tween an acid and sodium hydroxide solution. Here is some data: Average volume of sodium hydroxide solution delivered: 9.10 mL Concentration of sodium hydroxide standard solution: 0.1010 M Average mass of acid solution: 9.555 g The average volume of sodium hydroxide solution is the average of three titra- tions. In other words, you did the experiment three times and took an average. The same goes for the average mass of the acid. You ran the experiment three times and the average mass of the acid solution is given for those three titra- tions. The sodium hydroxide solution was standardized and the concentration is given. Show your step-by-step calculations for this experiment to find the mass per- cent of acid in the solution. Show each step explicitly.

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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CHEMICAL REACTIONS Determining the volume of base needed to titrate a given mass... A chemistry student weighs out 0.0878 g of phosphoric acid (H₂PO4), a triprotic acid, into a 250. mL volumetric flask and dilutes to the mark with distilled water. He plans to titrate the acid with 0.1500 M 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. Explanation Check X MacBook Air 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center
The student is required to determine the concentration of a basic NaOH by using the primary standard KHP (molar mass = 204.22 g/mol). The student dissolved the 1.130 g of KHP in 50.00 mL of DI water before titrating it with NaOH. (make sure to write the chemical reaction) The following data were obtained from the student standardization. Trial 1 Mass ok KHP (g) 1.130 Initial volume of 1.90 NAOH (mL) Final volume of 16.88 NaOH (mL) What is the concentration of NaOH?
During the standardization of NaOH , a drop of titrant was present on the tip of the buret when making the final volume reading. Would this affect the final calculations of molarity of NaOH? If so, how? Explain.
Please don't provide handwritten solution ....
For their first trial, a student pipettes 5.00 mL of a vinegar solution into an Erlenmeyer flask. The student titrates the vinegar with standardized NaOH with a molarity of 0.437 M. The volume of titrant used was recorded in the table above. Calculate the molarity of the vinegar solution for this trial. Enter a number without units.
Will the calculated Molarity of NaOH be too high or too low or unaffected if the following happen: When you answer the question, consider how the situation affects the calculation of molarity of NaOH and moles NaOH, which is calculated from the mass of KHP. For each answer, you must supply a clear explanation for your answer. Often times, students will restate the facts rather than explaining why they chose the answer they chose. a) You add the weighed KHP to a flask containing a 60mL of water rather than 50 mL of water. Explain. Your answer must contain a well-thought-out and clearly written explanation. b) The buret is still wet with water on the inside when you add your NaOH solution. Explain c) The KHP is wet when you weigh it. Explain. d) You titrate past the equivalence point by 0.50mL Answer a-d
Note:- • Do not provide handwritten solution. Maintain accuracy and quality in your answer. Take care of plagiarism. • Answer completely. • You will get up vote for sure.
You have been given a vinegar solution that is made of water and an unknown concentration (M) of acetic acid. Acetic acid is a monoprotic acid which reacts with NaOH in a 1:1 mole ratio. You have access to a premade NaOH solution of unknown concentration (M), potassium hydrogen phthalate (KHP) and an phenolphthalein indicator as well. Using whatever necessary glassware that would be available to you in the general chemistry lab, design an experiment to determine the Molarity concentration (M), and appropriate statistics, of the acetic acid in the vinegar solution. Write the procedure, including specific glassware, measurements, and calculations in a bulleted or numbered list.
Solving for a reactant in solution.
A 1.22 g sample of KHP is used to titrate a NaOH solution. A student finds that it requires 15.00 mL of the NaOH solution to reach the end point. What is the molarity of the NaOH solution?
Calculate the molar mass of the unknown acid. Be sure your answer has the correct number of significant digits.
13. A chemistry student offers a possible improvement to this lab. Since one goal of this lab is to determine the mass of the precipitate produced, wouldn't it be possible to measure the mass of an empty beaker, mix the solutions, and boil off the water until it is entirely evaporated, leaving only solid behind? Then the beaker with the precipitate could be weighed, and the difference between this mass and that of the empty beaker would be the mass of the precipitate. This would eliminate the need for the filtration step. Explain why this is a poor suggestion. Remember to check your reasoning on this question and all other questions with your instructor.