Using a pH meter, verify that 100 mL of distilled water is neutral. Dissolve 50.0 mg of naproxen drug substance, accurately weighed, in 50 mL of methanol. Add 25 mL of the neutralized water and mix. Add two drops of phenolphthalein as the indicator. What is the blank sample in this experiment? How many sample and blank titrations are required for this experiment? Use the equation below to calculate your expected end-point volume. Each mL of 0.01 N sodium hydroxide is equivalent to 2.303 mg of naproxen, C14H14O3

Using a pH meter, verify that 100 mL of distilled water is neutral. Dissolve 50.0 mg of naproxen drug substance, accurately weighed, in 50 mL of methanol. Add 25 mL of the neutralized water and mix. Add two drops of phenolphthalein as the indicator. What is the blank sample in this experiment? How many sample and blank titrations are required for this experiment? Use the equation below to calculate your expected end-point volume. Each mL of 0.01 N sodium hydroxide is equivalent to 2.303 mg of naproxen, C14H14O3

Chemistry: Matter and Change

1st Edition

ISBN:9780078746376

Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Chapter18: Acids And Bases

Section: Chapter Questions

Problem 2STP

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Students Mola and Rity were tasked to analyze the acidity of a 10.0-mL fermented milk sample diluted with water in a 250-mL volumetric flask. Mola obtained a 15.0-mL aliquot of this solution, diluted it to 50.0 mL, and then titrated this diluted sample. Titration data were given to Rity and she found out that the 50.0-mL diluted sample contains 0.21 mmol of lactic acid. MW: Lactic Acid (90.08) a. What is the lactic acid concentration (in M) of the titrated sample? b. Determine the lactic acid content (in M) of the 10.0-mL fermented milk sample. c. What is the lactic acid concentration (in %w/v) of the 10.0-mL fermented milk sample?
In Experiment 4, we used titration to determine the total acid content of samples, which we reported in terms of molarity. Reporting acidity through pH measurements is quite different, in that we can only measure the amount of the acid in its ionized form. You were tasked to investigate a clear aqueous solution of an unknown monoprotic acid. You decided to use two Chem 16.1 methods to gather data.Method 1 – TITRATION: A 10. mL aliquot of the sample was diluted with 25 mL distilled water. Two drops of phenolphthalein were added and then it was titrated 3.54 mL of 0.048 M standardized NaOH to the endpoint.Method 2 – pH STRIP: You took 1 mL of the sample and used a pH strip to estimate the pH, which turned out to be around 3.3. Another 1 mL of the sample was diluted with 9 mL of water. The pH was taken again and is now around 3.8 a) Calculate the molarity of the acid using the titration data.b) If we assume that the titrated unknown is a strong acid, predict the pH of the sample.c) Using…
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Acid-base Titration Assignment solves questions in end. if necessary use notebook to make the curve.A student conducted the following experiment in the lab. 50.00 mL of acetic acid (of unknown concentration) was pipetted into a 150 mL Erlenmeyer flask. An indicator was added and the pH of the solution was recorded. 0.1 M NaOH (a strong base) was added to the Erlenmeyer flask from a buret. The contents of the flask were continuously stirred and the pH was recorded every 2 mL using a pH meter.Data Collected: Volume of NaOH added (mL) pH 0.0 2.87 10.0 4.14 25.0 4.74 40.0 5.35 50.0 8.72 60.0 11.96 75.0 12.30 1. The chemicals involved in the titration are NaOH (a strong electrolyte) and CH3COOH (aweak electrolyte). Predict the shape of the titration curve that would be obtained from thedata above. Also predict what the pH at the equivalence point will be.2. What is the volume of NaOH at the equivalence point?3. What is the pH at the equivalence point?4. What does the…
please calculate the neutralization equivalent for each run for part II. and for part III, calculate the neutralization equivalent for malonic acid and maleic acid
This is a dilution lab of acetic acid. There is 1.0M acetic acid with ph of 2.297, 0.1M acetic acid with ph of 2.69897, and 0.01M acetic acid with ph of 3.69897. They were all filled up to 50ml in a volumetric flask. How do you build the ICE table for the different concentrations?I have attached some images for extra information if needed.
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Before running a titration, you calculate the expected endpoint. However, when performing the experiment, you pass the expected endpoint with no visible color change. What is the most likely problem with the titration set-up? Select one: There was an air bubble in the buret tip. The buret tip is leaking titrant into the analyte. There is not enough indicator in the analyte. The analyte solution is being stirred too quickly.
Draw/illustrate the chemical reaction involved in Seliwanoff’s test and explain the purpose of this qualitative test?
Which of these procedures would not make a pH =4.75buffer?(a) Mix 50.0 mL of 0.10 M acetic acid and 50.0 mL of 0.10 M sodium acetate.(b) Mix 50.0 mL of 0.20 M acetic acid and 50.0 mL of 0.10 M NaOH.(c) Start with 50.0 mL of 0.20 M acetic acid and add a solution of strong base until the pH equals 4.75.(d) Start with 50.0 mL of 0.20 M HCl and add a solution of strong base until the pH equals 4.75.(e) Start with 100.0 mL of 0.20 M sodium acetate and add 50.0 mL of 0.20 M HCl.
Titration 1 Titration 2 Titration 3 Volume of HCl solution (mL) 5.0 ml 5.0 ml 5.0 ml Initial buret reading (mL) 0.5 ml 0.5 ml 0.5 ml Final buret reading (mL) 45.61 ml 45.56 ml 45.64 ml Volume of NaOH used (mL)
Thank you! Data included in picture! No hand drawn graphs!! Determine the equivalence point of sudsy ammonia/citric acid reaction by graphing the titration data (pH vs volume citric acid) from Table 1: No Indicator Data Table. Draw a green arrow (use ‘Insert Shape’ feature to do this once you have copied your graph from Excel) on your graph indicating the data point that represents your equivalence point. Use a graphing software to create the x-y scatter plot showing the pH of the experimental solution as a function of the volume of citric acid (the titrant) added for the titration in Part 4. On your graph, the x-axis should be the volume of citric acid added (mL), and the y-axis should be the pH of the experimental solution at that volume. Do NOT connect your points; no trend line needed and make sure to: · Label the axes including the units in parentheses. · Include a figure legend (text below the graph) explaining the data in your graph that includes the arrow…