Apart from barium Sulfate preparation, Find any Preparation in the United States Pharmacopeia that involves precipitation titration. Identify the following Analyte, Titrant, Indicator, The percentage Requirement, the Assay procedure, Write the reaction involved in the assay. Provide a link to the USP (United States Pharmacopeia). Instruction "Please give a detailed explanation"
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- Apart from barium Sulfate preparation, Find any Preparation in the United States Pharmacopeia that involves precipitation titration. Identify the following Analyte, Titrant, Indicator, The percentage Requirement, the Assay procedure, Write the reaction involved in the assay. Provide a link to the USP (United States Pharmacopeia).
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- A student performed a titration to determine the exact concentration of NaOH(aq). The titration was performed against a standard 0.1000 M HCl(aq) solution. Phenolphthalein indicator was used. The following end-point volumes were recorded by the student in units mL: Trial Number Volume 1 25.06 2 25.15 3 25.02 4 25.17 5 25.07 Calculate the 95% confidence limit. Assume that there is no outlier. Provide your answer to the correct number of decimal places, without units, and without the ± sign. Use the T-table shown below.Write measurement of Carbon dioxide evolution during respiration of germinating seeds by the Titration methodIt is a solution of unknown concentration in which a solution of accurately known concentration is gradually added until the reaction is complete. Analyte Endpoint Indicator Titrant
- DATA AND CALCULATIONS Show all calculations neatly on an attached sheet. Trial 1 Trial 2 Trial 3 70.6849. 68.0749 2.61g 23.25ML O.65ML 22.6mL Mass of flask + vinegar Mass of empty flask Mass of vinegar used Final buret reading Initial buret reading Volume of NaOH used Moles of NaOH used 0.00226 mol Moles of açetic acid titrated Mass of acetic acid titrated Mass % acetic acid in vinegar 5.0%For the CO2 impact experiment station: 1) Obtain two plastic cups, red cabbage indicator, a straw, and plastic wrap. 2) Fill each cup approximately one-quarter to one-third full of tap water and add ~10 mL of the red cabbage indicator. 3) Place the two cups side by side on a sheet of white paper. 4) Place the straw into one of the beakers and cover that beaker with the plastic wrap. 5) Carefully blow bubbles into the test cup for 3 min. and observe both cups. 6) Compare the color to the control cup and record any differences. This the Question: Did the beaker with the solution into which CO2 was bubbled change pH/color? By how much? Is this what, you would predict, based on your knowledge of the chemistry of CO2?Part A - Reactions of Carbon Dioxide Gas Place a small lump of dry ice into a large test-tube. To the dry ice add about 5 mL of water. After the gas has bubbled through the water for a few minutes (so that it may be assumed the solution is saturated with the gas), test the acidity of the solution by adding 1 drop of universal indicator solution and check the pH on the colour chart provided. Record your observations onto your results page. 1. RESULTS (Remember to not include spectator ions in ionic equations.) Part A - Reactions of Carbon Dioxide Gas 2. Place two large test tubes in the test tube rack. In one tube place a small lump of dry ice and cover the mouth of the tube with a loose plug of cotton wool. Stand the test tube in a beaker of containing a little warm water (from the hot water tap) for a minute. The test tube will fill with carbon dioxide gas. In the meantime, obtain two small (100 or 150 mL) beakers, and place 20 mL of water in each and add 3 drops of universal…
- . Lets pretend for a moment that you’re now working as an analyst working for the policedepartment. You are asked to analyze a white powder confiscated from a suspect. The complainantclaimed that the powder was used by the suspect to slowly poison the victim. Suppose the suspectclaimed it is only sodium chloride, how would you analyze the material to confirm that is indeed NaCl.Outline the qualitative test that must be done and provide inference for each test.(NOTE: Make sure analysis is in logical order backed up with chemical reactions if possible because youwill present it during the court hearing)An honest MISTAKE in the analysis can be a reason why innocent person will suffer in jail or a trueblooded murderer will escape the case.In the analysis of H2O2 using KMnO4, the simulation first states that about 20 mL of water is added to the 1.00 mL aliquot of H2O2 to make the observation of the end point easier. Later, you are informed that your assistant diluted the 1.00 mL H2O2 sample to 10 mL with distilled water. Which of the following volumes is used in your analysis of the concentration of H2O2 in the original sample? Question 3 options: 10.00mL 20.00mL 11.00mL 21.00mL 1.00mLThe course is specifically quantitative analysis, I figured that would just fall under chemistry. The issue I'm having with this one is that I have absolutely no idea how to even begin. I figure benzoic acid wouldn't affect the pH of NaOH that much since it's a weak acid and NaOH is a strong base, but I don't think it'd be right to just take the pH using solely the concentration of NaOH. What approach should I take to solve this? 220 mL of 0.03 M NaOH were added to 200 mL of 0.03 M benzoic acid (pKa = 4.2). What is the pH of the resulting solution?
- Pharmac is a pharmaceutical company that manufactures various antacids used for symptomatic relief of heartburn. Yesterday, a batch of 250 mg calcium carbonate tablets (Brand Name: Calcarb) has been manufactured and is now up for quality control testing. Samples were transmitted to your laboratory for testing. As a laboratory analyst, you are tasked to perform the Acid Neutralizing Capacity Test. This test simulates the action of the antacid in the stomach and determines the number of milliequivalents of HCl that the antacid can neutralize. For Calcarb to pass the test, it must be able to neutralize NLT 5 mEq of HCl. Answer all subsequent questions. 1. In this test, the procedure requires that a 1 Normal Hydrochloric acid (HCl) be used. To perform the test, you need to prepare 500 mL of this acid. The available stock of HCl in the lab is concentrated HCl with a percentage concentration of 37.0% w/w. Calculate how many mL of this stock HCl must be used to prepare 500 mL of IN HCl. The…1. Predict the effect of each of the following conditions on the calculated concentration of NaOH. Explain briefly your answers. a) The burette to be used was not rinsed with the NaOH solution. b) The air space at the burette tip was not removed before titration. c) The flask used to weigh KHP contained traces of NaOH. d) The burette reading for NaOH was taken after rapid delivery of the titrant.2.1 Calculate the pH of 1.0 M HC2H3O2 solution, using Ka = 1.7 × 10-5 . Begin this calculation by defining the variable x. List the pH answer as “theoretical pH” on the report sheet. Have the instructor check this answer and all subsequent calculations. To test your prediction, obtain about 35 mL 1.0 M HC2H3O2 and add to a clean, dry 50 mL beaker. Measure the pH of this solution. Be sure the electrode is properly submerged and gives a stable reading. Record the pH reading in the “Observed pH” column on the report sheet. The value should be within ± 0.2 pH units of the calculated value. From the experimental pH and beginning concentrations of the solution components, calculate the remainder of the entries across the table to pKa . Save this solution for Sections 2.3 and 2.6. 2.2 Calculate the pH of 0.10 M HC2H3O2 solution. List this answer as “theoretical pH” on the report sheet. Test your prediction by placing 5 mL of 0.10 M HC2H3O2 in a test tube and testing its…