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
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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
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- Which of the following should be done first if, during a titration using phenolphthalein as an indicator, a student adds more than the expected amount of solution from the buret and the solution still hasn't turned pink? Hint: Asking the TA should never be your first step when problem solving. Ask the TA to do the titration. Put water in the burette. Pour out all of your solutions and leave the lab with a failed experiment. Add acid to the flask and continue the titration. Add a drop of phenolphthalein indicator to the solution to see if it turns pink.List the observations of a manual titration experiment and explain your expectations. of the outcome of this experiment. This should include color change and when the equivalence point (endpoint) might be reached. When do you stop and why.1. This acid affects other indicators if phenolphthalein is not used in the assay of sodium bicarbonate. 2.Determine the type of assay employed for this substance: SODIUM HYDROXIDE 3.This is the difference between the largest and smallest results in a series of measurements. 4.Determine the color of the indicator in a given condition: PHENOLPHTHALEIN IN AN ACIDIC ENVIRONMENT. 5.This is the weight in grams which is chemically equivalent to 1 gram-atom of hydrogen. CAN YOU HELP ME WITH THIS ONE PLS.. THE ANSWERS ARE ON THE WORD CLOUD (IMAGE ATACHED)
- What questions and topics where asked on the interview and how did you think you did? Converted to an essay question? This question is about a buffer solution made by mixing together solutions containing ethanoic acid and sodium ethanoate. a) If you add a small amount of an acid such as dilute hydrochloric acid to this, the pH doesn't change much. Explain what happens to the extra hydrogen ions you have added (think in terms of pkas, acid/base and conjugate acid/base). . b) If you add a small amount of an alkali such as sodium hydroxide solution to the buffer solution, again the pH doesn't change much. There are two ways in which the extra hydroxide ions can be removed. What are they?Using the letters on the image, identify each component of the titration set-up. Buret clamped to a ring stand with a beaker underneath. The letter A appears at the top of the buret, the letter B appears midway down the buret, the letter C appears at the bottom of the buret, the letter D appears next to the beaker, and the letter E appears on the other side of the buret, near the ring stand.List the observations of a manual titration experiment and explain your expectations. This should include color change and when the equivalence point (endpoint) might be reached. When do you stop and why.
- A buffer contains significant amounts of acetic acid and sodium acetate. a)Write an equation showing how this buffer neutralizes added acid (HBr(aq) Express your answer as a chemical equation. Identify all of the phases in your answer. b)Write an equation showing how this buffer neutralizes added base (KOH(aq) Express your answer as a chemical equation. Identify all of the phases in your answer.By applying Gravimetry, Titration (Chemical indicator) and Potentiometry lessons which technique should be used in following situations. Explain your answer. In your explanation, state what is the advantage of the technique you chose over other technique and /or the barrier/difficulty of using the technique. Your choice should not be dependent on cost. Answer in less than 7 sentences. For chem students - Total Acid content per tablet of a newly developed drug that has yellow coating Target level is 1%.a) Compare between equivalence point and endpoint. Distinguish which point comes first. b) James performed an acid base titration experiment. A 25 mL sample containing HCl was transferred to Erlenmeyer flask using volumetric pipette. HCl sample was titrated against standardized 0.5010 M NaOH. An average titre volume of 24.35 mL was reported. Suggest a suitable pH indicator for James to be used in this experiment. Predict the initial concentration of the HCl. c) Alan and friends wish to sketch a weak acid strong base titration curve. Before they can do so, they need some data points. In a case where 50 mL of 0.20 M CH3COOH (Ka = 1.80 x 10-5 ) was titrated with 0.05 M NaOH, deduce the pH after addition of different volumes of NaOH. (i) 0 mL NAOH (ii) 100 mL NaOH (iii) 200 mL NaOH
- Compare the results of two experiments: First, a small amount of base is added to an unbuffered solution with a pH of 7. Second, the same amount of base is added to a buffered solution with a pH of 7.In the laboratory, a general chemistry student measured the pH of a 0.392 M aqueous solution of hydrocyanic acid to be 4.920. Use the information she obtained to determine the Ka for this acid. Ka(experiment)BONUS: During a titration, ammonia is added to the flask and titrated with HCI. Looking at the titration below and the indicator table, what would be a good indicator to use for this experiment? What color change would be observed? 12 10 20 40 60 80 100 120 140 mL d.1 M HCI TABLE 16.7 Common Acid-Base Indicators Approximate pH Range over which the Color Changes Color Change Gower to higher pH) Indicator Thymol blue Micdni otanpr 3234 Filyl d Mechyl purple Broeno purpk