Why is it difficult to know whether you have added phenolphthalein to the flask solution before titrating? Considering the experiment, would it make a difference in your calculations if you used a volume of 25 mL of water to dissolve your acid rather than 50 mL?
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- If you have a stock solution of Janus Green B dye that is at a concentration of 1 gram/liter, what is the amount that you would have to remove from the stock solution and mix with distilled H2O to make 50 milliliters of a Janus Green B solution at 100 mg/L 1 mg/ml 250 µg/ml 100 ng/ml 100 pg/mlWhy you should not start a titration with zero mL as an initial volume What is the use of white paper (or background) at the bottom of the erlenmeyer flask? How to deliver a droplet (a.k.a. partial drop or half drop) How to remove air bubbles in the buret Why remove air bubbles? Correct way to empty the contents of a volumetric pipet Arrangement of volume markings on the buret Steps to properly clean and rinse the buret With how many trials or replicates should titrations be performed? Difference between end point and equivalence point? Which hand should be holding the Erlenmeyer flask? How should the meniscus be read?Acid-Base Titration: 10 mL of unknown acid sample was placed in a 250 mL Flask. 3 drops (0.15 mL) of Phenolphthalein was added to the unknown acid sample. The 10.0 M NaOH solution titrant was also dispensed into the unkown acid sample until it changed color. The final volume of the unknown acid sample is 11.680 mL. Please provide the computation for the final concentration of the unknown acid sample.
- How would your experimentally determined vinegar concentration have differed if the tip of the titrator was not filled with NaOH before the initial volume reading was recorded? Explain your answer.What is the importance of non-aqueous titrations in pharmaceutical analysis?What volume of 0.5 M NaOH is required to react completely with 25.0 mL of 1.0 M H2CO3? Assume the reaction of the strong base with the polyprotic acid goes to completion. 12.5 mL 50 mL 25 mL 200 mL 100 mL
- Why is there a need to dilute the samples? What is the effect on titration if dilution is not done?A student performed three KHP titrations in Part 1 in order to standardize their NaOH solution. They reported the following measurements: Determination #1 Determination #2 Determination #3 Mass of KHP + Vial 13.7766 g 13.8285 g 13.8302 g Mass of 'Empty' Vial 13.3405 g 13.3547 g 13.3673 g Final Burette Reading 20.61 mL 22.35 mL 22.69 mL Initial Burette Reading 0.41 mL 0.37 mL 1.03 mL What is the concentration of NaOH (in mol/L) based on the data from their first titration? Report your answer to the correct number of significant figures3. Why does adding a salt solution cause soap to precipitate?
- 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…Which of the following will result to a dimly lit light bulb when subjected to the conductivity test? a. 1.0 M citric acid b. Glacial acetic acid c. Mixture of 10.0 mL 1.0 M Mg(OH)2 and 10.0 mL 1.0 M HNO3 d. 70% (v/v) ethanolFor titration, what is the purpose of a dropwise rate?