Would the molarity of HCl as determined in this experiment be too high or too low if:The buret is contaminated with an acid solution. The buret contains a large air bubble in the tip, which disappears in the course of the titration.
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Would the molarity of HCl as determined in this experiment be too high or too low if:The buret is contaminated with an acid solution. The buret contains a large air bubble in the tip, which disappears in the course of the titration.
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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.Suppose there was a large air bubble in the tip of the acid burette during the titration and it was dislodged toward the end of your titration. Explain the effect that this would have on the calculated value of the acid's molarity.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)
- Name: Date: Experiment # 11: Acid-Base Titration: Standardization of NaOH Data and results Data table *Remember to include units Trial 1 Trial 2 Trial 3 Trial 4 Mass of KHC8H4O4 (KHP) Initial buret reading (NaOH) Final buret reading (NaOH) Volume of NaOH used Results table Trial 1 Trial 2 Trial 3 Trial 4 Moles of KHP Moles of NaOH Volume of NaOH (L) Molarity of NaOH Average molarity of NaOH Sample calculation: In the space below show complete calculations for moles of KHP and molarity of NaOH using data from TRIAL 2 only. Include formulas and units.Compute for the titratable acidity of vinegar sample if 6 ml of 1.0 N NaOH was used to titrate 25 ml of sample. Can this sample be used commercially if the standard is 4% titratable acidity?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 ofphenolphthalein 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
- In a titration experiment what would having a drop on the tip of the buret do for the accuracy of the end point? Is it a problem to have a drop on the end of your belt? Why or why not?Which one of the following is NOT a source of error during a titration? Group of answer choices Adding too much sodium hydroxide solution to the analyte Refilling the buret during a titration trial Rinsing the buret with the analyte Adding indicator to the analyteUsing 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.
- Would you recommend adding the phenolphthalein and methyl orange indicators together at the start of the titration to save time?The 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?Why is ethylene-di-amine tetra-acetic acid (EDTA) work as a base in complexometric titration? answer at your own words and answer should be to the point, not any irrelevant words