Quantity of Acetic Acid in Salad Dressing Titration Results: 1000 μL aliquots of salad dressing against a sodium hydroxide solution Please only fill in 3 concordant results! Titration number: 1 2 3 Error Final burette reading (mL) 7.9 15 22.2 ±0.05 mL Initial burette reading (mL) 0.9 7.9 17 ±0.05 mL Titre (mL) 7 7.1 7.2 ±0.10 mL Average (mean) volume of concordant titres: 7.1 Concentration of Acetic Acid (M) (to 3 sig figs): 6.88 mL IM Concentration of Acetic Acid (as %w/v) (to 3 sig figs): % Note: %w/v = (g/mL) x 100%
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- A 50.00 (±0.02) mL portion of an HCl solution required 29.71(±0.02) mL of 0.01963(±0.0032) M Ba(OH)2 to reach an end point with bromocresol green indicator. ? of HCL = 29.71?? ? 0.01963 ???? ??(??)2 ?? ? 2 ???? ??? ???? ??(??)2/ 50.00?? = 0.02333 ? Calculate the uncertainty of the result (absolute error).Calculate the coefficient of variation for the result.A student carries out a titration to determine the molar mass and structure of a weak acid A. The student follows the method below. Dissolve a weighed mass of A in 100 cm3 of distilled water and make the solution up to 250 cm in a beaker. Add the solution of A to a burette. Titrate the solution of A with a standard solution of sodium hydroxide, NAOH. (a) What is meant by the term standard solution? (b) Sodium hydroxide is an alkali. What is meant by the term alkali? (c) The student carries out a trial, followed by three further titrations. The diagram shows the initial and final burette readings for the three further titrations. The student measures all burette readings to the nearest 0.05 cm3. Titration 1 Titration 2 Titration 3 Initial reading Final reading Initial reading Final reading Initial reading Final reading 27Which one of the following indicators would be best to use when titrating 0.1M morphine (Kb = 1.6 × 10-6) with 0.3M HCl? Thymol blue (pKa = 1.9) Phenol red (pKa = 7.1) Methyl red (pKa = 4.9) Thymolphthalein (pKa = 9.7) Chlorphenol red (pKa = 6.1)
- Standardization of 1N H2SO4 Titration 1 Titration 2 Titration 3 Titration 4 Mass of flask and Sodium Carbonate 1.5067 g 1.5098 g 1.5076 g 1.5077 Final buret reading (mL) 22 mL 22mL 21.5 mL 22.5 mL Volume of Sulphuric acid used (mL) 30 mL 30 mL 30 mL 30 mL What is the result of my titration?Questions 30-35 refer to the same weak acid/strong base (WA/SB) titration. Prior to the beginning of the titration, there were 0.0090 moles of hypobromous acid present in the flask. The Ką of hypobromous acid is 2.8 x 10-9. (Q30) A 30.00 mL solution of 0.300 M hypobromous acid (HBRO) is being titrated with a solution that is 0.600 M in lithium hydroxide (LIOH). What is the initial solution pH (i.e., when 0.00 mL of titrant have been added)?Direct titration: 10.90 ± 0.02 mL of an unknown KHP solution required 11.72 ± 0.02 mL of 0.1090 ± 0.0006 M NaOH to reach the end point. What is the concentration of KHP in the unknown solution reported with absolute uncertainty? If the unknown solution was prepared by dissolving 5.128 g of the unknown KHP (204.22 g/mol) in 100.00 mL of water, what is the weight percent of KHP in the sample?
- 5. A 300.0 mg sample containing Na,CO3, NaHCO, and NaOH and inert material either alone or in some combination was dissolved and titrated with 0.1000 M HCI the titration required 24.41 ml to reach the phenolphthalein endpoint. And an additional 8.67 mL to reach the methyl red endpoint. Determine the composition of the sample and calculate the percent of each titrated component.In this double titration experiment determining composition of soda ash, you are given the following data: M HCl titrant: 0.0501 M +/- 0.0507 Mass of soda ash sample, g: 0.2505 ± 2.0e-4 (Analytical Balance) Total volume of Sample Stock, mL: 75 ± 0.05 (100mL graduated cylinder) Volume of Sample Stock Aliquot, mL: 25 ± 0.3 Find the missing information. Show solutionsFormulate a hypothesis regarding the solubility of aspirin at different pH.The experimentA) Three teaspoons of water (approx. 15 ml) were added to one tablet said to contain 300 mg of aspirin. Fizzingwas observed. Most of the tablet dissolved, but there were some solid particles. By heating the mug in amicrowave for 10 second increments until the water came to the boil (approx. 3x), all of the solid particlesdissolved. The solution was left to cool to room temperature and then placed in a fridge and NOTHINGHAPPENED. Try this yourself if you can spare two aspirin tablets, your results might look different.• Questions to ask:1. What might the fizzing bubbles be?2. Can you give a chemical explanation?3. Can you write a chemical reaction equation with aspirin reacting with something to give a gas and aspirinin another form?4. What might be the formulation (what the manufacturer mixes with aspirin in making the tablet) “trick”for aspirin to improve solubility?5. How does this compare with…
- A solution of HCl was titrated against sodium carbonate. What is the titer for Trial 1 in the given data? T2 0.3562 0.3479 0.3042 Weight (g) Initial V (ml) 0.80 1.60 35.20 36.70 39.80 Final V (ml) Vol HCI used (ml) 35.10 N of HC (eq/L) 0.1954 0.1870 Average N of HCl (eq/L) AA 0.5131-g sample that contains KBr (MM: 119.0023) is dissolved in 50 mL of distilled water. Titrating with 0.04614 M AgNO3 requires 25.13 mL to reach the Mohr end point. A blank titration requires 0.65 mL to reach the same end point. Report the %w/w KBr in the sample.Part A: Standardization of a Sodium Hydroxide Solution Titration 1 Titration 2 Titration 3 Mass of 125 mL flask 45.849g 46.715g 44.953g Mass of flask and KHP 46.849g 47.745g 46.003g Initial buret reading (mL) 0.5 ml 0.5 ml 0.5 ml Final buret reading (mL) 27.8 ml 26.5 ml 26.7 ml Volume of NaOH used (mL) 45.11 ml 45.06 ml 45.14 ml Calculations Titration 1 Titration 2 Titration 3 Moles of KHP Moles of NaOH Molarity of NaOH Average Molarity of NaOH: _______________