d) If the uncertainty in one volume reading for the class A burette used is 0.03 mL., find the percentage uncertainty in the mean titre of NaOH.
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Mean titre is 16.86
2 reading were taken.
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- 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 27A 50.00 (±0.03) mL portion of an HCl solution required 29.71(±0.03) mL of 0.01963(±0.0030) M Ba(OH)2 to reach an end point with bromocresol green indicator. The molar concentration of the HCl is calculated using the equation below (attached image): a.) Calculate the uncertainty of the result (absolute error). M=0.02333(±?????) M b.) Calculate the coefficient of variation for the result. CV= (Sy/y) x 100%Calculate the percentage CH3COOH in a sample of vinegar from the following data.Sample = 15.00 g, NaOH used = 43.00 ml ; 0.600 N H2SO4 used for back titration =0.250 ml ; 1.00ml NaOH is equivalent to 0.0315 g H2C2O4. 2H2O.
- 3. Complete neutralization of 10 ml of phosphoric acid solution by NaOH 0.I N in the presence of phenol phthalein until the appearance of purple color (pH, = 9) 11 ml. of NaOH is consumed. (a) What is the concentration of phosphoric acid? (b) Calculate the indicator error. pk2.1 pK. - 7.2 pK - 124In the experiment conducted to determine the amount of acetic acid in vinegar, 8.2 mL of NaOH standard solution adjusted to 0.098 M was spent besides the phenolphthaleley indicator. Accordingly, which of the following is the amount of acetic acid in the vinegar sample in grams? (Ma (CH3COOH): 60.05 g/mol) A. 0.048 B. 0.024 C. 0.096 D.0.072(a) In performing a titration, why is it better to use a solution of a concentration such that 30-45 mL is required, instead of a more concentrated solution that might only require about 5 mL to reach the end point? (b) To make a standardized NaOH solution, why is it better to prepare a NaOH solution of approxi- mate concentration and then standardize with KHP, rather than to weigh accurately some NAOH pellets, dissolve them, and dilute the solution in a volumetric flask? (c ) In analyzing a 0.003 weak acid by titration with 0.00300 M NaOH, why would you be able to obtain greater accuracy by using a pH meter instead of using a color-change indicator such as phenolphthalein?
- How do you choose the most suitable precipitate for gravimetric purposes if given many choices?Suppose that you want to titrate a sample of vinegar with standard sodium hydroxide solution to determine the concentration of acetic acid in it, and you want to use an indicator to help you determine the end-point. Which of the following indicator would be suitable? (A) Bromocresol Green (Ka ~ 2.0 x 10–5; color: yellow in acid; blue in base) (B) Methyl Red (Ka ~ 5.0 x 10–6; color: red in acid; yellow in base) (C) Bromothymol Blue (Ka ~ 6.0 x 10–8; color: yellow in acid; blue in base) (D) Any of themA 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) A
- Acid-Base titration: Standardization of 0.1 M NAOH Trial 1 Mass KHP used, g 0.297 g Final reading Volume NaOH, mL 15.59 mL Initial reading Volume NaOH, mL 0.23 mL Volume NaOH consumed, mL 15.36 mL Moles KHP used Moles NaOH used Molarity of NaOH solutionI made some titrations and the calculated molarity of HCI was 0.096, 0.097 and 0.098. The nomical concentrsrion of HCl is 0.1. How can I explain my results by comparing it to the nominal concentration if my confidence intervals don't include the nominal concentration?Benzoic acid extracted from 123.16 g of sample required a 27.13 mL titration with 0.0792 M barium hydroxide. What is the percent benzoic acid in the sample?