A standard serum sample containing 102 meq/L chloride was analyzed by coulometric titration with silver ion. Duplicate results of 101 and 98 meq/L were obtained. (a) Calculate the mean error (b) Calculate the relative error (c) Calculate the relative accuracy
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- It is a solution of unknown concentration in which a solution of accurately known concentration is gradually added until the reaction is complete. Analyte Endpoint Indicator Titrant(b) Sodium hydroxide reacts with propanoic acid in the following equation: NaOH + CH3CH,COOHCH3CH2COONA + HLO A buffer solution is formed when sodium hydroxide is added to an excess of aqueous propanoic acid. (i) Calculate the number of moles of propanoic acid in 50.0 cm of 0.125 mol dm aqueous propanoic acid. (ii) Use your answers to part (b)(i) to calculate the number of moles of propanoic acid in the buffer solution when 2.00 cm' of 0.500 mol dm aqueous sodium -3 hydroxide are added to 50.0 cm' of 0.125 mol dm aqueous propanoic acid. ) Hence calculate the pH of this buffer solution at 298.15 K.A solution of HCl was titrated against sodium carbonate. What is the normality of acid for Trial 3 in the given data? T1 T2 0.3562 0.3479 0.3042 Weight (g) Initial V (mL) 0.80 1.60 0.40 Final V (mL) 35.20 36.70 39.80 Vol HCI used (ml) 35.10 39.40 N of HC (eq/L) 0.1954 0.1870 Average N of HCl (eq/L)
- A student prepares a weak acid solution by dissolving 0.2400 g HZ to give 100. mL solution. The titration requires 30.0 mL of 0.1025 M NaOH. Calculate the molar mass of the acid. (a) Would the molar mass be too high, too low, or unaffected if the student accidentally used 0.1400 g in the calculation? Explain. ex. too high/too low/unaffected and directly proportional/inversely proportional/ unrelated (b) Would the molar mass be too high, too low, or unaffected if the student accidentally used 20.0 mL instead of 30.0 mL? Explain. ex. too high/too low/unaffected and directly proportional/inversely proportional/ unrelatedA student performed an acid-base titration in the lab and recorded the results as shown below. Look very carefully at the results and answer the questions which follow. 7. 演定結果 21 3. 346 27.40 00 36 終結摘定管讀數(cm) 開始定管數(Cm 所需演定州的積(cm) 44 標 (a) Why do we perform acid-base titrations in our labs? (b) In the titration performed by the student, what was the net ionic equation for the chemical reaction occurring?Q2) a) Explain the titration curve (variation of pH with respect to addition of titrant) with suitable diagram and reactions involved when a strong base is added as titrant to a weak acid as analyte. (b) The saline water discharged from a thermal desalination plant was analyzed and it has following composition.(i) If the discharged water sample contains 4.2 g of potassiumchloride (KCl) per 500 mL of solution, determine its molarity.(ii) The sample contains CaCl2 and its concentration was found to be 0.04M. Calculate grams of CaCl2 present in 100 mL of the sample. (c) In complexometric titration, explain why a constant pH need to be maintained during estimation of metal ions using EDTA.
- Exactly 10.00-mL aliquots of a solution containing phenobarbital were measured into 50.00-mL volumetric flasks and made basic with KOH. The following volumes of a standard solution of phenobarbital containing 2.000μg/mL of phenobarbital were then introduced into each flask and the mixture was diluted to volume: 0.000, 0.500, 1.00, 1.50, 2.00 mL. The fluorescence of each of these solutions was measured with a fluorimeter, which gave values of 3.26, 4.80, 6.41, 8.02, 9.56, respectively. a. plot the data. b. derive a least squares equation for the data plotted in (a). c. find the concentration of phenobarbital from the equation in (b). d. calculate a standard deviation for the concentration obtained in (c).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 27(1) Careless Carlie weighed her KHP sample, but forgot to bring her report sheet along, so she recorded the mass of KHP on a paper towel. During her titration, which required 18.46 mL of base, she spilled some base on her hands. She remembered to wash her hands, but forgot about the data on the towel, and used it to dry her hands. When she went to calculate the molarity of the base, Carlie discovered that she didn’t have the mass of her KHP. Her kindhearted instructor told Carlie that her base was 0.2987 M. Calculate the mass of Carlie’s KHP sample. Show calculations (2) What mass of solid NaOH would be needed to make 645 mL of Carlie’s NaOH solution? Show calculations.
- Formulate a hypothesis regarding the solubility of aspirin at different pH. The experiment A) Three teaspoons of water (approx. 15 ml) were added to one tablet said to contain 300 mg of aspirin. Fizzing was observed. Most of the tablet dissolved, but there were some solid particles. By heating the mug in a microwave for 10 second increments until the water came to the boil (approx. 3x), all of the solid partides dissolved. The solution was left to cool to room temperature and then placed in a fridge and NOTHING HAPPENED. 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 aspirin in 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…1. A sample of pure sodium oxalate, Na2C2O4 , weighing 0.2856 g is dissolved in water, sulfuric acid is added, and the solution titrated at 70°C , requiring 45.12 mL of a KMNO4 solution. The end point is overrun and back-titration is carried out with 1.74 mL of a 0.1032 N solution of oxalic acid. Calculate the normality of the KMNO4 solution. Hint: A redox reaction is involed between oxalate and permanganate. Look at the changes in oxidation state by determining the balanced redox reaction: 5C20,2 + + 2MN2+ 2 Mn04 + 10H* → 10CO2 + 8H20The ethyl acetate concentration in an alcoholic solution was determined by diluting a 10.00-mL sample to 100.00 mL. A 19.00-mL portion of the diluted solution was refluxed with 40.00 mL of 0.04601 M KOH: CH3 СОО С2H; + ОН — СH3 COO + C2H; ОН After cooling, the excess OH was back-titrated with 3.02 mL of 0.05056 M H2 SO4. Calculate the amount of ethyl acetate (88.11 g/mol) in the original sample in grams. Amount of ethyl acetate =