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- In an unprecedented initiative, the professor chose you to carry out the determination of a special sample in order to verify the inherent indication system. For that, an aliquot of 25.00 mL of a solution containing Fe(III) salts was titrated with EDTA 0.00982 mol/L, using potassium thiocyanate as indicator. In this case, you have found the volume of 31.10 mL of titrant to End Point. Based on the information given in the table, choose the option that best describes/explains the process linked to the indication system of the Final Point of the degree: (a) The indication of the system will be given by the disappearance of the reddish coloration, due to the displacement reaction: Fe(III) complex with EDTA is formed in detriment of the Fe(III) complex with thiocyanate. (b) The indication of the system will be given by the appearance of a reddish color, in function of the displacement reaction: Fe(III) complex with thiocyanate is formed in detriment of the Fe(III) complex with EDTA. (c) The…In complexometric titration ‘the reaction with analyte should be rapid andcomplete’ give reason with suitable justification for the above statement.True or False: Blank titration is indicated for the determination of the concentration of a sample. Can you please expound why?
- Which of the following is a good description of a standard solution as a titrant? a) selectively reactive with the analyte b) only reacts with the matrix c) oxidize when exposed to air d) reacts very slowly but completelyExplain why in Mohr's method neutral medium should be used in titration of AgNO3?The concentration of ammonia in a cleaning product was determined by back titration.Firstly, 10.00 cm3 of the cleaning product was pipetted into a large conical flask,containing 250.00cm3 of 0.50 mol/l HCl to give Solution A.Following a period of reaction and shaking, 50.00cm3 of Solution A was removed anddiluted to 250 cm3 with water in a volumetric flask to give Solution B.20 cm3 samples of Solution B were titrated against 0.05 mol/l Na2CO3 solution, givingan average titre of 12.45 cm3. i) Write equations for the reactions that have taken place.ii) Determine the concentration of NH3 in the original cleaning product in mol/l,g/l, ppm, and % w/v.
- In determination of mixed alkali, does adding H2O to the analyte can afect the process of titration?What is the importance of calibrating pH electrode and weighing balance during buffer preparation? What will happen if either of them is uncalibrated? Which will result to bigger error?Q: The concentration of the sulphate ion in a mineral water can be determinedby the turbidity which results from the addition of excess BaCl2, to a quantityof measured sample. A turbidometer used for this analysis has been standardisedwith a series of standard solutions of NaSO4. The following resultswere obtained:Standard solution Conc. (SO4)2− (mg/L) Reading of turbidometerS0 0.00 0.06S1 5.00 1.48S2 10.00 2.28S3 15.00 3.98S4 20.00 4.61i. In supposing that a linear relationship exists between the readings takenfrom the apparatus and the sulphur ion concentration, derive an equationrelating readings of the turbidometer and sulphate concentration(method of least squares).ii. Calculate the concentration of sulphate in a sample of mineral waterfor which the turbidometer gives a reading of 3.67.
- A student has a sea water sample which contains Ca2+ ions . Describe briefly how he willdetermine the concentration of Ca2+ ion in the sample using a simple titration. Explain the colourchanges at the endpoint. Which medium is suitable for performing the titration, acidic or basic medium and why?Determine the relationship between the observed/apparent value (EX) VERSUS that of the true value (ET) for the quantity being sought by writing either <, >, or = on the space provided Determination of water hardness using complexometric titration. During sample analysis (ppm CaCO3), the volume for blank correction was not subtracted to the volume of titrant. EX Blank 1 ET50 cm3 of 0.05 M weak acid solution is titrated with 0.1 M NaOH solution. The measured pH valuesare 7.345 and 7.497 at the consumptions of 6.0 and 6.1 cm3, respectively. What value of the buffer capacity can be calculated in the solution at pH = 7.421?
