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What is the importance of calibrating analytical balances?
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- What is the importance of Chemical Safety in the laboratory?2. Formaldehyde. Qualitative and quantitative analysis.Identify and explain the mistakes made in the following laboratory protocols: A 1250 mg sample of NaOH was weighed using an analytical balance. The pellets were directly transferred in the balance pans, pellets were gradually added until the reading of the balance was near to 0.2000 mg.
- What is calibration and why is it essential in relation to food analysis? Provide examples.Choose the one correct or one incorrect statement regarding the technique of weighing by difference: the weighing beaker should be moved with a strip of paper used as a handle or strap preparing 4 samples requires only 4 weighings the balance should be tared after each sample is removed from the weighing beaker the weighing beaker must be clean but does not need to be dry the receiving flasks must be both clean and dry before weighing beginsDetails Preparation of Dilute Table Solution Molarity of I₂ Standard Solution Molar Mass (g/mole) Ascorbic Acid Number of Tablets per Analysis Mass (g) Container plus 1 Tablet Mass (g) Container less 1 Tablet Mass (g) of 1 Tablet Volume (mL) of Dilute Tablet Solution Titrimetric Analysis of Dilute Tablet Solution Volume (mL) of Aliquot Portion of Dilute Tablet Solution Titrated Final Buret Reading (mL) Initial Buret Reading (mL) Volume (mL) I₂ Solution Delivered No. of mmol 1₂ Reacted No. of mmol Ascorbic Acid in Aliquot Total No. of mmol Ascorbic Acid Present in the Volumetric Flask Total Mass (mg) of Ascorbic Acid Present in 1 Tablet Average Mass Ascorbic Acid/Tablet Deviation Standard Deviation Coefficient of Variation (%RSD) Reported Composition of Tablet Trial 1 50.00 11.64 0.20 0.02512 M 176.14 1 12.2546 11.7824 0.4722 250.00 Trial 2 50.00 22.80 11.64 Trial 3 250 mg Ascorbic Acid/Tablet 50.00 11.20 0.00 mg Ascorbic Acid/Tablet
- From the calibration curve (yellow table calibration data) calculate the concentration of sugar in solutionIs the concentration of the solution prepared in the question below only approximate because sodium hydroxide is not a primary standard? * Find the mass in grams of sodium hydroxide that will be required to prepare a solution with a concentration of 0.500 mol·dm⁻³ in a 250 cm³ volumetric flask. [Round the answer to three decimal places. Do not type in the unit. Use a decimal point.] *You want to make a solution of the primary standard sodium oxalate. It has a molecular mass of 133.999 g/mol (no error). Your analytical balance has an error of 0.2 mg. You add some weighing paper to the balance and it reads a mass of 0.23626 g. You then add sodium oxalate onto the weighing paper until the mass registers as 2.8539 g. You carefully transfer this to a 250.0 ml volumetric flask with an error of 0.1 ml and dissolve the sodium oxalate in a sufficient volume of water. What is the concentration of the oxalic acid (in M) and what is the absolute error (also in M).
- What is precipitimetry?When coming to the aid of a laboratory accident victim, you should evaluate the situation first before rushing in. true falseExactly 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).