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To prepare 50 mL solutions of 0.01 M KMnO4 in water (calculation to prepare chemicals in spectrophotometer)
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- In the Analytical Chemistry laboratory, one of the B.Sc student Ms. Fatma wanted to analyze the presence of Iron(II) ion in the water samples collected from Sohar Industrial Area in the Sultanate of Oman and analyzed by Spectrophotometric method. (1) 250.00 mL of this water sample (Solution A) known to contain unknown amount of FeSO4. She has diluted Solution A by a dilution factor 10 to make 250.00 mL solution, which she labeled Solution B. Using Spectrophotometer, she has measured the absorbance value (0.642) for Solution B at 508 nm using 1.00 cm cell (cuvet). The molar absorptivity value for Fe2* ion at 508 nm is ɛ508 = 30.8 M-1cm1. (i) What volume of the solution A did she require to make the 250.00 mL of Solution В? (ii) in (i)? What instrument should she use to transfer the volume of the Solution A calculated (ii) Concentration of FeSO4 in Solution B. (iv) Concentration of FeSO4 in Solution A. Mass of FeSO4 in Solution A (Show your calculation) (v)A new analytic instrument is capable of detecting picogram quantities of a chemi-cal substance. How many times more capable is this instrument than one that candetect nanogram quantities of the same chemical?(d) Br. e 0.. K :Q'Bu
- 2 Analytical Chemi... -> Analytical Chemistry Problems Q1/ What is the weight, in milligrams, of 0.250 mmol Fe2O3 (ferric oxide), F.wt (159.7 mg/mmol)? Q2/ A solution is prepared by dissolving 1.26 g AGNO3 in a 250-mL volumetric flask and diluting to volume. Calculate the molarity of the silver nitrate solution. How many millimoles AGNO3 were dissolved? F.wt AGNO3 169.9 g/mol Q3/ How many grams per milliliter of NaCl are contained in a 0.250 M solution? F.wt NaCI 58.4 mg/mmol Q4/ Calculate the concentration of potassium ion in grams per liter after mixing 100mL of 0.250 M KCI and 200mL of 0.100 M K2SO4. (atomic weight K 39.1 mg/mmol) Q5/ How many milliliters of concentrated sulfuric acid, 94.0%, density 1.831 g/cm3, are required to prepare 1 liter of a 0.100 M solution? F.wt H2SO4 98.1 g/mol Q6/ You wish to prepare 500mL of a 0.100 M K2Cr2O7 solution from a 0.250 M solution. What volume of the 0.250 M solution must be diluted to 500 mL? Q7/ The concentration of zinc ion in blood serum…Give one application of tacheometry.The color change of a chemical indicator requires an overtitration of 0.03 mL. Calculate the percent relative error if the total volume of titrant is (a) 50.0 mL (b) 10. 0 mL (c) 25.0 mL (d) 30. 0 mL
- Kk.222. I need both parts solution....13. Mg(OH),(s) + 2HC{aq) → M9CL(aq) + 2H,0(1) The student found that 32.00 cm3 of 0 500moldm-3 HCIas needed to react with the Mg(OH2 in a 500 mg tablet. [1g = 1000 mg]. (i) Calculate the amount, in mol, of HCL used. amount = mol (i) Determine the amount, in mol, of Mg(OH), present in the tablet. amount = mol (iii) Determine the percentage by mass of Mg(OH), present in the tablet. answer = A carried out an to find by mass of in an (d) sell tablets to indigestion. indigestion tablet. The student reacted the tablet with dilute acid.A 2.0 g of MgCO3 was dissolved and diluted to exactly 500-mL volumetric flask. If 50-mL aliquot was used in the analysis, what is the weight of MgCO3 present in the aliquot sample
- 3 Bal, (aq)+ 2 Nag POq Caq) 7 BalPO42 + l6 Nal laq • Consider the reaction of 30.0mL of 0.270M Balz with 20.0 mL of 0.3ISM Naz PO4. Lwhat quantity in meles of Balz are preset in the solution? are produced /What quantitg in moles of precipitate E ali Bal were consumed based on the balanced chomical equation? 6) What auantity in males of Na3 Pla aro present in soluction? d) What quantity in moles of precipitate are paduced if all the Naz PO, were cansumed based on the balanced chemi.cal equation? e) which reactant is limisting f What mass (in g) of precipitate is firemed when the limiting reactant is considered?Fluorite, a mineral of calcium, is a compound off the metal with fluorine. Analysis shows that a 43.35-g sample of fluorite contains 21.11 g of fluorine. Calculate the following: (a) Mass of calcium in the sample. g Ca (b) Mass fractions of calcium and fluorine in fluorite. Calculate to 3 significant figures. mass fraction Ca mass fraction F (c) Mass percents of calcium and fluorine in fluorite. Calculate to 3 significant figures. mass % Ca mass % FExactly 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).