1. (a) A solution of NaCl is prepared by dissolving 0.0056 g NaCl with enough H2O in a volumetric flask to yield a final volume of 10 mL. Assuming a standard (0.1 mg) analytical balance and class A glassware is employed, calculate the concentration of the solution (M) and its corresponding error. The atomic weights of Na and Cl are 22.98976928(2) and 34.45(1), respectively (the number in parentheses indicating the error in the last digit). (b) What would the error be if a 1mL transfer pipet was employed (10x) rather than the 10 mL volumetric flask?
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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)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 % FYou are required to standardize a dilute solution of sulphuric acid, and undertake the following steps:(i) 4.805 g of solid sodium tetraborate (Na2B4O7) are added to a 250 mL volumetric flask, and the solution made up to the mark with distilled water.(ii) 25.00 mL aliquots of the stock solution from (i) are transferred to conical flasks, for titration against the sulphuric acid solution in the burette.(iii) You perform titrations using two different indicators: bromocresol green, and phenolphthalein.With bromocresol green, the average titre volume is 22.50 cm3, while with phenolphthalein, the average volume is 9.50 cm3.(a) Write the balanced equation for the reaction between Na2B4O7 and sulphuric acid
- Hydrogen peroxide solutions can easily be decomposed by dust, trace amounts of metals or light. It istherefore necessary to periodically determine the purity of the peroxide solutions.This can be done via a redox titration as follows: The density of a particular surgical grade hydrogen peroxide solution is 1.11g.cm-3. Exactly 10 mL of this solution was pipetted and quantitatively transferred, along with a sufficientamount of a dilute sulphuric acid solution, into a 250.00 mL volumetric flask and made up to the mark. A 25.00 mL portion of this diluted solution is pipetted into a conical flask, and titrated with a0.372 M KMnO4 solution. The endpoint of the titration is determined when the colourless solution in the conical flask turns apersistent bright pink due to the presence of excess permanganate ions. The average titration value is 26.20 mL of the KMnO4 solution 1.Determine the percentage of the hydrogen peroxide in the solution sample.2. Naturally occurring manganese…Be sure to answer all parts. Fluorite, a minéral of calcium, is a compound of the metal with fluorine. Analysis shows that a 10.78-g sample of fluorite contains 5.520 g of calcium. Calculate the following: (a) Mass of fluorine in the sample. 19.00 g F (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 % FThe organic base, tris-(hydroxymethyl)aminomethane (or simply TRIS or THAM) is an excellent primary standard. A 0.2486 g sample of the primary standard grad TRIS, (CH2OH)3CNH2 (M.M. = 121.14) was dissolved in distilled water and required 24.88 mL of a hydrochloric acid solution. Calculate the molarity of the solution
- You are preparing a 100.0 mL standard solution needed for titration analysis. The NaOH (40 g/mol) pellets are measured to be 0.5341 g in a balance with acceptable uncertainty of +0.001 g. Mass of the pellets is recorded after taring the container. The pellets are put in a beaker and added with 50 ml distilled water measured by a graduated cylinder. The solution is then quantitatively transferred to a 100-mL volumetric flask with uncertainty of ±0.08 mL and diluted to a 100-mL mark. What is the concentration (M) of the solution and estimate its uncertainty by propagation? Assumption: There is no uncertainty in molar mass. Express your answer as C+/- u M.The aluminum in a 1.200 g sample of impure ammonium aluminum sulfate was precipitated with aqueous ammonia as the hydrous Al(OH)3.xH2O. The precipitate was filtered and ignited at 10000C to give anhydrous Al2O3 which weighed 0.1798 g. Express the result of this analysis in terms of % Al2O3.A 0.879 g sample of a CaCl2·2H2O/K2C2O4·H2O solid salt mixture is dissolved in ~100mL of deionized water. The precipitate, after having been filtered and air-dried, has a mass of 0.284 g. The limiting reactant in the salt mixture was later determined to beCaCl2 ·2H2O. a.Write the ionic equation for the reaction. b.Write the net ionic equation for the reaction. c.How many moles and grams of CaCl2 ·2H2O reacted in the reaction mixture? d.How many moles and grams of the excess reactant, K 2C2O 4H2O, reacted in the mixture? e.How many grams of the K2C2O4·H2O in the salt mixture remain unreacted (inexcess)? f.What is the percent by mass of each salt in the mixture
- (a) A solution of 20.91 % by weight H₂SO4, has a specific gravity of 1.150. What is the normality of this solution? (b) Water is added to dilute this solution to a solution of 3.03% by weight H2SO4 (SG=1.020). What is the new normality of the resulting solution and how were they mixed? (Assume 100 mL of the original solution was used.)Although other solvents are available, dichloromethane(CH₂Cl₂) is still often used to “decaffeinate” drinks because thesolubility of caffeine in CH₂Cl₂ is 8.35 times that in water.(a) A 100.0-mL sample of cola containing 10.0 mg of caffeine is extracted with 60.0 mL of CH₂Cl₂. What mass of caffeine re-mains in the aqueous phase? (b) A second identical cola sampleis extracted with two successive 30.0-mL portions of CH₂Cl₂.What mass of caffeine remains in the aqueous phase after each extraction? (c) Which approach extracts more caffeine?A volumetric calcium analysis on triplicate samples of the blood serum of a patient believed to be suffering from a hyperparathyroid condition produced the following data: mmol Ca/L = 3.15, 3.25, 3.26. What is the 95% confidence interval for the mean of the data, assuming no prior information about the precision of the analysis?