It is the type of analytical method that relies on the absolute stoichiometric equivalences of balanced chemical reactions in order to compute the amount of analyte present in the sample. a. Instrumental methods b. Blank Correction Methods c. Classical methods
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- 1. Samples that should not be stored should be prepared/analyzed as soon as possible, especially for measurement…a. hardnessb. Nitritec. Conductivityd. Phenol 2. The following are general sample treatments in pesticide analysis, except…a. Extractionb. Cleaningc. Concentrationd. Filtering12. This type of analysis means that the amount of some constituents were determined. Complete analysis a. b. Ultimate analysis с. Partial analysis d. Single-component analysis 13. This process is one way of reducing occluded particles and mechanical entrapment impurities. a. Washing b. Heating c. Stirring d. DigestionDeterminati an 25 ml by dissolving 110n (111) per 1 This (as ml 750ml experiment Solution The to of was The a and process Q on added The portion layer taken 1 volumetric diluted Litre Colution Two These of in diluted ml soo 1% ETA of Question A. reaction an Solution 0₁ 446 9 of A. R. hydrated sulphate, (NH4) Fe (504) ₂ · 12H₂0 2 of distilled then of wertel) 0,0446 g/L of lion Absorbance was 250 ml in to ·layers frask was Is 2. 3. Was Chlore form and were 5 ml, 10 ml, 15 ml por tions 4. Iron • iron (111) four oxine it mixture the done. (111) seperatory conducted Volume SMT as 10 ml 15 ml 20 ml Plo + absorbance formed readings a (A.R) Jayer measured the por tions Solution was Water diluted out 20 ml were then Each of these mark against funnel as was after with for 8- ity droxy quinolate. follows. to iron (111) solution was prepared of then Calibration was ) 10 obtain collected. ammonium F. W-481,979 then these Absorbance 0,076 0,169 9185 0₁234. Shook. the shaking added portions…
- d Tap - Cengage Learning vo/index.html?deploymentld%3D55750828934189288909969212&EISBN=9781305657571&snapshotld%3D2199898&id=. * INDTAP Q Search this co Use the References to access important values if needed for this question. The colorless gas nitryl chloride (CINO,) reacts with water to give a mixture of nitric acid and hydrochloric acid . (a) Write a balanced chemical equation for this reaction. (b) Determine the concentration (in moles per liter) of each of the acids that result from the complete reaction of 3.64×10-² moles of nitryl chloride with enough water to give a solution volume of 746 mL. nitric acid M hydrochloric acid : M Submit Answer 5 question attempts remainingC. INSTRUCTOR LOCKER SECTION NAME NAME SECTION LOCKER INSTRUCTOR DATA SHEET 1 DATA SHEET 2 Naz CO3 Ala(5oa) II. Studying the Reactions of Unknown 2 30 VO3T0 1. Studying the Reactions of Known Solutions :- Clear OBSERVATIONS OBSERVATIONS Solution Solution 3 4 XX Pale S Whi te XX 1 XX NaCI Distinc whie Pardicins Whit Particks Very Milk XX XX NOIO3 C White(I Partales Pale O while XX BaCla Var yA, Very Milky Whi ke XX white Gran Very Pale 4 Pale Na, CO Milky Distinc white Particles XX Very Bacl 5 Mlk whit XX white Very Pale MilkyWhit white Partich Pale XX orand eases S: Soluable I: Inslabe W/ white on XX 6 edses Chunks S: Solvable I: Insoluoble 0 nom inCHC* Chapter... G N. F ● C L G A H Assuming that no equilibria other than dissolution are involved, calculate the concentration (in M) of all solute species in each of the following solutions of salts in contact with a solution containing a common ion. Show that changes in the initial concentrations of the common ions can be neglected under the 5% rule. (See the Solubility-Prom Constants table. Assume Kw = 1.01 x 10-14.) (a) TIBr in 1.320 M HBr [TI+] [Br] [H+] % error due to approximation (b) PbI, in 0.0368 M MgI₂ [Pb²+] [I] [Mg²+] % error due to approximation M ] M [OH ] % error due to approximation M % M (c) Ag₂ CrO4 in 0.230 L of a solution containing 0.876 g of K₂ CrO 4 [Ag+] [Cro42-] [K+] % error due to approximation M M % M (d) Co(OH)₂ in a solution buffered at a pH of 10.975 [Co²+ M M % M M % C
- 2. In the deposition method, one of the conditions that must be met is…a. The precipitate has a high solubility or solubility productb. The precipitate formed must be quite difficult to dissolvec. The precipitate formed does not have to be quite pured. Free precipitate form 3. One of the conditions for selecting a sampling location…a. Near motorized vehiclesB. Near the incineratorC. Near the treeD. Far from buildings1. A group of students from the instrumental analysis laboratory of the course analyzed the sodium content in a serum sample using ICP-OES. They used 5 flasks with 25 mL of sample serum in each and added different amounts of a standard 2.640MNaCl solution to a total volume of 50 mL . Calculate: a. Equation for calibration b. Serum sodium concentrationIn the deposition method, one of the conditions that must be met is…a. The precipitate has a high solubility or solubility productb. The precipitate formed must be quite difficult to dissolvec. The precipitate formed does not have to be quite pured. Free precipitate form
- c. potassium iodide + barium nitrate Observation Balanced Eqn. Complete lonic Eqn. NIE12. For each reaction below, the starting mass/volume of each reagent is provided as well as the final mass of product isolated. Calculate the theoretical and percent yield for each reaction. a. b. OH OH + l MW 122 1.50 g CI MW 141 d 1.21 g/mL 0.250 mL MW 60.1 7.40 g 1. PhMgBr MW 181 905 mg 2. HCI H3PO4 OH Ph MW 164 1.86 g Ph MW 260 547 mg + H₂OA student was tasked to perform gravimetric analysis of a soluble sulfate. His unknown sample weighed 0.7543 g. The sample underwentprecipitation using BaCl2 and was digested for overnight. The precipitate was then filtered off to obtain white crystalline precipitate that was collected inan ash less filter paper. In performing constant weighing, he obtained a crucible mass that is 29.9442 g. After burning his samples inside the crucible,the obtained mass was 30.3375 g. Compute for the theoretical % SO3 obtained by the student and the theoretical mass (g) of SO3 that should be obtained by the student using his weighed sample
