Study figures 31-6 a & b in chapter 31 (page 863) of your prescribed textbook, and draw separation of compounds A and B on a TLC plate (clear labelling will be appreciated).
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- A group of two students obtain the following data for the dissolution of borax. Using the data given, calculate AH-in kJmol-1 for the for borax dissolution studied. Record answer to 2 decimal places. R= 8.314 Jmol-1K-1 Measurement 20.0 °C 50.0 °C Volume of 0.20 M HCl used (ml) 3.97 11.55 [Borate] (M) 0.0397 0.1155 Ksp 0.000250 0.006163 1/T (K-¹) 0.003413 0.003096 Type your numeric answer and submitCalculate the molar solubility of Zn(OH)2 in a solution of 0.0167 M K₂SO4.Calçulate Hhe selubility iA Mofeach of Hhe Salts BaSoy ksp zliS Xlo(9) 2 MgCofA)2 ksp= 9.0Xld-12) A9CN kse: 2.0X10(-12). Dfes ksp-3-7 xlo(-19) Ag2sksp:1.6x10(-49)
- 1. Question: Pd (1I), Au (III) methiomeprazine (C19 H24 N2S2) with the complex. A mixture of their complexesis being analyzed. Pd (II) complex at 480 nm, The measurement results for Au (III) with max peak at 635 nm are as follows. of the mixture What is the concentration?(b=1) Pd(II) Au(III) Mixture 480 nm 3,55x103 2,96x103 0,533 635 nm 5,641x0³ 1,45x10 0,590lelution Cuclz in how to poepase 500 pm lelution of of this 500ppm lorletion, 200pp m Rodetion, wing 160 me water. cath the help cy dibution make: 180 ppm, 160 pprm 80 1२ ० १ ४ 0 । we 100 m l. 1The acid-base indicator HIn undergoes the following reaction in dilute aqueous solution: HIncolor1H++Incolor2 The following absorbance data were obtained for a 5.00 I0-4 M solution of HIn in 0.1 M NaOH and 0.1 M HC1. Measurements were made at wavelengths of 485 nm and 625 nm with 1.00-cm cells. 0.1 M NaOH A485 = 0.075 A625 = 0.904 0.1 M HC1 A485 = 0.487 A625 = 0.181 In the NaOH solution, essentially all of the indicator is present as In-; in the acidic solution, it is essentially all in the form of HIn. (a) Calculate molar absorptivities for In- and HIn at 485 and 625 nm. (b) Calculate the acid dissociation constant for the indicator ¡fa pH 5.00 buffer containing a small amount of the indicator exhibits an absorbance of 0.567 at 485 nm and 0.395 at 625 nm (1.00-cm cells). (c) What is the pH of a solution containing a small amount of the indicator that exhibits an absorbance of0.492 at 485 nm and 0.245 at 635 nm (1.00-cm cells)? (d) A 25.00-mL aliquot of a solution of purified weak organic acid HX required exactly 24.20 mL of a standard solution of a strong base to reach a phenolphthalein end point. When exactly 12.10 mL of the base was added to a second 25.00-mL aliquot of the acid, which contained a small amount of the Indicator under consideration, the absorbance was found to be 0.333 at 485 nm and 0.655 at 625 nm (1.00-cmcells). Calculate the pH of the solution and Ka for the weak acid. (e) What would be the absorbance of a solution at 485 and 625 nm (1.50-cm cells) that was 2.00 10-4 M in the indicator and was buffered to a pH of 6.000?
- In the development o f an analytical method for the quantitative analysis o f iron using Atomic Absorption spectrophotometry (AAS), a linear calibration curve for standards o f 0.00, 5.00, 10.00, 15.00 and 20.00 ppm was prepared. An iron ore sample with an expected iron content o f 40-60% w/w is to be analysed by this method. An approximately 0.5-g sample is taken, dissolved in a minimum amount o f concentrated HC1 and diluted to 1 L in a volumetric flask using distilled water. A 5.00-mL aliquot is removed with a pipette. With explanation, to what volume (10, 25, 50, 100, 250 500 or 1000 mL) should the 5.00 mL aliquot be diluted, to minimize the uncertainty in the analysis?) tecno Al CAMERA Nitrogen in organic Compunds is tested by the addition of few drops of Saturated ironCii) Sulphae Solution to a Small Portion of Sodiem filein filtrate. Dilute hydregen tetmoxosulphate(v) is albso added to the lator Solution Leading to a formatiīon oF prusien blue colour or preaipitate Signalling the presenca Of nitrogen. Shaw these steps Using equations and name your find product(i) (ii) (iii) (iv) 'I OMe HO H g H N Me Br SnMe3 OSiMe3 CHO OH NaNH, NH3 (1) Phl, Pd(PPH3)4 THF, reflux 1. Ph3P=CMe2 2. "Bu4NF 3. H30 + CH₂12, Zn C C₂H₂NO D C₁1H₁1N E C10H16O F C15H26O2
- 9- I. FilteringII. EvaporationIII. Magnet zoomIV. Dissolving in waterA mixture of iron powder, naphthalene and table salt.To separate the mixture into its components, the above work-In what order should the actions be applied?a)IV, III, I, II B)III, IV, II, I NS)III, IV, I, II D)II, III, I, IV TO)IV, I, III, IIName: Date: Section: Data Report Sheet: Spectrophotometric Determination of an Equilibrium Constant. Part A: Determination of a Calibration Curve: Stnd.1 Std. 2 Stnd. 3 Stnd 4 Stnd. 5 Stnd. 6 (CH) [Fe(SCN)*] Column A Absorbance Column E Equation of Calibration Line: Correlation Coefficient: Slope (bɛ): Part B: Determination of K Expt. 1 Expt. 2 Expt. 3 Expt. 4 Expt. 5 (Fe"linitial (Table 1) [SCNJinitial (Table 1) [Fe(SCN)**]eqi. Tịnbə Column F [Fe"lequil. ([Fe"Imital -[Fe(SCN)**I«qull.) [SCNleguil [SCN'], (ISCN']initial "[Fe(SCN)*"lequil. K Average K:Part IV: Equilibrium Involving Chromate and Dichromate Ions Steps 2 & 3 Step Steps 5 & 6 4 Steps 7 & 8 Step 9 2CrO₂² (aq) + 2 H (aq) Cr₂O, (aq) + H₂O (1) Initial Colour + 1 M NaOH + 1 M HC1 Ba² (aq) + CrO² (aq) BaCrO. (s) 0.1 MK₂CrO₂ Yellow Yellow Yellow Initial Colour + 1 M HC1 + 1 M NaOH 0.1 MK₂CrO₂ + 0.1 M Ba(NO3)2 Other Observations: 0.1 MK₂CrO₂ Yellow Orange Yellow Initial Colour Yellow 0.1 MK₂Cr₂O, Orange Initial Colour + 1 M NaOH Yellow + 1 M HC1 Orange 0.1 MK₂Cr₂O, Orange Yellow Orange 0.1 MK₂Cr₂O₂ + 0.1 M Ba(NO3)2 Orange Orange Orange Immediately cloudy with white precipitate and yellow solution + 0.1 M Ba(NO₂)₂ Orange + 1 M HC1 Orange with precipitation + 1 M NaOH Yellow with precipitation 0.1 MK₂CrO₂ 0.1 MK₂Cr₂O, Immediately a lot of precipitate Very little precipitate formed in formed in yellow solution orange solution