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x P UTF-8"Chapter 12 Solutions -20 X 2-xythos.content.blackboardcdn.com/5b19550bob538/10621560?X-Blackboard-Expiration%=1649052000000&X Vorksheet.docx Edits will not be automatically saved. Save now d changes A Garamond 14. 三三 of NaHCO3 6. What is the molarity of 325 ml of a solution containing 46.8 (Molar 84.007 g/mol) | mass =

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter20: Applications Of Oxidation/reduction Titrations

Section: Chapter Questions

Problem 20.6QAP

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The water sample from the polluted estuary (number 4), was then subjected to a series ofinstrumental analysis like chromatography and spectroscopy to determine the exact identities of thepollutants. What kind of analysis are done to the unknown?a. Qualitative analysisb. Quantitative analysisc. Characterization analysisd. Fundamental analysis
In the ternary phase diagram experiment acetic acid (7.6 mL) and water (1.4 mL) mixture is titrated with chloroform until the solution is turbid. 12 mL chloroform is consumed to complete the titration. Calculate the final mass percentage of acetic acid. density of chloroform = 1.49 g/mL density of water= 1 g/mLdensity of acetic acid = 1.05 g/mL Mw of acetic acid = 60.05 g/mol
1. Find the number of millimoles of solute in a. 226 ?? of 0.320 ? HClO4. b. 25.0 ? of 8.05 ? 10−3 ? K2CrO4. c. 6.00 ? of an aqueous solution that contains 6.75 ??? of AgNO3. d. 537 ?? of 0.0200 ? KOH. 2. Describe the preparation of a. 5.00 ? of 0.0500 ? KMnO4 from the solid reagent. b. 4.00 ? of 0.250 ? HClO4, starting with an 8.00 ? solution of the reagent. c. 400 ?? of a solution that is 0.0250 ? in I2, starting with MgI2. d. 200 ?? of 1.00% (?/?) aqueous CuSO4 from a 0.365 ? CuSO4 solution. e. 1.50 ? of 0.215 ? NaOH from the concentrated commercial reagent [50% NaOH (w/w), ?? ?? = 1.525]. f. 1.50 ? of a solution that is 12.0 ??? in K+, starting with solid K4Fe(CN)6. 3. Exactly 75.00 ?? of a 0.3132 ? solution of Na2SO3 were treated with 150.0 ?? of 0.4025 ? HClO4 and boiled to remove the SO2 formed. a. What was the mass in grams of SO2 that was evolved? b. What was the concentration of the unreacted reagent (Na2SO3 or HClO4) after thereaction was complete?
Approximately 6.0mL of concentrated perchloric acid (70%) was transferred to a bottle and diluted with about 1.0L of water. A sample containing 251.5 mg of primary standard Na2B4O7.10H2O required 27.41 mL of the HClO4 solution to reach the methyl red end point. Calculate the molar concentration of the HClO4 (Fwt = 382g/mole)
Explain how you would dilute 14.8 M of ortho(phosphoric acid), H3PO4 to make 500.0 mL of 0.296 M ortho(phosphoric acid), H3PO4. (Use the appropriate steps, computations, and safeguards for this scenario.)
Compute for the needed values for slution preparation: 1. Prepare the following solution quantitatively using boiled distilled water per group:250.0 mL 0.0500 M standard HCl solution from 1.0 M HCl 2. a. 500.0 mL 0.1000 M stock EDTA solutionb. 100.0 mL 0.0500 M stock Ca2+ solution
Calculated solely at 25 Celsius of PbCrO4 in pure water and in a .0130M. Na2CrO4 solution. Ksp of PbCrO4 is 2.8x10^-13
What is the percentage purity of acetic acid if 2.6 grams required 32.5 ml of 0.994 N NaOH solution to reach the endpoint? Does it conform to USP requirements for acetic acid 3%-6%?
Full acid, HOOC = CH-COOH is a biphatic acid and we will label it as H2M. Acid constant data for the two protonation phases of the acid: K H.M+H2O = H, 0++HM- HM +H2O = H, 0++M2– a1 = 1.3x10-2 K.2 = 5.9 x 10-7 Measure 0.1 ml of 0.100 M of malic acid with 0.100M NaOH and measure the H variability as a function of the added base volume. A. Calculate the PH value at the beginning of the titration. B. Calculate the pH value at the first equivalent point. C. Calculate the pH value at the second equivalent point. D. Draw the titration curve in the graph. Indicate in the graph titles and units for the axes.
Analysis of a groundwater sample collected from Well No. 8 of Stratford, Ontario showed: pH = 7.8, silica = 10 mg SiO2/L, calcium = 65 Ca2+ mg/L, magnesium = 18.2 mg Mg2+/L, sodium = 76 mg Na+/L, sulphate = 28 mg SO42-/L, bicarbonate = 287 mg HCO3-/L; and chloride = 98 Cl- mg/L. Is the water quality analysis satisfactory from the point of view of analytical accuracy? (hint: aquatic solutions much be electroneutral so check if the solution is charge balanced)
On the redox titration experiment, Standardization of Na2S2O3 with KIO3 standard solution, what can be replaced KIO3 to make safer solvent and auxiliaries( reduced toxic waste)? explain why?
Firstly, What is the final molar concentration of a 500.0ml solution prepared from 15.0 ml of a 12.0 M solution of sulfuric acid? Secondly, solid potassium permanganate and standard laboratory equipment are available. Briefly describe how you prepare 100.0 ml solution of 0.050 M potassium permanganate? Potassium permanganate Mr= 158.03 g mol-1 Thirdly, are methonal (CH3OH) and acetic acid (CH3COOH) expected to be miscible? explain with reasoning