artfHomieOWLV2 Online teachin Xtps://cvg.cengagenow.com/ilm/takeAssignment/takeCovalentActivity.do?locator3Dassignment-take&takeAssignmentSessionLocator=Dassignment-take[References]If 37.65 mL of HCl is required to titrate 2.575 g of Naz CO3 according to the following equation, what is the concentration (mol/L) of the HCl solution?Na, CO3 (aq) + 2 HCI(aq)2 NaCl(aq) + CO2 (g)+H,0(2)Concentration =%3DSubmit AnswerTry Another Version10 item attempts remainingPreviousShow Hint?へE日acSUprt schoref812delete00 S Smarttl iNu Announcements2020 SprHomeSe OWLV2 | Online teachin Xhttps://cvg.cengagenow.com/ilm/takeAssignment/takeCovalentActivity.do?locator=assignment-take&takeAssignmentSessionLocator=assignment-take[References]If 37.65 mL of HCl is required to titrate 2.575 g of Nag C03 according to the following equation, what is the concentration (mol/L) of the HCl solution?Naz CO3 (aq) + 2 HCI(aq) 2 NaCl(aq) + CO2 (s) + H20(4)Concentration:м%3DSubmit AnswerTry Another Version10 item attempts remainingPreviousShow Hat

Given, Volume of HCl solution = 37.65 mL = 0.03765 L (1 mL = 0.001 L) Mass of Na2CO3 = 2.575 g…

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Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter4: Calculations Used In Analytical Chemistry

Section: Chapter Questions

Problem 4.24QAP

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Give typed solution only. 34.0 mL of 1.34 M hydroiodic acid is added to 39.1 mL of calcium hydroxide, and the resulting solution is found to be acidic. 25.8 mL of 0.899 M sodium hydroxide is required to reach neutrality. What is the molarity of the original calcium hydroxide solution?
Zhongli is a speleologist tasked to analyze the CaCO₃ content of a limestone stalactite. A 5.0000-g sample was dissolved in 25.00 mL of 1.350 M HCl, it was then heated to expel any CO₂ formed. The excess HCl was titrated to a phenolphthalein end point, it used 37.50 mL of 0.1200 M NaOH. A. How many moles of HCl was added initially to digest the limestone sample? B. How many moles of CaCO₃ is present in the limestone sample? C. What is the purity of the limestone in terms of %w/w CaCO₃?
A solution of I3- was standardized by titrating freshly dissolved arsenious oxide (As4O6, FM 395.683). The titration of 25.00 mL of a solution prepared by dissolving 0.3663 g of As4O6 in a volume of 100.0 mL required 31.77 mL of I3-. Calculate the molarity of the I3- solution. As4O6(s) + 6H2O ⇌ 4H3AsO3 H3AsO3 + I3- + H2O ⇌ H3AsO4 + 3I- + 2H+ a. 0.01657 M b. 0.02914 M c. 0.1166 M d. 0.0957 M
3.) In the assay of NaHCO3, 3.0g of the solid is dissolved in 25mL water. What is the normality? How many mL of 1N H2SO4 will be required to neutralize this solution? From this volume of acid, compute the percent purity of NaHCO3.
Zhongli is a speleologist tasked to analyze the CaCO₃ content of a limestone stalactite. A 5.0000-g sample was dissolved in 25.00 mL of 1.350 M HCl, it was then heated to expel any CO₂ formed. The excess HCl was titrated to a phenolphthalein end point, it used 37.50 mL of 0.1200 M NaOH. How many moles of HCl was added initially to digest the limestone sample? How many moles of CaCO₃ is present in the limestone sample? What is the purity of the limestone in terms of %w/w CaCO₃?
Lemon juice contains citric acid which is tribasic(H3Y). 25cm^3 of lemon juice was diluted to 250cm^3. 25cm^3 of the solution was neutralized by 15cm^3 of 0.1M sodium hydroxide. a) Calculate; i) concentration of the diluted solution of lemon juice ii) concentration of the original lemon juice. iii) percentage by mass of citric acid in lemon juice.
Treatment of hydroxylamine (H2NOH) with an excess of Fe (lIl) results in the formation of N2O and an equivalent amount of Fe(II): 2HNOH + 4Fe3+ = N2O(g) + 4Fe2+ + 4H+ + H2O Calculate the molar concentration of an H2NOH solution if the Fe(ll) produced by treatment of a 25.00-mL aliquot required 14.48 mL of 0.01528 M K2Cr2O7.
Calculate the volume in liters of 0.545 M KOH necessary to titrate 0.0113 moles of hydrochloric acid, HCl, to a phenolphthalein end-point. Report the answer with three significant figures.
3 L contaminated air 50 mL 0.0116 M in an air pollution analysisCarbon dioxide (CO2) BaCO3 is passed through Ba (OH) 2 solution.is precipitated as. Excess of base, next to phenol phthalate (f.f.) indicatorIt is titrated with 23.6 mL of 0.0108 M HCl. CO2 in this air sampleCalculate its concentration in ppm. (Density of CO2Take it as 1.98 g / L. C = 12, O = 16 g / mol).
A sample is known is known to consist of NaOH (40 g/mol) or NaHCO3 (84 g/mol), or Na2CO3 (106 g/mol) or possible compatible mixtures of these, together with inert matter. With methyl orange, a 1.10 g sample requires 31.4 ml of HCl (of which 1.00 ml ≈ 0.0140 g CaO, 56 g/mol). With phenolphthalein, the same weight of sample requires 13.3 ml of the acid. Calculate the percentage of inert matter in the sample.
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
If 1.000 ml. of a solution of KMn04 is equiva- lent to 0.1000 millimole of NaCHO2 (sodium formate) in the fol- lowing titration: 3CHO2- + 2MnO- + H2O -> 3CO2 + 2MnO2 + 5OH-, what is the value of the KMnO4 in terms of grams of CaO in the volumetric method for calcium in which that element is precipitated as CaC2 4 .H2O and the precipitate is filtered, dis- solved in dilute H2S04 , and the oxalate titrated with permanganate?

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