7. A 3.00 g sample of pure iron is dissolved in hydrochloric acid and creating a 500.0 mL solution containing Fe) which is then titrated with KMnO4(aq) a) Draw a diagram that shows the lab setup. Your diagram should include the following • A Burette • Erlenmeyer Flask • Titrant • Analyte/Sample ₂2+ b) What volume of 0.0500M KMnO4(aq) is required to titrate a 25.0 mL sample of the Felda) solution?

7. A 3.00 g sample of pure iron is dissolved in hydrochloric acid and creating a 500.0 mL solution containing Fe) which is then titrated with KMnO4(aq) a) Draw a diagram that shows the lab setup. Your diagram should include the following • A Burette • Erlenmeyer Flask • Titrant • Analyte/Sample ₂2+ b) What volume of 0.0500M KMnO4(aq) is required to titrate a 25.0 mL sample of the Felda) solution?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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answer in mL,to make sure your math is correct know it has to be less than 25 mL since the buret is 25 mL
Use the data below to determine the % by mass of Fe to TWO decimal places, if a 0.019 M KMnO4 solution was used for the titration. (MM Fe = 56 g/mol) mass of iron compound (g) 0.637 initial buret reading (mL) 0.86 16.60 final buret reading (mL) Type your answer...
Given the reaction: Fe^3+ + SCN^- --> FeSCN^2+. How many moles of SCN are there?
Mark and John, two vinegar enthusiasts, are each tasked to determine the acetic acid content of their respective vinegar concoctions by titration. First, a 1 M-labeled KOH solution was standardized against the KHP (MW = 204.22 g/mol) standard that is 99.4% pure. In the process, 0.540 g KHP was found to require 2.80 mL of the KOH solution to completely react up to the phenolphthalein endpoint. Then, Mark and John both prepared their samples by taking 10.0-mL aliquots of each vinegar and diluting them to 25.0 mL. Using the same titrant and indicator, Mark’s vinegar required 18.60 mL of the standardized titrant to reach the endpoint, while John’s vinegar required 16.50 mL of the same titrant to reach the same endpoint. Question: What is the acetic acid concentration of Mark’s and John’s vinegar in molarity given that the Concentration of KOH is 9386 M?
Hello, can you help me understand the question attached below?
You are performing an experiment in lab that involves the titration of 25.0 mL of H2SO4 solution. You titrate the acidic solution with 0.8067 M NaOH and the equivalence point is reached by the addition of 17.31 mL of NaOH solution. Using the balanced equation below, calculate the molartity of H2SO4 in the flask. Do NOT include units. 2NaOH(aq) + H2SO4(aq) --> 2H2O(l) + Na2SO4(aq)
d) In 4 test tubes, divide equally the solution prepared in procedure c into four parts. Reserve the first test tube as a standard. 1) To the second test tube add 1 mL of ferric chloride solution. 2) To the third test tube add 1 mL of ammonium thiocyanate solution. 3) To the fourth test tube add a pack of solid ammonium chloride. Compare the color obtained in test tubes 2,3,4 with the first test tube(standard solution). Record and explain your observations. Was the reaction in procedure c complete? Can the reaction be made reversible? Define common ion effect. 2. a) Heat a pack of sawdust in a stained test tube. Observations. Is the reaction reversible or irreversible? Complete or incomplete? b) Recall the reactions of: i. Magnesium ribbon (ignited) and oxygen; ii. potassium chlorate and heat; iii. blue vitriol and heat. Write the chemical equations for each of the above reactions and classify each as reversible or irreversible and complete or incomplete?
Can you help me with the attached probelm?
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||| y google - Yahoo Search Results mL Q OCHEMICAL REACTIONS Determining the volume of base needed to titrate a given mass... Explanation 0 Check www-awu.aleks.com y pearson login - Yahoo Search Results Yahoo Search Results X A chemistry student weighs out 0.0878 g of phosphoric acid (H₂PO4), a triprotic acid, into a 250. mL volumetric flask and dilutes to the mark with distilled water. He plans to titrate the acid with 0.1500M NaOH solution. Calculate the volume of NaOH solution the student will need to add to reach the final equivalence point. Round your answer to 3 significant digits. C MacBook Air A ALEKS-Latoya Johnson - Le 1/3 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Acc
Use the following balanced chemical equation to answer the below question: 2H&PO4 (aq) +3Mg(OH)2 (aq) 6H2O m + Mg3(PO4)2 (s) The titration of a 14.0 mL sample of H3PO, requires 3.51 mL of 0.400 M Mg(OH)2 to reach the equivalence point. What is the concentration of H3PO,?
3. A 10.0-mL sample of aqueous NaOCl is treated with excess KI in an acidic solution. The quantity of iodine that is liberated is such that 28.02 mL of 0.0250 M 2- S,0“ solution must be added to cause the disappearance of the dark blue color due to 3 starch indicator. What is the molarity of the solution of NaOCl?