Question 2-A A chemist did an experiment for the determination of iron content in an iron ore. The following are the steps in the procedure: • Weighing of 1.0000 grams of sample or powdered iron ore. • Acid digestion of 1.0000 grams of iron ore by adding excess 10% of HCI. • After digestion, an excess amount of ammonia was added to form the precipitate Fe,O3. • The precipitate is filtered out and subjected to heat. Finally, the weight of precipitate was determined, and calculation is followed and the mass of Fe in the sample is 0.3587 grams. Consider the following statement: Statement I: The experiment is a classical-volumetric method of analysis. Statement II: The experiment is a macroanalysis based on the amount of sample. Statement III: The experiment is a minor analysis based on the amount of analyte. Which of the following option is correct? O A. Statement I is correct and statement Il and II are incorrect B. Statement Il is correct and statement I and II are incorrect OC. Statement I and Il are correct and statement II is incorrect D. Statement Il and IIl are correct and statement I is incorrect O E. Statement I, II, and III are correct

Question 2-A A chemist did an experiment for the determination of iron content in an iron ore. The following are the steps in the procedure: • Weighing of 1.0000 grams of sample or powdered iron ore. • Acid digestion of 1.0000 grams of iron ore by adding excess 10% of HCI. • After digestion, an excess amount of ammonia was added to form the precipitate Fe,O3. • The precipitate is filtered out and subjected to heat. Finally, the weight of precipitate was determined, and calculation is followed and the mass of Fe in the sample is 0.3587 grams. Consider the following statement: Statement I: The experiment is a classical-volumetric method of analysis. Statement II: The experiment is a macroanalysis based on the amount of sample. Statement III: The experiment is a minor analysis based on the amount of analyte. Which of the following option is correct? O A. Statement I is correct and statement Il and II are incorrect B. Statement Il is correct and statement I and II are incorrect OC. Statement I and Il are correct and statement II is incorrect D. Statement Il and IIl are correct and statement I is incorrect O E. Statement I, II, and III are correct

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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O Microsoft O shift V A chemistry student weighs out 0.0608 g of formic acid (HCHO₂) into a 250. mL volumetric flask and dilutes to the mark with distilled water. He plans to titrate the acid with 0.1400M NaOH solution. OCHEMICAL REACTIONS Determining the volume of base needed to titrate a given mass... Calculate the volume of NaOH solution the student will need to add to reach the equivalence point. Be sure your answer has the correct number of significant digits. W Microsoft Microsoft 6.52.210... tab esc caps lock mL control Explanation ! 1 (8) Q A Check N © 2 W S #3 X T option command E x10 X D NOV 14 $ 4 C R S F do L % 5 V T G tv ♫ 6 MacBook Pro 9 Y & 7 H Ⓒ2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility U 8 1 9 BN M A O J K O O JOD 05 L H W P > { I command option DOCX + 11 ? | 1 9 OC
You have an unknown solution and you want to determine if it contains ammonia. How will you detect its presence in the laboratory analysis? Please provide two ways to analyze its presence and explain your chosen technique in determining the ammonia.
[Review Topics] [References] Be sure to specify states such as (aq) or (s). If a box is not needed leave it blank. The following molecular equation represents the reaction that occurs when aqueous solutions of silver(I) nitrate and iron(III) iodide are combined. 3AGNO3 (aq) + Fel3 (aq) →3AgI (s) + Fe(NO3)3 (aq) Write the balanced net ionic equation for the reaction. + + Submit Answer Retry Entire Group 4 more group attempts remaining Previous Next Save and Exi Email Instructor
You have aqueous solutions of Ag* and PO43- that have equal concentrations. You mix them according to the following table: Test Tube # Number of drops Ag Number of drops PO4³- 01 0 4 2 1 3 3 9 2 t 8 3 6 4 Assuming the product of the reaction is insoluble, which test tube will contain the most. precipitate? 8 5 9 3
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A Ba(OH)2 solution was standardized against potassium hydrogen phthalate (KHP). The titration of 0.4513 g of KHP required 26.50 mL of the solution. Calculate the molarity of the barium hydroxide solution. Establish your stoichiometric ratio. Calculate the mole of Ba(OH), from the titration values and the stoich ratio. Solve for molarity.
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Jack was asked to determine iron (55.845 g/mol) content in dietary supplement. He tookfew random tablets and ground them into fine powder. Next, he weighed 3.116 g of thefine powder. Sample was dissolved and iron was precipitated as Fe(OH)3 (106.867 g/mol).The precipitate was then ignited to a constant weight of 0.355 g as Fe2O3 (159.69 g/mol).Report the iron content in dietary supplement as % w/w FeSO4·7H2O (278.01 g/mol).
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