In the analysis of H2O2 using KMno the simulation first states that about 20 ml of water is added to the 1.00 mL aliquot of H,O, to make the observation of the end point easier. Later, you are informed that your assistant diluted the 1.00 mL HO2 sample to 10 mL with distilled water. Which of the following volumes is used in your analysis of the concentration of H;O2 in the original sample? 11.00 mL 10.00 mL 20.00 mL O1.00 ml. O 21.00 ml

In the analysis of H2O2 using KMno the simulation first states that about 20 ml of water is added to the 1.00 mL aliquot of H,O, to make the observation of the end point easier. Later, you are informed that your assistant diluted the 1.00 mL HO2 sample to 10 mL with distilled water. Which of the following volumes is used in your analysis of the concentration of H;O2 in the original sample? 11.00 mL 10.00 mL 20.00 mL O1.00 ml. O 21.00 ml

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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3. Analysis of a mixture consisting of NaOH + Na2CO3 + inert matter gives the following data: 10.00 g. Its aqueous solution is diluted to 250.0 mL and two separate 25.00 mL sample portions are titrated. With one portion, an end point with phenolphthalein is obtained in cold solution, with 44.52 mL of 0.5000 N HCI. The other portion requires 46.53 mL of the acid for an end point with methyl orange. Calculate the percentage composition of the original sample.
a) What mass of Fe(NH4)2(SO4)2•2H2O(s) is required to prepare a 500 mL solution containing 100 ppm (m:v) in Fe? b) Using this stock solution, what aliquot must be used to prepare calibration solutions, 100 mL volume, of the following concentrations: 0.100 ppm, 0.500 ppm, 2.00 ppm, 4.00 ppm, and 7.00 ppm.
In the analysis of H2O2 using KMnO4, the simulation first states that about 20 mL of water is added to the 1.00 mL aliquot of H2O2 to make the observation of the end point easier. Later, you are informed that your assistant diluted the 1.00 mL H2O2 sample to 10 mL with distilled water. Which of the following volumes is used in your analysis of the concentration of H2O2 in the original sample? Question 3 options: 10.00mL 20.00mL 11.00mL 21.00mL 1.00mL
A 12.63 g sample of calcium ore was dissolved in HCl and gravimetrically analyzed, through the precipitation of calcium into CaC2O4 · H2O. The precipitate was filtered, washed, dried, and ignited at 500 oC until the weight was constant, giving a final mass of 2.35 grams pure CaCO3 (100.087 g/mol). Calculate the % Calcium (40.078 g/mol) in the sample.
A fertilizer railroad car carrying 34,300 gallons of commercialaqueous ammonia (30% ammonia by mass)tips over and spills. The density of the aqueous ammoniasolution is 0.88 g>cm3. What mass of citric acid,C(OH21COOH21CH2COOH22, (which contains three acidicprotons) is required to neutralize the spill? 1 gallon = 3.785 L.
The digestion of a 0.1159 gram sample of a phosphorous-containing compound in a mixture of HNO3 and H2SO4 resulted in the formation of CO2, H2O, and H3PO4. Addition of ammonium molybdate yielded a solid having the composition (NH4)3PO4·12MoO3 (FW = 1876.3). This precipitate was filtered, washed, and dissolved in 50.00 mL of 0.2000 M NaOH: (NH4)3PO4•12MoO3(s)+26OH-(aq)->HPO42-(aq)+12MoO42-(aq)+14H2O(l)+3NH3(g) After the solution was boiled to remove the NH3, the excess NaOH was back-titrated with 14.84 mL of 0.1626 M HCl to a phenolphthalein end point. Calculate the percent phosphorous (FW = 30.9737) in the sample.
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) Describe the preparation of 1.00 L of 0.150 M KMNO: from a solid KMNO4 1. reagent. 2. . * A sodium hydroxide solution is standardized by titrating 0.8592 g of ordinary standard potassium hydrogen phthalate (204.22 g/mol) to a phenolphthalein end point, requiring 32.67 ml. What is the molarity of the NaOH solution? co,K coK + NaOH + H0 CO,H Pnim ydog phala
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(1) Careless Carlie weighed her KHP sample, but forgot to bring her report sheet along, so she recorded the mass of KHP on a paper towel. During her titration, which required 18.46 mL of base, she spilled some base on her hands. She remembered to wash her hands, but forgot about the data on the towel, and used it to dry her hands. When she went to calculate the molarity of the base, Carlie discovered that she didn’t have the mass of her KHP. Her kindhearted instructor told Carlie that her base was 0.2987 M. Calculate the mass of Carlie’s KHP sample. Show calculations (2) What mass of solid NaOH would be needed to make 645 mL of Carlie’s NaOH solution? Show calculations.