In a gravimetric chloride analysis, it was found that 0.82g AgCl and 0.80g AgCl was obtained from an unknown that had a mass of 0.3g a. What is the mass of CL in the original sample for each b. Percentage chloride in original sample for each c. Average percent chloride d. Standard deviation e. Relative standard deviation expressed as a percent
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In a gravimetric chloride analysis, it was found that 0.82g AgCl and 0.80g AgCl was obtained from an unknown that had a mass of 0.3g
a. What is the mass of CL in the original sample for each
b. Percentage chloride in original sample for each
c. Average percent chloride
d. Standard deviation
e. Relative standard deviation expressed as a percent
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- Mass of Sample Volume of KMnO, solution used in titration Equivalents of permanganate used Equivalents of iron (II) in sample Moles of iron (II) in sample Grams of Iron in Sample % Iron in Sample Average % Iron in Unknown Instructor's Grade for Precision in Part B. Sample Calculations Part B: 0.58179 0.68719 28.19 ml 31,96m6 007662 00266 2 11 nN History Bookmarks Profiles Tab Window Help 101 Chem101 C Chegg Search O Ella Enchanted Wa. O They Both Die at t. A Request to Withdr.. U Forms | Office of t. KB Viewing Your Aca.. Have Changes n. Scho Question 8.b of 8 [Tutorial: Titration stoichiometry] This question will walk you through the steps of calculating the volume of titrant required to reach the endpoint based on the volume and concentration of analyte. Consider the standardization of NaOH by titration with C HO, according to the following chemical reaction: 3 N2OH(aq) + C,H,0,(aq)= Na C,H,0,(aq) + 3 H,O(1) Step 2: Design a problem-solving strategy. Which equation will be most helpful for solving this problem? A) PV = nRT B) M,V, = M,V, C) pH = -log[H] D) M,V /n, = M,V/n, MacBook Air * ES 24 4. 23 & 2 3. 5 6. 7 8. YIs prepared by dissolving a definite weight of a substance in a definite volume. a. primary standard b. secondary standard c. standard addition d. standard sample e. standard solution
- BaSO, precipitated from a 1.800 g sample was contaminated with 9.4 mg of Ferrous sulfate and weighed a total of 314.0 mg. Calculate: a. apparent %BASO4 b. true %BaSO4help with Part B Please. 5. Compare the values of Keq for each of the five solutions: a. Are any of the values outside the sample standard deviation for the set? b. Does the value of the equilibrium constant change when the concentration of either the reactants or products is altered? Why or why not? Explain this based on your calculations of Keq: c. What caused variation (three reasons) in your values of Keq? NOTE: the standard deviation is 3.9x102 The procedure is in the images Data: Unknown solution Equilibrium concentration of {FeNCS2+} in unknown solution(M) Equilibrium concentration [Fe3+](M) Equilibrium concentration [SCN-](M) Keq 1 3.7x10-5 9.6x10-4 1.6x10-4 2.4x102 2 6.2x10-5 9.4x10-4 3.4x10-4 1.9x102 3 1.1x10-4 8.9x10-4 4.9x10-4 2.5x102 4 1.1x10-4 8.9x10-4 6.9x10-4 1.8x102 5 1.8x10-4 8.2x10-4 8.2x10-4 2.7x102Multiple Choice Each of the numbered items or incomplete statements is followed by answers or by completions of the statement. Select the one lettered answer or completion that is best in each case. Write your answer before each number. 33. Neutralization reactions in titrimetric methods of analysis may be: a. Complexomtery C. Argentimetry Mercurimetry b. Alkalimetry d. 34. The following drugs/substances is assay by direct alkalimetry EXCEPT: a. Phosphoric acid C. Soda ash b. Boric acid d. Hydrochloric acid 35.Analysis wherein the constituents of a sample are separated and then the product is weighed: a. Gravimetric C. Chromatographic b. Spectrophotometric d. Volumetric
- 1. Which among these is/are desirable properties for the type of precipitate required in gravimetric analysis? I. large particles III. known composition A. I only II. reactive with atmospheric constituents IV. small particles C. I & III В. I & II D. III & IV Е. I, П, IMultiple Choice Each of the numbered items or incomplete statements is followed by answers or by completions of the statement. Select the one lettered answer or completion that is best in each case. Write your answer before each number. 69. The presence of a cotton fiber in a liquid preparation is considered as a/an: a. Ocular defect C. d. Internal defect Critical defect b. Variable defect 70.A type of titration where the first titrant is added in excess with the sample and the second titrant reacts with the added excess is: a. Back Titration Blank Titration C. d. b. Direct Titration None of the above 71. theory attributes the change in color of indicators to certain ions an increase in which causes the appearance of a new color, and a decrease in which causes the disappearance of a color or the appearance of a different color. a. Physico-Chemical C. Lewis b. Colloidal d. Organic XTitration Experiment 1: Acid-Base Titration: Unknown HCl Write chemical equation *+ HClcags N s → Naclceg) + H,O Write NIE OH c) + HEogs → H2OC) Enter the data into the table and choose three titrations to find the molarity of the unknown HCI. Unknown # HCI Titration 1 Titration 2 Titration 3 Titration 4 Titration 5 Volume NaOH used to titrate unknown HCI solution 17.43ml 16.5O ml662 mll16.57ml16.6dmL Molarity of NaOH used for each titration 0.2564 0.1787/01692/0.1704/oiado1703 Molarity of HCI Average M HCI (avg ± standard deviation) 10.1717 1.63 % Precision Calculations 1. Provide one representative calculation that you used to determine the molarity of HCI. Be sure to show all units and use proper sig figs! V HCI-25mL MHCI =? VN2OH = 16.6lmL MNAOH=0.2564 MHCI VHCI=MNAOH VAa OH MHCI 25=O. 1564 16.61 MHCI= 0.2564.16.61 25 MHCI=0.1703 2. Average molarity of three titrations. 6.1787+0.1692+0.1704+0.1619+ O.1703 MACI= 0.117
- When we make a calibration curve, we want the range of calibration standards to the analyte concentrations in the samples. If this is not the case, we will have to the samples, depending on the analyte concentration. O Exclude, concentrate or dilute O Include, spike O Include, concentrate or dilute None of These O Exclude, calculate the concentration of You have prepared a set of calibration standards for nitrate in surface water where you are using Beer's Law to generate the calibration curve. The calibration equation for the standards you have prepared between 1 and 15 ppm is y = 0.0820x +0.00900. You analyze a 3.00 mL water sample and generate an absorbance response of 1.12. You report the concentration of nitrate in this sample as: O None of These O 4.52 ppm O The concentration is out of range so it cannot be reported O 13.5 ppm O 13.5 absorbance17. This type of analysis implies that the constituent determined was present in very, very low concentration. a. Macro analysis b. Semi-macro analysis c. Micro analysis 18. Which of the following does not happen during digestion? The crystals dissolve and re-precipitate under equilibrium conditions. b. Weakly bound water are lost from the precipitates. c. Filterability improves d. None of the choices1. A student performed this experiment and obtained the following concentration values: 0.02813 M, 0.02802, and 0.02788 M a. what is the mean concentration? b. what is the standard deviation of these results? 3. how would the following errors affect the concentration of Cl- obtained in question 2b? give your reasoning in each case. a. the student read the molarity of AgNo3 as 0.02104M instead of 0.02014M b. the student was past the endpoint of titration when he took the final buret reading.