Standardization Answer the concentrations in 3 significant figure. The tolerance or error should follow the decimal place of the value. You can use scientific notation using "e". Example: 0.0010 = 1.0e-3 Primary Standard: Na2CO3 Formula Mass of 1º Standard: 105.99 g/mol Purity of 1º Standard: 95% Instrument used: Analytical Balance Trial 1⁰ Standard weight, g Net vol. of HCI, mL M HCI of Hydrochloric Acid Solution Average M HCI 1 0.0504 + 0.0002 ± 2 0.0510 (same as 1) 18.00 ± 0.14 18.30 ± 0.14 17.90 +0.14 ± 3 1+ 0.0501 (same as 1) ±

Standardization Answer the concentrations in 3 significant figure. The tolerance or error should follow the decimal place of the value. You can use scientific notation using "e". Example: 0.0010 = 1.0e-3 Primary Standard: Na2CO3 Formula Mass of 1º Standard: 105.99 g/mol Purity of 1º Standard: 95% Instrument used: Analytical Balance Trial 1⁰ Standard weight, g Net vol. of HCI, mL M HCI of Hydrochloric Acid Solution Average M HCI 1 0.0504 + 0.0002 ± 2 0.0510 (same as 1) 18.00 ± 0.14 18.30 ± 0.14 17.90 +0.14 ± 3 1+ 0.0501 (same as 1) ±

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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ame: Table 2. Determination of Acetylsalicylic Acid in Aspirin. 1) Aspirin Brand (and amount of acetylsalicylic acid on label) 2) Average molar concentration of NaOH Solution B (from Part A) 3) 4) 5) 6) Mass of aspirin tablet Mass of pulverized aspirin sample Initial buret reading Final buret reading 7) Volume of NaOH Solution B added 8) Moles of NaOH 9) Moles of acetylsalicylic acid in sample 10) Mass of acetylsalicylic acid in sample 11) Amount of acetylsalicylic acid per tablet T₁ 1.264 12) Mean amount of acetylsalicylic acid per tablet 13) Standard deviation for acetylsalicylic acid per tablet 14) RSD for acetylsalicylic acid per tablet 15) Relative percent error (%) 16) Is the mean amount per tablet acceptable? (Yes or no.) 0.000153 * 180. Kg Imol T₂ √3 1.261 1-259 Seat กา Basic 8.25 mg 0.0975 M Trial 1* Trial 2 *Show all calculations related to Trial 1, standard deviation, RSD, and relative % error. Mole of NaOH (0.0975) (14.3) = 0.000139 (0.0975) (15.7) = 8.000 253 23 0.0975)…
4.00 mL of a 7.20 x 10-4 M solution of an unknown acid is diluted with 6.00 mL of hexane, forming solution X. Then 3.00 mL of solution X is diluted with 7.00 x 10-3 L of hexane, forming solution Y. Then 2.00 x 10-3 L of solution Y is diluted with 8.00 mL of hexane, forming solution Z. How many grams of unknown acid are 4.00 mL of solution Z? (Molar mass for unknown acid = 345 g/mol) Select one: O a. 2.38 x 10-5g O b. 5.08 x 10-6g Oc. 2.03 x 102g O d. 1.02 x 10g O e. 5.08 x 104g
A student sets up the following equation to solve a problem in solution stoichiometry. (The ? stands for a number the student is going to calculate.) Enter the units of the student's answer. I'm confused on what the next step is from here. I dont know if I need to switch the 10-3 to the bottom to make the 103 and how would I solve the problem from here?
A student performed an 3. experiment to determine the solubility of KCL The following data was collected: Mass of empty 250-mL beaker = 105.6 g Mass of the 250-mL beaker and the saturated KCI solution=110.lg Mass of the 250-mL beaker and the KCl residue (after heating) = 106.9 g Use the above data to determine: a) The solubility of KCl as mass percent of solute b) The solubility of KCl as mass of KCI per 100 mL of water
The unknown metal ion gave a red/orange flame test and precipitate with ammonium carbonate, What is the unknown metal? Type just the symbol of the metal ion with no charge included. For example, iron ion would be Fe. ORAD WOITAMAO RETOV STRATOV J30 WOIDAMAOR 80 ATBLAAT ith Your Answer: x10 MacBook Air DD 80 888 F7 F8 F9 F10 F5 F6 F1 F2 F3 F4 & ! @ #3 $ 1 3 7 8 9 Q W E R Y A S D F H J K > CV B
What volume (in mL) of 30.0% hydrogen peroxide solution is required to provide the mass required in question 8 above? Mass=10.2g of a 30% hydrogen peroxide soltuion. Density of 30.0% H2O2 = 1.11 g/mL Answer with 3 sig figs.
Question 10 of 26 Submit How many mililiters of water should a chemist add if they want to prepare an 0.200 M aqueous solution with 30.2 g of NaCI ? Assume the density of the resulting solution is the same as the water. STARTING AMOUNT ADD FACTOR ANSWER RESET *( ) 2580 22.99 2.58 0.200 0.517 151 1 0.001 1000 58.44 6.022 x 1023 30.2 1.51 x 105 mL g NaCl/mol mol NaCl M NaCI L g NaCI +
More Practice 5.2 - Enhanced - with Feedback 5 of 5 I Review I Constants I Periodic Ta Part A What volume, in milliliters, of a 0.125 M solution of KCl contains 2.80 g of the compound? Express the volume to three significant figures and include the appropriate units. Value ml volume = Submit Previous Answers Request Answer X Incorrect; Try Again; 2 attempts remaining To determine the volume of solution that contains 2.80 g of KCI, calculate the number of moles of KCI in the given mass. Then convert the number of moles of KCl to the corresponding solution volume using the molarity, and report the volume in the appropriate units. Recall that 1 L = 1000 mL. < Return to Assignment Provide Feedback NOV 21
(Incorrect) In order to prepare very dilute solutions, a lab technician chooses to perform a series of dilutions instead of measuring a very small mass. A solution was prepared by dissolving 0.360 g of KNO3 in enough water to make 500. mL of solution. A 10.0 mL sample of this solution was transferred to a 500.0-mL volumetric flask and diluted to the mark with water. Then 10.0 mL of the diluted solution was transferred to a 250.0-ml flask and diluted to the mark with water. What is the final concentration of the KNO3 solution? 7.12 x 103 M (Your answer) 2.85 × 10-6 M 7.91 × 10-⁹ M 5.70 x 106 M (Correct answer) 1.42 × 10-4 M
Current Attempt in Progress A 66.7 ml sample of 18.0 M sulfuric acid was diluted with enough water in a volumetric flask to make 5.00 x 102 mL of solution, A 25.0 mL aliquot of this solution was then further diluted to a volume of 1.50x 102 mL. What is the molarity of the solution after the second dilution? M e Textbook and Media Hint Save for Later Attempts: 0 of 2 used Submit Answer pe here to search 2/ Cop 10 insert prt sc $ 4 %23 % & 3 8 %\ RI T. U D G H. pause alt ctrl B
[References] A solution is prepared by dissolving 16.2 g ammonium sulfate in enough water to make 260.0 mL of stock solution. A 35.00-mL sample of this stock solution is added to 60.00 mL of water. Calculate the concentration of ammonium ions and sulfate ions in the final solution. Assume that the volumes are additive. Concentration of ammonium ions = Concentration of sulfate ions = M Suhmit Answer Toy Another Version
Part D Find the number of moles of water that can be formed if you have 114 mol of hydrogen gas and 52 mol of oxygen gas. Express your answer with the appropriate units. • View Available Hint(s) Value Units Submit Part A 1.4 L of a 2.50 MHNO, solution is added to water so that the final volume is 7.0 L. Express your answer to two significant figures and include the appropriate units. ? Value Units Submit Previous Answers Request Answer nta amainina Part B Water is added to 0.50 L of a 8.1 M NaF solution to make 2.0 L of a diluted NaF solution. Express your answer to two significant figures and include the appropriate units. HẢ Value Units Submit Request Answer