In this experiment, the mass of pure copper provided is 0.491 gram, and then it was dissolved in nitric acid. An ammonia solution was added into it and transferred to a 100mL volumetric flask and dilute to 100ml with distilled water. This is the original standard solution. Then a diluted solution was prepared by adding 11 mL original standard solution to a 100ml volumetric flask and diluting to 100ml with distilled water. Please calculate the copper molarity of the diluted solution.

In this experiment, the mass of pure copper provided is 0.491 gram, and then it was dissolved in nitric acid. An ammonia solution was added into it and transferred to a 100mL volumetric flask and dilute to 100ml with distilled water. This is the original standard solution. Then a diluted solution was prepared by adding 11 mL original standard solution to a 100ml volumetric flask and diluting to 100ml with distilled water. Please calculate the copper molarity of the diluted 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...

See similar textbooks

Similar questions

You are analyzing the effluent from a lotion plant for parabens using HPLC. You have a working standard solution with a concentration of 59.4 ppm which returned a Peak Height of 10,164 and Peak Area of 5,315. You take 44.4 L of the water sample and concentrate it to 0.3 L and analyze this solution. The Peak Height is 9,119 and the Peak Area is 6,320. What is the concentration of parabens in the effluent of the plant in mg/L to two decimal places.
Please send me the question in 20 minutes it's very urgent plz
The NaOH titrant in this experiment was prepared to be approximately 0.1 M and then was standardized to determine its exact concentration. What possible reasons could there be for not simply weighing the solid NaOH, dissolving to a known volume and calculating its molarity?
A. The weight of 25 tablets of morphine sulfate (150 mg) is 3.075 g. If 0.3075 g was used in the assay and it required 10.3 ml of 0.023N NaOH to back titrate 25 ml of 0.021N H2SO4. Calculate the percent labeled amount of morphine sulfate. Each ml of 1N H2SO4 is equivalent to 758.83 mg of morphine sulfate.
Saved Normal BIIIU fxl Ix Actual mass used in solution prep (g) Volume solution prepared Measured conductivity (uS/cm) Substance 0.1 g Naci 0.1003 100 mL 1149 0.1 g Nal 0.10 100 ml 419 Calculate the mass of Nal that would be necessary to yield the same conductivity as the NaCl solution. Clearly show these calculations in your lab notebook. Saved T BII U X X + fr Normal
Considering the procedure below: “Determination of the concentration of HCl: Pipette 10 mL of hydrochloric acid and transfer to a 100 mL volumetric flask, complete the volume with water and homogenize. Remove a 10 mL aliquot of this solution and transfer it to a second dilution in a 100 mL volumetric flask, complete the volume with water and homogenize. Take a 20 mL aliquot of this last solution and transfer to a 250 mL erlenmeyr and add 20 mL of distilled water and 4 drops of the acid-base indicator. Titrate with a previously standardized 0.100 mol/L sodium hydroxide solution until the indicator turns.” Answer: a) In this titration, the indicator used is phenolphthalein. Discuss the use of this indicator considering its turning range and pH at the stoichiometric point of the titration. Justify. b) Considering that the volume of titrant used was equal to 24.5 mL, calculate the concentration of HCl in the sample in mol/L.
A sample containing this BTEX was referred to the laboratory for quantitative and qualitative evaluation. What is your suggested way of working?
00 mL of a diprotic acid primary standard solution was accurately prepared to a concentration of 0.1431 M. Three samples of this primary standard solution were used as samples in a titration to standardize an aqueous solution of sodium hydroxide, NaOH, which would be used as a titrant. Using the following table of data for the titration of the primary standard acid with NaOH, calculate the average concentration of NaOH. Trial # Volume of primary standard Initial titrant volume Final titrant volume 1 10.00 mL 8.21 mL 27.22 mL 2 10.00 mL 27.22 mL 46.23 mL 3 10.00 mL 30.28 mL 49.29 mL 0.1506 M 0.0753 M 0.0376 M 0.1431 M 0.0526 M
In Purification by Recrystallization, why the solution must be filtered while hot?
DATA AND CALCULATIONS Show all calculations neatly on an attached sheet. Trial 1 Trial 2 Trial 3 70.6849. 68.0749 2.61g 23.25ML O.65ML 22.6mL Mass of flask + vinegar Mass of empty flask Mass of vinegar used Final buret reading Initial buret reading Volume of NaOH used Moles of NaOH used 0.00226 mol Moles of açetic acid titrated Mass of acetic acid titrated Mass % acetic acid in vinegar 5.0%
11. A 100.00 mL sample of orange juice, which has been fortified with calcium is titrated with 0.02357 M EDTA in the same method as this experiment. The initial buret reading is 0.15 mL and the final buret reading is 15.23 mL. How many mg of calcium are contained in the orange juice sample? Show your work. 12. What is the molarity of calcium in the orange juice sample from the above ques- tion? Show your work.
A student extracted 2.3521g of lycopene from tomato paste. The solid was placed it into a 20 ml volumetric flask and added solvent to the line. 2 ml of this solution was removed using a 2 ml volumetric pipet and placed into a 10 ml graduated cylinder and solvent was added to the 10 ml mark. What was the concentration of the dilute solution?