A student determined the concentration of copper by ion exchange. He obtained the following results: \( (4.68 \times 10^1) \) mL of \( (9.7770 \times 10^{-2}) \) M NaOH solution was required to titrate the eluate (HCl solution) from the column. He used a 15.0 mL sample of copper chloride solution initially.Calculate the number of moles of Cu\(^{+2}\) that were absorbed by the column.Your answer should be in correct scientific notation (that is what the red text in BrightSpace means.)**Note:** Your answer is assumed to be reduced to the highest power possible.Your Answer: [________] x 10^[________] Answer A student determined the concentration of copper by ion exchange. He obtained the following results: \(4.2180 \times 10^1\) mL of \(9.64 \times 10^{-2}\) M NaOH solution was required to titrate the eluate (HCl solution) from the column. He used a 15.0 mL sample of copper chloride solution initially.Calculate the concentration of \( \text{Cu}^{2+} \) in the original solution.Your answer should be in correct scientific notation (that is what the red text in BrightSpace means).**Note:** Your answer is assumed to be reduced to the highest power possible.**Your Answer:**[Input Box] x10 [Input Box]Answer

Answered: Image /qna-images/answer/7c5c7124-8fe0-4c3e-a7f5-e19e3ed3cacc.jpg

A student determined the concentration of copper by ion exchange. He obtained the following results: (4.68x10^1) mL of (9.7770x10^-2) M NaOH solution was required to titrate the eluate (HCI solution) from the column. He used a 15.0 mL sample of copper chloride solution initially. Calculate the number of moles of Cu*2 that were absorbed by the column. Your answer should be in correct scientific notation (that is what the red text in BrightSpace means.) Note: Your answer is assumed to be reduced to the highest power possible. Your Answer:

A student determined the concentration of copper by ion exchange. He obtained the following results: (4.68x10^1) mL of (9.7770x10^-2) M NaOH solution was required to titrate the eluate (HCI solution) from the column. He used a 15.0 mL sample of copper chloride solution initially. Calculate the number of moles of Cu*2 that were absorbed by the column. Your answer should be in correct scientific notation (that is what the red text in BrightSpace means.) Note: Your answer is assumed to be reduced to the highest power possible. Your Answer:

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

A student determined the concentration of copper by ion exchange. He obtained the following results: 37.62 mL of 0.0859 M NaOH solution was required to titrate the eluate (HCl solution) from the column. He used 15.0 mL sample of copper chloride solution initially. Calculate the number of moles of NaOH used in the titration.
An analytical chemist weighs out 0.185 g of an unknown monoprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. She then titrates this solution with 0.2000 M NAOH solution. When the titration reaches the equivalence point, the chemist finds she has added 9.5 mL of NaOH solution. Calculate the molar mass of the unknown acid. Be sure your answer has the correct number of significant digits. g x10 mol
You are preparing standard acid and base solutions for the laboratory, using potassium hydrogen phthalate (KHC₈H₄O₄, abbreviated KHP) as the primary standard. KHP (molar mass = 204.22 g/mol) has one acidic hydrogen. You prepared solutions of both NaOH and HCl. It took 22.65 mL of the NaOH solution to titrate (react exactly with) 1.55 g KHP. It then took 32.35 mL of HCl solution to titrate 25.00 mL of the NaOH solution. What is the molarity of the HCl solution?
A chemistry student needs to standardize a fresh solution of sodium hydroxide. She carefully weighs out 51 mg of oxalic acid (H2C2O4), a diprotic acid that can be purchased inexpensively in high purity, and dissolves it in 250 mL of distilled water. The student then titrates the oxalic acid solution with her sodium hydroxide solution. When the titration reaches the equivalence point, the student finds she has used 19.2 mL of sodium hydroxide solution. Calculate the molarity of the student's sodium hydroxide solution.
A science teacher needs to determine the concentration of an old, unmarked bottle of hydrochloric acid. She prepares a base titrant by dissolving 40.0 g of potassium hydroxide in 500.0 mL of water. The base is pipetted into a 28.00 mL sample of the acid, which also contains phenolphthalein as an indicator. The solution turns from clear to pink after the addition of 7.34 mL of base. What is the concentration of the hydrochloric acid?
A 10.00 ml sample of a solution of hydrofluoric acid, HF, is diluted to 500.00 ml. A 20.00 ml aliquot of the diluted solution requires 13.51 ml of a 0.1500 M NaOH solution to be titrated to the equivalence point. What is the normality of the original HF solution? HF+OH → F + H₂O
In a lab, you diluted a sample of bleach to 1/10 concentration in a 250 volumetric flask. Then quantitatively transferred 25 ml of the 1/10 concentration diluted bleach into a beaker and titrated it with a standard sodium thiosulfate solution that has a molarity of 0.1215M. You repeated this 3 times. The data below is the amount of sodium thiosulfate that was titrated in the 3 runs. Calculate the molarity in each run of the diluted bleach and the concentration of undiluted bleach sample. Titration 1: 45.55 ml Titration 2: 45.67 ml Titration 6: 45.58 ml
Determining the volume of base needed to titrate a given mass of acid.
You want to determine the % of an acetic acid sample solution by acid/base titration. Therefore, you prepare a NaOH solution. To determine the exact concentration of this NaOH you titrate exactly 390.3 mg KHPhthalate (M = 204.22 g/mol) with this NaOH solution requiring 8.2 ml. Subsequently you use this NaOH solution to titrate 25.0 ml of your acetic acid sample (M(acetic acid)=60.05 g/mol, density of solution 1 g/ml) resulting in a consumption of 6.9 ml of the NaOH solution. = Please give all relevant reaction equations (with correct stoichiometry). Calculate the exact concentration (in mol/L) of the NaOH solution. Please calculate the weight-% of acetic acid in the sample solution. Which indicator would you use for this titration/at which pH range would you expect the equivalence point? (8)
A chemistry student needs to standardize a fresh solution of sodium hydroxide. He carefully weighs out 79. mg of oxalic acid (H,C,0,), a diprotic acid that can be purchased inexpensively in high purity, and dissolves it in 250. mL of distilled water. The student then titrates the oxalic acid solution with his sodium hydroxide solution. When the titration reaches the equivalence point, the student finds he has used 23.0 mL of sodium hydroxide solution. Calculate the molarity of the student's sodium hydroxide solution. Be sure your answer has the correct number of significant digits.
A student determined the concentration of copper by ion exchange. He obtained the following results: 28.61 mL of 0.0810 M NaOH solution was required to titrate the eluate (HCl solution) from the column. He used 15.0 mL sample of copper chloride solution initially. Calculate the number of moles of H+ present in the eluate.
The iodine contained in every one mL of the 0.010 M iodine solution in the buret will react with 1.76 mg of vitamin C. (In other words, every mL of iodine solution needed for the titration indicates the presence of 1.76 mg of vitamin C in the juice sample.) If your titration used 5.86 mL of iodine solution, what mass of vitamin C is in your fruit juice sample (in milligrams, mg)?