A student determined the concentration of copper by ion exchange. He obtained the following results: (4.3810 x 10^1) mL of (9.46 x 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 NaOH used in the titration.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: \[ \text{[ ]} \times 10^{\text{[ ]}} \]Answer A student determined the concentration of copper by ion exchange. He obtained the following results: \( (2.97 \times 10^1) \) mL of \( (7.0820 \times 10^{-2}) \) 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 \( \text{H}^+ \) present in the eluate.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:**\[ \boxed{\hspace{2cm}} \times 10^{\boxed{\hspace{1cm}}} \]

Answered: Image /qna-images/answer/38eb80a6-e0c8-487b-a27d-01bfa79441a2.jpg

A student determined the concentration of copper by ion exchange. He obtained the following results: (4.3810x10^1) mL of (9.46x10^-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 NaOH used in the titration.

A student determined the concentration of copper by ion exchange. He obtained the following results: (4.3810x10^1) mL of (9.46x10^-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 NaOH used in the titration.

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

To a 25.00 mL volumetric flask, a lab technician adds a 0.100 g sample of a weak monoprotic acid, HA, and dilutes to the mark with distilled water. The technician then titrates this weak acid solution with 0.0841 M KOH. She reaches the endpoint after adding 44.65 mL of the KOH solution. Determine the number of moles of the weak acid in the solution. moles of weak acid: Determine the molar mass of the weak acid. molar mass= pKa mol After the technician adds 16.63 mL of the KOH solution, the pH of the mixture is 5.79. Determine the pK₁ of the weak acid. = g/mol
You have been provided with a 2.08 x 10-2 L sample of lithium hydroxide (LiOH) of unknown concentration. You perform a titration with 2.19 M nitric acid (HNO3), and find that 24.6 mL are required to reach the equivalence point (as determined using a coloured indicator). What is the concentration of the lithium hydroxide solution in mol L-1?
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.
Table 1: Titration Data Volume of magnesium hydroxide solution in Erlenmeyer flask Concentration of magnesium hydroxide 0.135 mol/L solution in Erlenmeyer flask Initial volume of nitric acid solution in burette Final volume of nitric acid solution in burette 10.Use the data in Table 1 to answer the folowing (a) Write the balanced chemical equatio. (b) Calculate the molar concentration of nitric acid 20.00 mL (c) Calculate the pH of the acid. 1.06 mL 23.08 mL
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
When 50.0 mL of a 0.3000 M AgNO3 solution is added to (4.65x10^1) mL of a solution of MgCl₂, an AgCl precipitate forms immediately. The precipitate is then filtered from the solution, dried, and weighed. If the recovered AgCl is found to have a mass of (1.2x10^-1) g. what was the concentration in molarity of chloride ions in the original MgCl₂ solution? 2AgNO3(aq) + MgCl₂(aq) → 2AgCl(s) + Mg(NO3)2(aq) Use the correct number of significant figures and type in the unit abbreviation for the answer. Answer: 8.0x10^-1 M.
A solution of sodium hydroxide is standardized against potassium hydrogen phthalate (molecular mass = 204.224 g mol-1). From the following data, calculate the molarity of the NaOH solution. The mass of the KHP is 0.7840 g. Before the titration the buret reading was 0.8400 mL and afterwards it was 39.20 mL. A 85.12 mL sample of a solution of sulfuric acid, H2SO4, is neutralized by 59.82 mL of the NaOH solution from the problem above. Calculate the molarity of the sulfuric acid solution.
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
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)
Sonomic acid is a monoprotic acid developed in the chemistry department of Sacramento state University. The storeroom staff successfully obtained a sample of sonomic acid and made a solution. They made the solution by adding 302.4 g of sonomic acid and diluting it to a volume of 10.00 L with water. Unfortunately, the stockroom attendant, Steven , does not know the molar mass of sonomic acid so he could not calculate the molarity of the solution he prepared. It would be great if you could help him.
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.