During lab, a student used a Mohr pipet to add the following solutions into a 25 mL volumetric flask. They calculated the final volumes added, which are recorded below. The student then followed the directions in the manual to make the stock solution. Volumes Used to Create Stock Solution Volume 0.200 M Fe(NO3)3 (mL) Volume 0.00200 M KSCN (mL) 2.83 mL Stock Solution 8.57 mL Using the stock solution above, the student made additional dilutions, with the final volumes below. Calculate the concentration of iron(III) thiocyanate ion in Standard 2. For grading purposes, report your answer in mM with four places after the decimal. Volumes Used to Create Standard Solutions Solution Volume Stock solution (mL) Volume Water (mL) Standard 1 Standard 2 Standard 3 Standard 4 6.96 5.04 3.14 0.90 3.26 5.22 7.41 8.83

During lab, a student used a Mohr pipet to add the following solutions into a 25 mL volumetric flask. They calculated the final volumes added, which are recorded below. The student then followed the directions in the manual to make the stock solution. Volumes Used to Create Stock Solution Volume 0.200 M Fe(NO3)3 (mL) Volume 0.00200 M KSCN (mL) 2.83 mL Stock Solution 8.57 mL Using the stock solution above, the student made additional dilutions, with the final volumes below. Calculate the concentration of iron(III) thiocyanate ion in Standard 2. For grading purposes, report your answer in mM with four places after the decimal. Volumes Used to Create Standard Solutions Solution Volume Stock solution (mL) Volume Water (mL) Standard 1 Standard 2 Standard 3 Standard 4 6.96 5.04 3.14 0.90 3.26 5.22 7.41 8.83

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 measured the mass of an empty micropicnometer to be 2.000g. A student places 0.500mL of citric acid solution into a micropicnometer. The student reweighed the micropicnometer and found the mass of the citric acid solution and micropicnometer to be 2.525g. A student titrates 0.101mL of citric acid solution using the standardized 0.1M solution (use the exact concentration calculated from the previous titration problem). The sample required 0.819mL of NaOH solution to reach the end point. Given the following chemical equation. NaOH + H3C6H5O7 → Na+ + H2O + C6H5O73- Given the above information. Calculate the mass of citric acid in the 0.101mL citric acid solution. Given the above information. Calculate the total mass of the 0.101mL citric acid solution.
How can we find the volume for both questions?
A solution is prepared by dissolving 24.5 g of CaCl2 (MW = 110.98 g/mol) in 355 mL of water. The density of the resulting solution is 1.05 g/mL. The concentration of CaCl2 in this solution is ________ molar.
Use the following information to answer the next three questions Electrowinning of Copper Battery Thin sheet of pure copper (Cathode) Thick block of impure Cu (Anode) - Tank Cu2+ Acidified copper sulphate solution (Electrolyte) Cu2+ Impurities (Anode mud) The cell shown above is used to purify copper. At one electrode, impure copper is converted into copper(II) ions, which are later converted into copper solid of high purity at the other electrode. 6. The plating of pure copper will occur at the cathode where oxidation occurs. O cathode where reduction occ occurs. O anode where reduction occurs. O anode where oxidation occurs. 7. During the operation of this cell O the total energy of the system decreases. O the pH of the electrolyte increases. O the predicted net cell potential is 0.00 V.
Please do not round values until the end. The final answer should be in 3 significant figures. Thank you!
Question 12
What is the concentration of FeSCN2+ in each standard solution? (Show ALL calculations for each solution) Stock Solution of the concentration of FeSCN^2+ is 0.00200 M
4) did i do this right?
Calculate the total concentration of ions after mixing Solution 1 and Solution 2 together; with the compositions described in the table below. Solution label Salt Concentration (M) Volume (mL) Solution 1 KF 0.500 1000 Solution 2 Fe2(SO4)3 0.750 350 a. 0.759 M b. 0.954 M c. 1.25 M d. 1.71 M e. 3.52 M
A solution is initially 0.10 M in Mg2*(aq) and 0.10 M in Fe2* Mg(OH)2 first precipitates? Ksp (Mg(OH)2) = 6.0 x 10-10; Ksp(Fe(OH)2) = 7.9 x 10-16 your answer in E-notation, rounded to 2 significant digits. *(aq). A solution of NaOH is slowly added. What is the concentration of Fe2+ when %3D Provide
- Part C Write a balanced ionic equation for this acid-base reaction: Ca(OH)2 (aq) + 2CH3CO₂H(aq) → Express your answer as a chemical equation. Identify all of the phases in your answer. ΑΣΦ A chemical reaction does not occur for this question. Submit Request Answer Part D ? Write net ionic equation for this acid-base reaction: Ca(OH)2 (aq) + 2CH3CO₂H(aq) → Express your answer as a chemical equation. Identify all of the phases in your answer.
If the initial volume reading for the first titration was 0.16 mL and the final volume reading was 11.68 mL, what volume of iodine solution was used in your first titration (in mL)? Include the unit in your answer and two decimal places in your answer.