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3. An equilibrium solution was prepared by mixing 3.20 mL of 0.00200 M SCN ,5.00 mL...
How do I calculate [SCN-]i given that: Stock [Fe3+] = 0.00200 M Stock [SCN-] = 0.00200...
How do I calculate [SCN-]i given that:
Stock [Fe3+] = 0.00200 M
Stock [SCN-] = 0.00200 M
[Fe+3] [SCN]: of Table 2. Initial Data to Determine Keq Trial Volume Volume Total | Absorbance of Fe+3 volume KSCN(mm) (mm) (mL) hao 5.00 10.00 10.110 | 2 200 5.00 10.00 0.225 3 3.00 5.00 10.00 0.359 4 4.00 5.00 10.00 0.479 5 5.00 5.00 10.00 0.626 11.00×10 -3 2.00x104
4.81 mL of 0.00200 M Fe(NO3)3, 2.85 mL of 0.00200 M KSCN and 2.34 mL of...
4.81 mL of 0.00200 M Fe(NO3)3, 2.85 mL of 0.00200 M KSCN and 2.34 mL of distilled water were mixed. The resulting solution was allowed to attain equilibrium at 24 oC. The absorbance of the equilibrium solution was recorded, and the [FeSCN2+] was determined graphically to be 7.58 x 10-5 M. Part A: Calculate the number of moles of Fe3+ initially added to the solution. Part B: Calculate the number of moles of FeSCN2+ formed in the solution at equilibrium....
Prelab Question 12 (modified): If 5.00 mL of 0.00200 M Fe(NO3)3is mixed with 3.00 mL of...
Prelab Question 12 (modified): If 5.00 mL of 0.00200 M Fe(NO3)3is mixed with 3.00 mL of 0.00200 M KSCN, calculate the initial concentration of Fe3+ and SCN1-in the solution.
4. Calculate the initial concentrations of Fe3+ and SCN? in each of the equilibrium mixtures you...
4. Calculate the initial concentrations of Fe3+ and SCN? in each of the equilibrium mixtures you will prepare using the information in Table 2 Volume of delonged water (ml) Total volume ml) Table 2. Preparation of Equilibrium Mixtures Volume of Volume of Volume of 0.10 M Mixture 0.00200 M 0.00200 M HNO, (ml) KSCN (ML) Fe(NO3)3 (ml) 1,50 3.00 1.00 2.00 1.00 2.50 1.00 1.50 350 1.00 1.00 2.50 2.00 4.50 4.50 4.50 4.50 4.50 10.00 10.00 10.00 10.00 10.00...
A 25.0 mL volume of 0.0200 M Fe(NO3)3 is mixed with 50.0 mL of 0.00200 M...
A 25.0 mL volume of 0.0200 M Fe(NO3)3 is mixed with 50.0 mL of 0.00200 M NaSCN and 25.0 mL of 0.100 HNO3. The blood-red FeSCN2+ ion forms and the equilibrium is established: Fe3+(aq) + SCN-(aq) <---> FeSCN2+(aq) The equilibrium concentration of FeSCN2+ ([FeSCN2+]) was measured spectrophotometrically and found to be 7.0 x 10-4 mol/L. To calculate the equilibrium constant (Kc) for thr equilibrium system, proceed through the following steps: A. Moles of Fe3+, initial B. Moles of SCN-, initial...
For the reaction Fe3+ + SCN 1- FeSCN2+ 9.00 mL of 0.00800M Fe(NO3)3 were diluted to...
For the reaction Fe3+ + SCN 1- FeSCN2+ 9.00 mL of 0.00800M Fe(NO3)3 were diluted to a volume of 450.0 ml, then... 4.00 mL of the diluted Fe(NO3)3 were mixed with 4.00 mL of KSCN and 4.00 mL of HNO3. Calculate the initial concentration of Fe3+ at the time of mixing. Short answer LE- _ (no extra Scientific notation format spaces) How many mL of 0.00200 M Fe(NO3)3 are required to prepared 12.50 mL total volume with a concentration of...
help with calculating the “initial [SCN^—]” M and the Equilibrium [Fe(SCN^2+)] M. i have one. just...
help with calculating the “initial [SCN^—]” M and the Equilibrium
[Fe(SCN^2+)] M.
i
have one. just not sure how to set up the equation to find the
inital [SCN^-] . not sure if im calculating it correctly.
Data Manipulation and Calculations Calibration Solutions Data 1. Calculate the "Initial [SCN']" molarities for the solutions using the dilution equation CiVI=C2V2 2. Use the net ionic equation for the reaction, the ratio of [Fe3 [SCN'] used, and your knowledge of Le Châtelier's Principle...
help with finding the equilibrium of [Fe(SCN)^2+] morality value Equilibrium Solutions Data 1. Use your "Absorbance...
help with finding the equilibrium of [Fe(SCN)^2+] morality value
Equilibrium Solutions Data 1. Use your "Absorbance of Solution" values and the graph you made above to interpolate the "Equilibrium [Fe(SCN)]" molarity values. 2. Calculate both the "Initial [Fe ]" and the "Initial [SCN']" molarity values using then dilution equation CiVi C2V2. 3. Calculate the "Equilibrium [Fe ]" molarity values by subtracting the "Equilibrium [Fe(SCN) " molarity values from the "Initial [Fe'" molarity values. 4. Calculate the "Equilibrium [SCN']" molarity values...
Determination of an Equilibrium Constant 1) If 20.0 mL of 0.00200 M Fe(No3)3 is diluted to...
Determination of an Equilibrium Constant 1) If 20.0 mL of 0.00200 M Fe(No3)3 is diluted to 50.0 mL, what is the concentration of Fe^+3 in the diluted solution? 2) Write the equilibrium for the following reaction. Co^+2 +4SCN^-1 <--> Co(SCN)4 ^-2 3) How many mmoles of SCN^-1 ion are there in 3.0 mL of 0.00200 M KSCN?
Show all work to receive full credit. Express answers to the correct number of significant figures. Note: Complete...
Show all work to receive full credit. Express answers to the correct number of significant figures. Note: Complete the table below by calculating the initial SCN and equilibrium Fe(SCN)2+ concentrations for each of the five standard solutions. In addition to the volume of KSCN indicated in the table below each solution contains 5.00 mL of Fe(NO,)a and sufficient 0.050 M HNO3 to produce a total volume of 25.00 mL of solution. 1. Fe3+ +SCN Fe(SCN)2+ 0.00200 M Molarity of KSCN...
How do I calculate [SCN-]i given that:
Stock [Fe3+] = 0.00200 M
Stock [SCN-] = 0.00200 M
[Fe+3] [SCN]: of Table 2. Initial Data to Determine Keq Trial Volume Volume Total | Absorbance of Fe+3 volume KSCN(mm) (mm) (mL) hao 5.00 10.00 10.110 | 2 200 5.00 10.00 0.225 3 3.00 5.00 10.00 0.359 4 4.00 5.00 10.00 0.479 5 5.00 5.00 10.00 0.626 11.00×10 -3 2.00x104
4. Calculate the initial concentrations of Fe3+ and SCN? in each of the equilibrium mixtures you will prepare using the information in Table 2 Volume of delonged water (ml) Total volume ml) Table 2. Preparation of Equilibrium Mixtures Volume of Volume of Volume of 0.10 M Mixture 0.00200 M 0.00200 M HNO, (ml) KSCN (ML) Fe(NO3)3 (ml) 1,50 3.00 1.00 2.00 1.00 2.50 1.00 1.50 350 1.00 1.00 2.50 2.00 4.50 4.50 4.50 4.50 4.50 10.00 10.00 10.00 10.00 10.00...
For the reaction Fe3+ + SCN 1- FeSCN2+ 9.00 mL of 0.00800M Fe(NO3)3 were diluted to a volume of 450.0 ml, then... 4.00 mL of the diluted Fe(NO3)3 were mixed with 4.00 mL of KSCN and 4.00 mL of HNO3. Calculate the initial concentration of Fe3+ at the time of mixing. Short answer LE- _ (no extra Scientific notation format spaces) How many mL of 0.00200 M Fe(NO3)3 are required to prepared 12.50 mL total volume with a concentration of...
help with calculating the “initial [SCN^—]” M and the Equilibrium
[Fe(SCN^2+)] M.
i
have one. just not sure how to set up the equation to find the
inital [SCN^-] . not sure if im calculating it correctly.
Data Manipulation and Calculations Calibration Solutions Data 1. Calculate the "Initial [SCN']" molarities for the solutions using the dilution equation CiVI=C2V2 2. Use the net ionic equation for the reaction, the ratio of [Fe3 [SCN'] used, and your knowledge of Le Châtelier's Principle...
help with finding the equilibrium of [Fe(SCN)^2+] morality value
Equilibrium Solutions Data 1. Use your "Absorbance of Solution" values and the graph you made above to interpolate the "Equilibrium [Fe(SCN)]" molarity values. 2. Calculate both the "Initial [Fe ]" and the "Initial [SCN']" molarity values using then dilution equation CiVi C2V2. 3. Calculate the "Equilibrium [Fe ]" molarity values by subtracting the "Equilibrium [Fe(SCN) " molarity values from the "Initial [Fe'" molarity values. 4. Calculate the "Equilibrium [SCN']" molarity values...
Show all work to receive full credit. Express answers to the correct number of significant figures. Note: Complete the table below by calculating the initial SCN and equilibrium Fe(SCN)2+ concentrations for each of the five standard solutions. In addition to the volume of KSCN indicated in the table below each solution contains 5.00 mL of Fe(NO,)a and sufficient 0.050 M HNO3 to produce a total volume of 25.00 mL of solution. 1. Fe3+ +SCN Fe(SCN)2+ 0.00200 M Molarity of KSCN...
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