Homework Answers
As per HOMEWORKLIB POLICY, I can answer only 1 question completely:
6) As Hydrochloric Acid is a very strong acid, we assume its 100% dissociation into H+ and Cl- ions.
We have the formula:
pH = -log[H+]
Here because of full dissociation, [H+]= [HCl] = 0.09M
So,
pH = -log(0.09)
= 1.045(Answer)
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Canvas +→ COD cuvet Question 11 25 pts A reaction mixture of 4.00 mL of 0.00200...
Name:. Date: Lab Section: 4. The blank solution used to calibrate the spectrophotometer is 5.0 mL...
Name:. Date: Lab Section: 4. The blank solution used to calibrate the spectrophotometer is 5.0 mL of 0.2 M Fe(NO)) diluted to 50 mt with H:O Why is this solution preferred to simply using de-ionized water for the calibration? Te celibutoneans ser He astanat os errors-free Te deionized woser alane sho no abtorpton 5. A reaction mixture of 4.00 mL. of 0.00200 M SCN and 5.00 mL of 0.00200 M Fe is uoreangth diluted to 10.00 mL with 0.1 M...
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....
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...
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?
1. You prepare a mixture to use to create a colorimetry calibration curve for FeSCN2+ by...
1. You prepare a mixture to use to create a colorimetry calibration curve for FeSCN2+ by mixing these things in a 25.00 mL volumetric flask and then diluting to the volume of the flask with 0.3 M HNO3. 5.00 mL 0.00200 M NaSCN 10.00 mL 0.30 M Fe(NO3)3 What is the concentration of FeSCN2+ in this mixture? [Pay attention to the values to determine which reactant is being driven to completely react...] 2. You prepare a mixture to use to...
Consider the following: A student mixes 5.00 mL 2.00 × 10−3 M Fe(NO3)3 with 3.00 mL...
Consider the following: A student mixes 5.00 mL 2.00 × 10−3 M Fe(NO3)3 with 3.00 mL 2.00 × 10−3 M KSCN. She finds that in the equilibrium mixture the concentration of FeSCN2+ is 1.28 × 10−4 M. Find Kc for the reaction Fe3+(aq) + SCN−(aq) ↔ FeSCN2+(aq). a. What is the initial concentration of Fe3+ in the reaction mixture? [Fe3+] = ___ x 10-3 M b. What is the initial concentration of SCN- in the reaction mixture? [SCN-] = ___...
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...
5. In this experiment, you will prepare a standard solution for a calibration curve for the...
5. In this experiment, you will prepare a standard solution for a calibration curve for the formation of FeSCN2 complex by reaction different volumes of 0.2 M Fe(NO,), and 0.002 M NaSCN. You will use 0.05M HNO, for all dilutions. Using the table, Calculate the equilibrium concentrations of FeSCN2 Vol of Fe Vol of SCN 0.1 M HNO Equilibrium concentration Fe[SCN]2' (mL) (mL.) (mL) 10.00 0.00 10.00 10.00 1.00 9.00 10.00 2.00 8.00 10.00 3.00 7.00 10.00 4.00 6.00 10.00...
2.) Explain why the concentration of Fe(SCN)2+ is equal to the intial concentration of the SCN- f...
2.) Explain why the concentration of Fe(SCN)2+ is equal to the
intial concentration of the SCN- for each solution in part A?
3.) also!!
thank you!!! :)
Post-Lab Questions: A solution is made by mixing 5.00 ml. of 0.00300 M Fe(NO,)s with 4.00 mL. of 0.00300 M KSCN and 3.00 mL. of 1.0 MHNO,. After equilibrium is established, the concentration Fe(SCN)P was determined to be 2.72 x 10* M. Calculate the value of the equilibrium constant for the reaction. Fe...
4. When 5.00 mL of 0.500 M Fe (NO3)3 are mixed with 5.00 mL of 0.250...
4. When 5.00 mL of 0.500 M Fe (NO3)3 are mixed with 5.00 mL of 0.250 M NaSCN, the following reaction occurs: Fe3+ (aq) + SCN(aq) $ FeSCN2+(aq) At equilibrium the concentration of FeSCN2- is found to be 6.00 x 10-2 M. A. Fill in the table below with the proper numerical values. (Remember to take into account the effects of dilution when calculating the initial molarity of Fe3+ (aq) and SCN'(aq) Fes- (aq) SCN (aq) FeSCN-(aq) Initial Molarity Change...
Name:. Date: Lab Section: 4. The blank solution used to calibrate the spectrophotometer is 5.0 mL of 0.2 M Fe(NO)) diluted to 50 mt with H:O Why is this solution preferred to simply using de-ionized water for the calibration? Te celibutoneans ser He astanat os errors-free Te deionized woser alane sho no abtorpton 5. A reaction mixture of 4.00 mL. of 0.00200 M SCN and 5.00 mL of 0.00200 M Fe is uoreangth diluted to 10.00 mL with 0.1 M...
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...
5. In this experiment, you will prepare a standard solution for a calibration curve for the formation of FeSCN2 complex by reaction different volumes of 0.2 M Fe(NO,), and 0.002 M NaSCN. You will use 0.05M HNO, for all dilutions. Using the table, Calculate the equilibrium concentrations of FeSCN2 Vol of Fe Vol of SCN 0.1 M HNO Equilibrium concentration Fe[SCN]2' (mL) (mL.) (mL) 10.00 0.00 10.00 10.00 1.00 9.00 10.00 2.00 8.00 10.00 3.00 7.00 10.00 4.00 6.00 10.00...
2.) Explain why the concentration of Fe(SCN)2+ is equal to the
intial concentration of the SCN- for each solution in part A?
3.) also!!
thank you!!! :)
Post-Lab Questions: A solution is made by mixing 5.00 ml. of 0.00300 M Fe(NO,)s with 4.00 mL. of 0.00300 M KSCN and 3.00 mL. of 1.0 MHNO,. After equilibrium is established, the concentration Fe(SCN)P was determined to be 2.72 x 10* M. Calculate the value of the equilibrium constant for the reaction. Fe...
4. When 5.00 mL of 0.500 M Fe (NO3)3 are mixed with 5.00 mL of 0.250 M NaSCN, the following reaction occurs: Fe3+ (aq) + SCN(aq) $ FeSCN2+(aq) At equilibrium the concentration of FeSCN2- is found to be 6.00 x 10-2 M. A. Fill in the table below with the proper numerical values. (Remember to take into account the effects of dilution when calculating the initial molarity of Fe3+ (aq) and SCN'(aq) Fes- (aq) SCN (aq) FeSCN-(aq) Initial Molarity Change...
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