Calculate the initial concentration of iron(III) in solution #1, #2, #3. Beaker (mL) Table 1. Reagent...

Question

Question

Calculate the initial concentration of iron(III) in solution #1, #2, #3.

Beaker (mL) Table 1. Reagent Solutions Provided by the Stockroom Solution Name Reagent [Reagent] (M) Volume (mL) Standard iro Worksheet 1 #1 5.00 #2 10.00 #3 15.00 Dilute iron (mL) [Fe**] (M) [Fe(SCN)?*] (M) %T 480 58.9 35.8 21.5 A480 from slope E480

A. Preparation of the Dilute Iron Solution In addition to the standard iron provided by the stockroom, you need a “Dilute Iro

CALCULATIONS A. Concentration of Fe3+ in the Dilute Iron The concentration of Fe(NO3)3 in dilute iron is about 1.25 x 10-6 M. Determination of Ke Data Concentration 2.50E-03 Solution Standard iron Dilute iron nitric acid Conc. SCN Dilute SCN Reagent F

science chemistry

Add a comment Improve this question Transcribed image text

Answer 1

Similar Homework Help Questions

Calculate the initial concentration of Fe3+ in test tubes 1-4. (you will need to take the...

Calculate the initial concentration of Fe3+ in test tubes 1-4. (you will need to take the dilution in to account) Calculate the initial concentration of SCN-in each of test tubes 1-4. (you will need to take the dilution in to account) 2. Label four 20 x 150 mm test tubes 1-4. Pour about 30 mL of 0.0020 M Fe(NO3)3 into a clean, dry 100-ml beaker. Pipet 5.0 mL of this solution into each of the four labeled test tubes. Use...
Part A of lab: pour 30 ml of 0.150 M Fe(NO3)3 into a 50 ml beaker...

Part A of lab: pour 30 ml of 0.150 M Fe(NO3)3 into a 50 ml beaker and pipette 10 ml of this solution into a 25 ml volumetric flask. This is the standard reagent blank Part B of lab: pour 30 ml of 1.50*10^-3 M Fe(NO3)3 into a 25 ml volumetric flask. This is the reagent blank. Why is a large excess of Fe3+ added to make the standard solution, and why do you NOT add a large excess of...
In a dilute nitric acid solution, Fe3+ reacts with thiocyanate ion (SCN−) to form a dark...

In a dilute nitric acid solution, Fe3+ reacts with thiocyanate ion (SCN−) to form a dark red complex: [Fe(H2O)6]3+ + SCN− ⇌ H2O + [Fe(H2O)5NCS]2+ The equilibrium concentration of [Fe(H2O)5NCS]2+ may be determined by how dark the colored solution is (measured by a spectrometer). In one such experiment, 1.0 mL of 0.20 M Fe(NO3)3 was mixed with 1.0 mL of 9.2 ×10−3M KSCN and 8.0 mL of dilute HNO3. The color of the solution quantitively indicated that the [Fe(H2O)5NCS]2+ concentration was...

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...
3. Experimental Procedure, Part A.1. For preparing a set of standard solutions of FeNCS, the equilibrium...

3. Experimental Procedure, Part A.1. For preparing a set of standard solutions of FeNCS, the equilibrium molar con- centration of FeNCS is assumed to equal the initial molar concentration of the SCN in the reaction mixture. Why is this assumption valid? A. A Set of Standard Solutions to Establish a The set of standard solutions is used to determine the absorbance of known molar con- centrations of FeNCS2. A plot of the data, known as a calibration curve, is used...
(10 pts) The iron content of a well water sample is determined by UV-Vis spectroscopy. A...

(10 pts) The iron content of a well water sample is determined by UV-Vis spectroscopy. A 10.00 mL aliquot of well water is transferred to a 100.0-mL volumetric flask and 20 mL of 0.10 M nitric acid is added to oxidize iron (II) to iron (II). Next 30 mL of a 0.1 M sodium thiocyanate solution is added to form the deep red complex iron (II) thiocyanate. The solution is diluted to volume with DI water. A reagent blank is...

Calculate initial concentration of Fe+3 for tubes 1-3. Show your work. Procedure A. Determination of B...

Calculate initial concentration of Fe+3 for tubes 1-3. Show your work. Procedure A. Determination of B for Beer's Law 1. Using a buret, add 4.00 mL of 0.0025 M Fe(NO3)s (which is in 0.1 M HNOs) to a 100- mL volumetric flask. Add enough deionized water to bring the total volume to the mark on the neck of the flask. Stopper and shake the flask. Label this flask “Diluted Fe.” spectrophotometer tubes (cuvettes), they are too small to use at...
How do I find the concentration of KSCN & FeSCN2+ from the following data? Solution Beaker...

How do I find the concentration of KSCN & FeSCN2+ from the following data? Solution Beaker 1 Beaker 2 Beaker 3 Beaker 4 Beaker 5 Volume of 0.200 M Fe(NO3)3. mL 2.5 mL 2.5 mL 2.5 mL 2.5 mL 2.5 mL Volume of 0.0020 M KSCN, mL .50 mL .75 mL 1.0 mL 1.25 mL 1.5 mL Volume of 0.50 M HNO3, mL 7 mL 6.75 mL 6.5 mL 6.25 mL 6 mL Total volume, mL 10 mL 10 mL...
Question 13 of 13> Attempt 1 A standard solution of FeSCN2+ is prepared by combining 9.0...

Question 13 of 13> Attempt 1 A standard solution of FeSCN2+ is prepared by combining 9.0 ml of 0.20 M Fe(NO) with I.0 mL of 0.0020 M KSCN. The standard solution had an absorbance of 0.540. Fe* (ag)+SCN (ag)FeSCN*(a) A trial solution was made in a similar manner, but with a more dilute Fe(NO,), reagent. The initial SCN" concentration. immediately after mixing, was 0.00060 M. This trial solution had absorbance of 0.250. What is the equilibrium concentration of SCN in...

As described in part A of the lab, you are preparing a solution by adding 2.00...

As described in part A of the lab, you are preparing a solution by adding 2.00 mL of 0.00200 M KSCN in HNO3 and 25.00 mL of 0.200 M Fe(NO3)3 in HNO3 into a clean, labeled 100.00 mL volumetric flask and diluting to the 100.00 mL mark with 0.25 M HNO3. Calculate the final concentration of KSCN in HNO3. 0.00200 M 0.000400 M 0.0000400 M 0.0000315 M 0.0500 M

Calculate the initial concentration of iron(III) in solution #1, #2, #3. Beaker (mL) Table 1. Reagent...

Homework Answers

Request Answer!

Add Answer to:
Calculate the initial concentration of iron(III) in solution #1, #2, #3. Beaker (mL) Table 1. Reagent...

Post as a guest

Earn Coins

Calculate the initial concentration of Fe3+ in test tubes 1-4. (you will need to take the...

Part A of lab: pour 30 ml of 0.150 M Fe(NO3)3 into a 50 ml beaker...

In a dilute nitric acid solution, Fe3+ reacts with thiocyanate ion (SCN−) to form a dark...

1. You prepare a mixture to use to create a colorimetry calibration curve for FeSCN2+ by...

3. Experimental Procedure, Part A.1. For preparing a set of standard solutions of FeNCS, the equilibrium...

(10 pts) The iron content of a well water sample is determined by UV-Vis spectroscopy. A...

Calculate initial concentration of Fe+3 for tubes 1-3. Show your work. Procedure A. Determination of B...

How do I find the concentration of KSCN & FeSCN2+ from the following data? Solution Beaker...

Question 13 of 13> Attempt 1 A standard solution of FeSCN2+ is prepared by combining 9.0...

As described in part A of the lab, you are preparing a solution by adding 2.00...

Calculate the initial concentration of iron(III) in solution #1, #2, #3. Beaker (mL) Table 1. Reagent...

Homework Answers

Request Answer!

Add Answer to: Calculate the initial concentration of iron(III) in solution #1, #2, #3. Beaker (mL) Table 1. Reagent...

Post as a guest

Earn Coins

Add Answer to:
Calculate the initial concentration of iron(III) in solution #1, #2, #3. Beaker (mL) Table 1. Reagent...