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Using these charts1) I need to find the molarity of the diluted KSCN solution. 2) Also need to find the initial molarities for Fe3+ ion and SCN- ion in test tubes 1 through 5. Chart 1Test tube Diluted KSCN (mL) 0.25M Fe(NO3)3 (mL) 0.1M HNO3 (mL) 1 1.0 5.0 4.0 2 2.0 5.0 3.0 3 3.0 5.0 2.0 4 4.0 5.0 1.0 5 5.0 5.0 0 Chart 2Test tube 0.0025M Fe(NO3)3 (mL) 0.0025 KSCN(mL) 0.1M HNO3 (mL)6 1.0 1.0 5.07 1.0 1.5 4.5 8 1.0 2.0 4.09 1.0 2.5 3.510 1.0 3.0 3.011 2.0 1.0 4.012 2.0 1.5 3.513 2.0 2.0 3.014 2.0 2.5 2.515 2.0 3.0 2.0

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Casey Durgan
Casey DurganLv2
28 Sep 2019

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Related questions

Find the concentration of Fe(SCN)2+ for each test tube.

30mL of 0.200M Fe(NO3)3 was prepared. Then, 15mL of 0.0020M KSCN was prepraed in another beaker. 10.0mL of prepraed KSCN solution was pipetted into a 100mL flask and the volume was brought up to 100.0 mL with distilled water.

Then, five solutions were prepared according to the chart.

Test Tube #

0.200 M Fe(NO3)3 (mL)

Diluted KSCN (mL)

H2O (mL)

1

5.0

1.0

4.0

2

5.0

2.0

3.0

3

5.0

3.0

2.0

4

5.0

4.0

1.0

5

5.0

5.0

0

6 (blank)

5.0

0.0

5.0

Find the concentration of Fe(SCN)2+ for each test tube.

CHEMISTRY REPORT DUE TONIGHT HELP!!! About Equilibrium Constants, and I would appreciate any feedback that can help me answer my last couple of questions!!

Part 2: Determining the equilibrium constant

Table .2 shows the amounts of 2.00 ´ 10–3 M Fe(NO3)3 (in 1 M HNO3) solution, 2.00 ´ 10-3 M KSCN solution, and DI water that you should add to each tube. Add these chemicals to your three test tubes. Note that your test tubes are labeled by number. Be sure to add the solutions to the correct tube. Pipet the approximate amount of each solution into each tube. On your data sheet, record the exact amount of each solution that you add. You will need to use these actual amounts in your calculations.

Table 2 Composition of solutions for determining the equilibrium constant.

Test Tube

Vol of 2.00 ´ 10-3 M Fe(NO3)3 in 1 M HNO3 (mL)

Vol of 2.00 ´ 10-3 M KSCN (mL)

Vol of DI water
(mL)

1

5.0

1.0

4.0

2

5.0

2.0

3.0

3

5.0

3.0

2.0

4

5.0

4.0

1.0

5

5.0

5.0

0

Data and Results

3. You have been told that the reaction you are observing is:

Fe3+ (aq) + SCN-– (aq) ⇄ FeSCN2+ (aq)

Another possibility is that the reaction is:

Fe3+ (aq) + 2 SCN-– (aq) ⇄ Fe(SCN)2+ (aq)

Write the equilibrium equation for this new reaction.

Using your data from the mixtures in test tubes 1, 3, and 5 of Part 2, recalculate three new equilibrium constants for this new possible reaction. Hint: Notice that the change in concentration of SCN- in your equilibrium table will change because of the new stoichiometry. Also, the exponent on [SCN-] in the equilibrium constant expression will change for the same reason.

What are the three new equilibrium constants?

Why do the results of your calculations show that the reaction you are observing is more likely to be the first one (one mole of SCN- with one mole of Fe3+)?

4. In Part 1 of this experiment, you made the assumption that the FeSCN2+concentrations in your standard solutions were equal to the initial concentrations of SCN- ions. Now that you know the value of the equilibrium constant, calculate the actual equilibrium concentrations of Fe3+, SCN-, and FeSCN2+ in mixture in test tube 2. How good was the assumption? Did this satisfy the 5% rule (the loss of reactant is less than 5% of its initial concentration)?

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