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I'm doing a worksheet for my Chemistry 209 lab and I need to knowhow to write the equilibrium constant expressions for: Please alsowrite the net ionic equation
A.The formation of FeSCN2+ from Fe3+ and SCN-
B.The reaction of KHP with NaOH
C.The titration of Na2CO3 with HCl

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Beverley Smith
Beverley SmithLv2
28 Sep 2019

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Related questions

I am doing analytical chemistry lab of preparing standard acid and base (titration)

I need the sample calculation of Naoh and HCL molarity each for their own 3 trials

Data for Naoh (I have to prepare Naoh by my self I believe molarity is 0.1)

trial KHP Naoh volume Naoh molarity

1 0.51g 33.82 mL ?

2 0.51g 30.64 mL ?

3 0.51g 31.12 mL ?

Data for HCL (I have to prepare HCL by my self I made a mistake by only use 500ml water instead 1000. I believe molarity is 0.2)

trial Na2CO3 HCL volume HCL molarity

1 0.13g 13.1 ?

2 0.13g 11.59 ?

3 0.13 9.87 ?

Please show calculations for all the molarity. Big thanks

Please can you help me with the explanation and observations in terms of LeChatelier on each page. I have 3 altogether. Thanks.

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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