An equilibrium solution is prepared from 1.5 mL of 0.0020 M KSCN, 2.5 mL of 0.0020 M Fe(NO3)3, and 6.0 mL of 0.1 M HNO3. Calculate the initial concentrations of Fe3+ and SCN- in the solution. Hint: The initial concentrations in the solution will change from what is listed above.

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Irving HeathcoteLv2

28 Sep 2019

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Help please!

A student mixes 5.00 mL of 0.0020 M Fe(NO3)3 with 4.00 mL of 0.0020 M KSCN solution and 1.00 mL water at a certain temperature. He places a sample of the resulting solution in a spectrometer, and measures the transmittance as 31% at 447 nm.

a) What are the initial concentration of [Fe3+] and [SCN-]?

b) What are the final concentrations of [Fe3+], [SCN-], and [FeSCN2+]?

c) What is the measured value of Keq?

The molar absorptivity at 447 nm (Îµ = 4400). Path length = 1 cm.

amethystmule446

a student mixes 5.00 mL of 0.0020 M Fe(NO3)3 with 5.00 mL of.0020 KSCN solution at a certain temperature. He places a smaple ofthe resulting solution in a spectrometer, and measures thetransmittance as 37% at 447 nm.

a. What are the initial concentrations of FE and SCN

b. What are the final concentrations of FE, SCN, and FeSCN?

c. What is the measured value of Keq? PLEASE EXPLAIN STEPS FOR ALL POINTS WHICH I WILL GLADLY REWARD IFUNDERSTOOD< THANK YOU