using your average value for the equilibrium constant, calculate the equilibrium NCS- concentration in your solution...
using your average value for the equilibrium constant, calculate the equilibrium NCS- concentration in your solution of "known concentration"
Average K = 620.4
Volume of "known concentration" = 0.02L
Known Concentration = 10.0mL of 0.05 M Fe(NO3)3 in 1M HNO3, 2.0mL of 0.0005M NaNCS, and 8.0mL of distilled water.
(you can assume that all the NCS- is converted to FeNCS2+)
Homework Answers
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using your average value for the equilibrium constant, calculate
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What's the concentration of [FeSCN2+] using limiting
reactant theory and equation?
For each test tube solution enter the initial concentration of Fe+ and SCNthe equilibrium concentration of FeSCN2: into the ICE table given. Complete entries for the rest of the table and calculate the K value for each of the tables. The values of K should be confined to a narrow range to reflect constancy. Comment on the quality of your work in this regard and calculate the average K....
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Determine the equilibrium concentration of FeSCN2+ in each
solution. (Page below are the initial concentrations of FE3+ and
scn- for each solution )
Secondly, use stoichiometry to determine equilibrium FE3+ and
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the absorbance of each standard in the same test tube used to blank the spectrophoto standards from least to most concentrated, rinsing with a small amount of the next sta tilling the test tube. Record absorbance...
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Calculate the initial moles of Fe3+ and SCN- for solutions E2
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You obtain the moles of the reactants by multiplying their molarity
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Determine the equilibrium concentration of FeSCN2+ for each of
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