3.0 mL of 0.02 M Fe(NO3)3 solution is mixed with 3.0 mL of 0.002 M NaNCS and diluted to the mark with HNO3 in 10 mL volumetric flask. The blood-red [Fe(NCS)]2+ ion that forms has an equilibrium molar concentration of 2.5*10-4 mol/L as determined from the calibration plot. Calculate the Kc for [Fe(NCS)]2+ formation. Assume the volumes are additive.

The for formation is .

Explanation:

Concentration of ferric ion =

Volume of ferric solution = 3.0 mL = 0.003 L

Moles of ferric ion  

1 mL = 0.001 L

Concentration of ion =

Volume of ion solution = 3.0 mL = 0.003 L

Moles of ion=

Volume of nitric acid solution = 10 mL = 0.010 L

After mixing all the solution the concentration of ferric ion and ion will change

Total volume of solution = 0.003 L + 0.003 L + 0.010 L = 0.016 L

Initial concentration of ferric ion before reaching equilibrium :

=

Initial concentration of ion before reaching equilibrium :

=

Initially:

0.00375 M    0.000375 M       0

At equilibrium :

(0.00375-x)   (0.000375-x)       x

Equilibrium concentration of

The expression of equilibrium constant for formation is given by :

The for formation is .

answer: option (b) is the correct answer.

explanation:

a covalent bond is formed by sharing of electrons. whereas polarity arises due to difference in electronegativity of two atoms.

therefore, more is the electronegativity of an atom which combines with the titanium, more readily it will induce a partial positive and negative charge.

thus, out of the given options fluorine is most electronegative and has an incomplete octet. therefore, it will readily combine with titanium to share the electrons and complete its octet.  

yes

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