# How would the addition of 0.050 M nitric acid to the solution affect the equilibrium constant for the reaction?

IF a student added more KSCN solution than instructed when making standards solutions. Assuming no other errors were made in the experiment, would the value of the equilibrium constant determine in the experiment higher or lower than it should be? Justify your answer with an explanation. 2) Solutions: 0.00150 M KSCN, 0.050 M HNO3, 0.150 M Fe(NO3)3 (numbers after solutions are subscripts). HNO3 was used as the “blank solution”. Why are KSCN and Fe(NO3)3 not used as the blank solution? justify your answer. 3) When Fe(NO3)3 is dissolved in water, hexaaquairon(III) ions, Fe(H2O)6 ^3+, form. Hexaaquairon(III) ions hydrolyze in aqueous solution according to the equation given below. [Fe(H2O)6]^3+ + H2O <—> [Fe(H2O)5(OH)]^2+ + H3O^+ How would the addition of 0.050 M nitric acid to the solution affect the equilibrium constant for the reaction? justify your answer with an explanation.
1) IF a student added more KSCN solution than instructed when making standards solutions. Assuming no other errors were made in the experiment, would the value of the equilibrium constant determine in the experiment higher or lower than it should be? Justify your answer with an explanation. 2) Solutions: 0.00150 M KSCN, 0.050 M HNO3, 0.150 M Fe(NO3)3 (numbers after solutions are subscripts). HNO3 was used as the “blank solution”. Why are KSCN and Fe(NO3)3 not used as the blank solution? justify your answer. 3) When Fe(NO3)3 is dissolved in water, hexaaquairon(III) ions, Fe(H2O)6 ^3+, form. Hexaaquairon(III) ions hydrolyze in aqueous solution according to the equation given below. [Fe(H2O)6]^3+ + H2O <—> [Fe(H2O)5(OH)]^2+ + H3O^+ How would the addition of 0.050 M nitric acid to the solution affect the equilibrium constant for the reaction? justify your answer with an explanation.