Adding Fe(NO3)3 to the aqueous equilibrium system: Fe3+ + SCN -- FeSCN2+ (light yellow) - (deep red) will produce which of the following changes? The color in the test tube becomes a lighter red because the equilibrium will shift to make more products.

For instance, the only reagent that will contribute to [Fe3+] is from Fe(NO3)3. Therefore use the corresponding M (molarity) and multiply with the volume added and finally divide by the total volume (0.010 L) Please explain how you worked this problem out

An aqueous solution of iron(III) nitrate, Fe(NO3)3, is made by dissolving 18.0 grams of iron(III) nitrate in sufficient water in a 200. mL volumetric flask, and then adding enough water to fill the flask to the mark. What is the weight/volume percentage of iron(III) nitrate in the solution? Weight/volume percentage = % Match the solutions to the

Question: calculate the concentration of FeSCN2+, calculate the concentration of Fe(NO3)3 after dilution with KSCN and HNO3 and then assume all the Fe(NO3)3 is converted to FeSCN2+. Volume of Solution A 0.1M HNO3:4.0 mL

For the equilibrium Equation Fe 3+ + SCN-<--> Fe(SCN)-all aqeous. Write the equilibrium constant expression: Explain the color changes in terms of LeChateliers's Principle; when you add Fe(NO3)3 when you add KSCN and when you add NaOH. 2. write a net ionic equation for the reaction of OH- and the Fe(SCN)2+ complex

When solution of Fe(NO_3)_3 and NaC_7H_5O_3 are mixed, the Fe^+3 and C_7H_5O^-_3 ions react to form a reddish-purple material having the formula (FeC_7H_5O_3)^+2. The reaction between the Fe^+3 and C_7H_5O_3^+ ions is fast and reversible and reached the equilibrium quickly. (a) Write a balanced molecular equation for the above reaction.

A. The solution in Procedure A: 1. Calculate the number of moles of Fe(NO3h 9H,O actually used to make the solution (The molecular weight must include the 9 waters.) 2. Calculate the % of Fe(NO3), in the Fe(NO)-9H20 crystals. 3. Calculate the density of the solution. 4. Use the mass of Fe(NO3), in the solution to calculate the % Fe(NO3), in the ...

A solution of iron(III) nitrate, Fe(NO3)3, was mixed with a solution of potassium carbonate, K2CO3. A precipitate was formed. What is the chemical formula of the precipitate? (See Appendix 2 and Appendix 3 at the end of this experiment.)

Question: Fe(SCN)3 formed in the reaction has where two solutions meet. KSCN starts the left, Fe(NO3)3 starts on the right(10) Answer the following based on the video a) appearance of solid Fe(NO3)3 b) appearance of solid KSCN c) appearance of dissolved Fe(NO3)3 d) appearance of dissolved KSCN e) Reaction observations2.

K2CO3(aq)+Fe(NO3)3(aq) the mixture contains the ions listed below. Sort these species into spectator ions and ions that react. Drag the appropriate items to their respective bins. NO3-)aq), Fe3+ , CO3 2-, K+. Part B. What is the correct net ionic equation, including all coefficients, charges, and phases, for the following set of reactants?