Question 1. Dscribe the change you observed when you added 1 mL of 0.1 M KSCN to the 2 mL portion of the diluted solution. Copy the equation from the procedure and explain your observations in terms of LeChatelier’s Principle. Choose the best answer. The additional thiocyantate ion shifted the equilibrium toward the products, producing morehexathiocyanatoferrate(III) lightening the color. Fe3+(aq) + 6SCN-(aq) Fe(SCN)63-(aq). The additional thiocyantate ion shifted the equilibrium toward the reactants, producing lesshexathiocyanatoferrate(III) and deepening the color. Fe3+(aq) + 6SCN-(aq) Fe(SCN)63-(aq). The additional thiocyantate ion shifted the equilibrium toward the reactants, producing morehexathiocyanatoferrate(III) lightening the color. Fe3+(aq) + 6SCN-(aq) Fe(SCN)63-(aq). The additional thiocyantate ion shifted the equilibrium toward the products, producing morehexathiocyanatoferrate(III) and deepening the color. Fe3+(aq) + 6SCN-(aq) Fe(SCN)63-(aq). Question 2. Show your calculations to determine the final volume of the 0.001 M FeCl3 solution. Choose the best answer. M1V1 = M2V2. (0.001 M)V1=(0.1 M)(0.05 L) V1=0.050 L = 50 mL M1V1 = M2V2. (0.001 M)V1=(0.1 M)(0.005 L) V1=0.500 L = 500 mL M1V1 = M2V2. (0.1 M)(0.005 L)=(0.001 M)V2 V2=0.500 L = 500 mL M1V1 = M2V2. (0.1 M)(0.0005 L)=(0.001 M)V2 V2=0.050 L = 50 mL Question 3. Describe the change you observed when you added 1 mL of 0.1 M FeCl3 to the diluted mixture of 0.001 M FeCl3(aq) and 0.1 M KSCN(aq). Refer to the equation in step 1 and explain your observations in terms of LeChatelier’s Principle. Choose the best answer. Additional iron(III) ion shifted the equilibrium toward the products to form the red-colored hexathiocyanatoferrate(III) complex and the intensity of color increased.color. Fe3+(aq) + 6SCN-(aq) Fe(SCN)63-(aq). Additional iron(III) ion shifted the equilibrium toward the products to form the red-colored hexathiocyanatoferrate(III) chloride precipitate. Fe3+(aq) + 6SCN-(aq) Fe(SCN)6Cl3(s). Additional iron(III) ion caused the equilibrium to shift to the reactants to compensate for the additional added iron(III), which increased the intensity of the red color. Fe3+(aq) + 6SCN-(aq) Fe(SCN)63-(aq). Additional iron(III) ion increased the concentration of the red-colored iron(III) ion. Fe3+(aq) + 6SCN-(aq) Fe(SCN)63-(aq). Question 4. Predict and then describe what happened when you added HCl(aq) to the copper nitrate solution. Write down the equation for the reaction. Choose the best answer. The added hydrogen ion shifted the equilibrium toward the products so that more CuCl42-(aq) was createdand the solution changed from blue to green. Cu(H2O)42+(aq) + 4Cl-(aq) CuCl42-(aq) + 4H2O(l). The added chloride ion shifted the equilibrium toward the products so that more CuCl42-(aq) was created and the solution changed from blue to green. Cu(H2O)42+(aq) + 4Cl-(aq) CuCl42-(aq) + 4H2O(l). The added chloride ion caused the precipitation of CuCl42-(s), which shifted the equilibrium toward t.