I need help with my homework question 5 6 and the question 1 ### Educational Chemistry Experiment: Observing Chemical Reactions#### Color Changes in 0.01 M Solutions of Fe(NO3)3 and KSCNThis experiment involves observing the color changes in a series of reactions with varying conditions. The table details the reactants added and the corresponding observations.#### Data Table| Experiment Number | Reactant Added | Observed Color | Reaction Direction ||-------------------|-------------------------------------------|---------------------|---------------------|| 1 | 10 drops water | Dark Red | Forward Reaction || 2 | 8 drops Fe(NO3)3 | Dark Red | Forward Reaction || 3 | 8 drops KSCN | Dark Red | — || 4 | 8 drops HCl | Light Orange | Backward Direction || 5 | 10 drops H2O + Heat | Light Orange | Backward Direction || 6 | 10 drops H2O + Cold | Dark Red | — |#### Questions1. **Show calculations for making the 0.01 M solutions of Fe(NO3)3 and KSCN.**##### Explanation of Observations- **Dark Red:** Indicates a forward reaction, suggesting the formation of the complex between Fe(NO3)3 and KSCN.- **Light Orange:** Indicates a backward direction, hinting at the dissociation of the complex or less formation. ##### Additional Notes- The **reference color** acts as a standard for evaluating the observed color changes.- The observation column further includes notes on the reaction direction (forward or backward) indicating the equilibrium shift. This simple experiment is useful for understanding chemical equilibria and the effects of concentration and temperature changes on reaction direction. **Title: Observing Equilibrium Shifts Through Color Change in a Chemical Reaction**---**Introduction:**In chemical reactions, observing the color change can provide insight into equilibrium shifts between reactants and products. This experiment demonstrates how adding hydrochloric acid provides chloride ions that form a complex ion with Fe³⁺, thereby shifting the equilibrium.---**Chemical Equation:**\[ \text{Fe}^{3+} (\text{aq}, \text{yellow}) + \text{Cl}^- (\text{aq}, \text{colorless}) \leftrightarrow \text{FeCl}_4^- (\text{aq}, \text{colorless}) \]---**Materials:**- **Equipment:** - Small beaker - 2 x 250 mL beakers - 6 x test tubes - Ice - Test tube rack - Pipettes- **Chemicals:** - 0.01 M Fe(NO₃)₃ - 0.01 M KSCN - 1 M Fe(NO₃)₃ - 1 M KSCN - 3 M HCl---**Procedure:**1. **Preparation of Stock Solution:** - Mix 50 mL of 0.01 M Fe(NO₃)₃ and 50 mL of 0.01 M KSCN to create a 100 mL "stock" solution.2. **Setup:** - In a small beaker, mix 10 mL each of 0.01 M Fe(NO₃)₃ and 0.01 M KSCN.3. **Test Tube Preparation:** - Set up 6 test tubes on a rack. - Add 3 mL of the stock solution to each test tube.4. **Color Observation:** - Add 10 drops of water to test tube 1 (control). - Record the color and compare it with other tubes.5. **Addition of Fe(NO₃)₃:** - Add 8 drops of 1 M Fe(NO₃)₃ to test tube 2. - Mix and observe any color shift.6. **Addition of KSCN:** - Add 8 drops of 1 M KSCN to test tube 3.

Since only first question is given, we'll answer that one.The Iron-Thiocyanate equilibrium When Iron (III) nitrate is mixed with potassium thiocyanate (KSCN), an equilibrium mixture of Fe3+, NCS- and FeNCS2+ is formed. The reaction is; Fe3+ + NCS-↔ FeNCS 2+yellow colourless blood red A red colour solution indicates that the equilibrium is shifted to right. When the solution is yellow, the equilibium is shifted to left.On adding con. HCl, the reaction goes backward as the Cl- consumes Fe3+ ion according to Le-Chateliers principle. The reaction is; Fe3++Cl-↔FeCl4- Calculations for making 50 mL 0.01 M Fe(NO3)3 and 50 mL of 0.01 M KSCN Calculations for making 50 mL 0.01 M Fe(NO3)3 from 1.0 M Fe(NO3)3 Using the Molarity equation; M1V1=M2V2where,M1=Initial concentration=1.0 MV1=initial volumeM2=final concentration=0.01 MV2=final volume=50 mLM1V1=M2V21.0×V1=0.01×50=0.5 mL On taking 0.5mL of the stock solution and diluting to 50 mL gives 50 mL of 1.0 M solution.Calculations for making 50 mL of 0.01 M KSCN from 1.0 M solution M1V1=M2V2where,M1=Initial concentration=1.0 MV1=initial volumeM2=final concentration=0.01 MV2=final volume=50 mLM1V1=M2V21.0×V1=0.01×50=0.5 mL On taking 0.5mL of the stock solution and diluting to 50 mL gives 50 mL of 1.0 M solution of KSCN.Answer The volume of Fe(NO3)3 solution for making 0.01M from 1M is 0.5mL The volume of KSCN solution for making 0.01M from 1M is 0.5mL