Question
Read MISC Graphical a discussion of graphing procedures. Measurements in this Briefly explain each of the following Why are all of the solutions used in this experiment 10 times 10^-1 M for HNO_3? What are the hazards of using solutions HNO_7 Briefly explain the meanings of the following terms reversible reactions state of dynamic equilibrium constant expression equilibrium constant absorbance Boer's Law plot A student determining the equilibrium constant is followed the procedure in this experiment In pare 1, 200 times 10^-3 and Fe^3+ and 3.00 times 10^-3 are used. All standard solutions were prepared in 100mL volumetric fluids. Complete the following calculations, and enter the data in Table 3 on the next page. Calculate the initial molar SCN^- are used. All standard solutions were prepared in 100 mL volumetric flasks. Complete the following calculations, and enter the data in Table 3 on the next page. Calculate the initial molar SCN^- ion concentration in standard solutions S3 and S5. Calculate the molar FeNC5^2+ ion concentration in standard solutions S3 and S5. Calculate the absorbances for standard solutions S3 and S5. Prepare a Beer's Law plot, on the graph paper earlier in this experiment, for the FeNC5^2+ ion, using data for standard solutions S1-S6. In part II, 200 times 10^-3 M Fe^3+ ion and 2.00 times 10^-3 M SCN^+ ion stock solutions were used to prepare the equilibrium mixtures indicated in table 4 on the next page. The %T of the equilibrium solutions (E2-E4) are listed in Table 5 on the next page. Make the following calculations in the spaces provided, and enter the results in Table 5. Calculate the initial Fe^2+ ion concentration in equilibrium mixtures E2-E4. Calculate the initial SCN^- ion concentration in equilibrium mixtures E2-E4. Express the %T readings for solutions E2-E4 as equivalent absorbances. Use your Beer's Law plot to determine the equilibrium FeNCS^2+ ion concentration in solutions E2-E4. Determine the equilibrium molar Fe^3+ ion concentration in solutions E2-E4. Determine the equilibrium molar SCN^- ion concentration in solutions E2-E4. Calculate K_aq for the formation of FeNCS^2+ ion at the experimental temperature, using the data for solutions E2-E4. Use your calculated K_eq8 from (11) to calculate the mean K_eq for the formation of FeNCS^2+ ion at the experimental temperature.
Explanation / Answer
Q2.
a.
all solutions are the same concentration of HNO3 in order to have a standard, so this facilitates operation/calculations. Also, this concentration is safe to work with
b.
The hazards are low, but yet, since it is a strong acid, hazards are --> exothermic reaciion with bases, irritates skin/eyes
Q3.
briefly explain
a. reversible reaction --> a reaction that could form reactants from its products
b. State of dynamic eq. this is a definition in which in reality, there is a change between reactants/products, but the overal rate is 0, terefore this is in equilbirium, yet dynamics
c. eq. constant exp. This is a vlaue that relates the concentration of reactants/products in equilibrium
d. eq. constnat --> this is a value which only depends on T, it is a value that relates concentrations of reactants/produts
e. spectrometer --> this is an equipment used in analytical chemistry, it helps to identify via light many analytes
f. absorbance --> how much a specie "absorbs" light
g. beer Law plot --> A plot that relates absorbance vs. Concentration
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