Procedure Fe3+ (aq) + SCN . (ay-FeSCN2+ (aq) light brown coess Eq. 11.8) red 1. Put 1 drop of 0.1 M iron (II) nitrate solution (Fe(NO,) into a clean 10-cm test tube. Add 1 drop of 0.1 M potassium thiocyanate solution (KSCN) to the test tube. Add 5 mL of distilled water to the test tube and mix well. 2. Put 20 drops of the solution prepared in Step 1 into each of five clean 10-cm test tubes. 3. Use one of the test tubes as a color reference that represents the initial equilibrium condition Note its orange color that results from the equilibrium mixture containing both the light-brown-colored Fe ions and red-colored FeSCNons in solution. Set the reference tube aside so you can compare other tube colors to it 4. The remaining four samples in the test tubes will be used in the four tests described below. Perform one test on each test tube. In each test, make sure the test tube contents are mixed well during heating or cooling and after test reagents are added. Then note and record in Table 11.7 any differences in the color intensity of the solution compared to the reference solution (lighter or darker orange than the reference) a. Add 2 drops of 0.1 M iron (III nitrate solution (Fe(NO to one test b. Add 2 drops of 0.1 M potassium thiocyanate solution (KSCN) to one c. Add 1 drop of 0.1 M silver nitrate solution (AgNO,) to one test d. Cool one test tube in a small beaker of ice and water for 10 minutes. tube. test tube. tube. 5. Put 20 drops of a saturated solution of calcium acetate (Ca(C2HO22) into a clean, dry 10-cm test tube. Note that this solution contains the equilibrium concentration of both Ca and C2H3O ons that are in- volved in the equilibrium represented by Equation 11.9. Note that this is an equilibrium between undissolved solid and dissolved solid. Focus on the amount of undissolved solid present. Eq 11.9) 6. Record the initial appearance of the original solution in Table 11.9 Then put the test tube into a boiling water bath for 3 minutes. Agitate the test tube to mix the contents after heating for 3 minutes, then note and record the appearance of the sample in the test tube 7. Cool the sample in a small beaker of ice and water for 3 minutes. Agitate the test tube two or three times during the cooling. When the cooling is completed, note and record the appearance of the sample.

A student combines Fe(NO3)3 solution and KSCN solution to produce a solution in which the initial concentrations of Fe3+(aq) and SCN–(aq) are both 5.58 × 10–2 M. The chemical equilibrium forms FeSCN2+(aq):             Fe3+ + SCN- <=> FeSCN2+ The absorbance of this solution (from FeSCN2+) is measured as 0.161, and Beer's law equation (the trend line from best fitting) as Absorbance = 189 x Concentration of FeSCN2+ + 0.02 Determine the equilibrium concentration for SCN- in mol/L.

Could you please baland identify what type of reaction this is?

To rule out metabolic acidosis in a patient's blood sample, the total carbon dioxide content should be measured (HCO3-+CO2), this was determined by acidifying the sample and measuring the volume of CO2 released. The concentration of H2CO3 was 28.5 mmol/L, the pH of the blood at 37 ℃ is 7.48 with a pka of 6.10, what is the concentration of HCO3- in mmol/L in the blood? a) 27.36b) 22.77c) 28.50d) 29.60