For Sample 1, the glucose/fructose standard (0.2 mg/mL for each of glucose and fructose): From the absorbance, calculate the concentration of glucose in Sample 1, in mg/mL.  The absorbance of glucose is 0.345

you get an order of 5% amino acid 15% dextrose premixed parenteral nutrition solution, 2L at 83mls/hr.  Your pharmacy technician tells you there is a manufacture's backorder on those.  How many ml of 20% dextrose would you need to provide the same amount of dextrose in 24 hours?

The following data give the constant dissociation, Ka (for acetic acid at various temperatures): T(°C) 0 Ка 1.657 x 10-5 10 1.729 x 10-5 15 1.745 x 10-5 25 1.753 × 10-5 kJ ΔΗ° = 1.53 mol Submit Previous Answers Part B Correct Plot Inka vs. 1/T and fit a line to the points. The slope will correspond to —▲H° / R. 1/T InKa 3.66 x 10-3-11.01 3.53 x 10-3-10.97 3.47 x 10-3-10.96 3.36 × 10-3-10.95 InKa = (−184 K) (±) — 10.3 = slope -184 K = AH° R AH° -184 K = 0.008314 kJ/(mol·K) AH 1.53 kJ/mol = Use these data, and the constant dissociation at 25 °C, to calculate AS° for acetic acid ionization. (InK Express your answer with the appropriate units. μÅ AS° = Value Units ? -AH° + ᎡᎢ. AS° R

How do I calculate the final concentration? I just need one solution to walk through the steps.    Prepare eight standards of glucose with your 1 mM glucose solution, each with a final volume of 10 mL. Complete the table on the next page, indicating what your final concentration of glucose will be for each standard, in mM. Volume of Potassium Ferrocyanide Solution Volume of Enzyme Solution Volume of 1 mM glucose solution Final volume of solution Final Concentration of glucose in final solution (mM) 2.50 mL 1.00 mL 0.00 mL 10.00 mL   2.50 mL 1.00 mL 0.50 mL 10.00 mL   2.50 mL 1.00 mL 1.00 mL 10.00 mL   2.50 mL 1.00 mL 2.00 mL 10.00 mL   2.50 mL 1.00 mL 3.00 mL 10.00 mL   2.50 mL 1.00 mL 4.00 mL 10.00 mL   2.50 mL 1.00 mL 5.00 mL 10.00 mL   2.50 mL 1.00 mL 6.00 mL 10.00 mL