Aspirin (acetylsalicylic acid, structure below), has a pKa of 3.5. The pH at which aspirin is most soluble is water is OCOCH3 COOH pH = 0 pH >> 3.5 pH = 3.5 pH << 3.5

Make a 100 ml of a 1M stock solution of NaCl (you will need the molecular weight of NaCl).

How would I calculate the amount of each component in each solution?  Stock solutions provided: 0.5 M EDTA, pH 8 10% bromophenol blue 10% xylene cyanol Sucrose powder Tris powder Glacial acetic acid  Solution A: 50 mL of 50x Tris Acetate EDTA (TAE) Buffer 2M Tris Base 50mM EDTA, pH 8 11.4% (v/v) glacial acetic acid Solution B: 1L of 1x TAE Buffer 40mM Tris-acetate 1mM EDTA Solution C: 5mL of 10x Loading Dye 0.25% (w/v) bromophenol blue 0.25% (w/v) xylene cyanol 66.5% (w/v) sucrose 100mM EDTA, pH 8

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?

Calculate the unknown concentration of the PROTEIN C with an absorbance value of A412 given the standard curve indicated in the table below. Write your final answer (NUMBER ONLY) in two decimal places rounded off. Protein concentration (µg/mL) 0 0.02 0.04 0.06 0.08 0.10 Your answer APIENT Absorbance 0.000 0.161 0.284 0.438 0.572 0.762

what is the pH of a solution with a H+ concentration of 1.44 x 10-3 M

Bonly

Protein Solubility 3.5 5.5 5 5 0.068 0.028 Absorbance 0.098 Conc.(mg/ml) 0.195 0.130 0.044 0.9% 2.786% 9.429% 11.3: % solubility 4.179% The above table indicates the concentration of protein in the diluted supernatant and the supernatant before dilution at different pH. Dilution Factor 30 22.5 15 PH 7.5 1.5 4.5 5 0.027 3 0.042 Protein Solubility Versus pH 6.5 6 4.5 pH Value The above figure shows a plot of protein solubility versus pH. 50 7.5 7.5 50 0.032 0.053 8.5 50 0.054 0.100 21.429% 9 Please provide a brief discussion and explanation of the results. (using isoelectric point and net charge to explain)

A buffer contains 0.015 mol of lactic acid (pK₁ = 3.86) and 0.080 mol of sodium lactate per liter. H₂C OH Lactic acid OH Calculate the pH of the buffer. H₂C. Calculate the change in pH after adding 9.0 mL of 0.10 M HCl to 1.0 L of the buffer. O OH Sodium lactate Calculate the change in pH after adding 9.0 mL of 0.10 M HCl to 1.0 L of pure water. O Na+ buffer pH: buffer pH change: water pH change: units units

pH of solution 14.00 12.00 10.00 8.00 6.00 First 4.00 equivalence point 2.00 0 First midpoint Second equivalence point Third midpoint pH = pKa=12.32 Third equivalence point HPO4(aq) + OH(aq) PO4(aq) + H2O(1) Second midpoint pH = pKa = 7.21 H2PO4 (aq) + OH(aq) HPO42 (aq) + H2O(1) Using the Henderson- Hasselback equation, show how to create 2L of a 0.1 M KPhos pH 7.5 buffer using K2HPO4 and KH2PO4. The chart to the left should help you understand what pKa to start with. Show your work. pH = pKa = 2.16 H3PO4(aq) + OH(aq) H2PO4(aq) + H2O(l) 25.0 50.0 75.0 100.0 Volume of NaOH added (mL)