You want to study the oxygen binding ability of hemoglobin at pH 7.4. You decide to use a phosphate buffer. How would you make up 600 ml of 50 mM phosphate buffer, pH 7.4, starting with 3 M Na3PO4 and either 2 M HC1 or 1 M NaOH? Show all calculations.
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- You are conducting a biochemical experiment with an enzyme that has optimal activity at pH = 10.50. You decide to use carbonate (pKa1 = 6.38, pKa2 = 10.30) as the buffer to keep the pH stable throughout the enzymatic reaction. (Recall that the formula for carbonic acid is H2CO3.) You prepare a 0.6 M solution of carbonate buffer at pH = 10.50. Calculate the concentrations of the major carbonate species in your solution. Show your calculations.Calculate the pH of a blood plasma sample with a total CO₂ concentration of 25.6 mM and bicarbonate concentration of 24.5 mM. The relevant pKa of carbonic acid is 6.1. Enter the answer with three significant figures. pH = Hyperventilating can result in a decrease in CO₂(g) concentration in the blood. How would this affect the pH of the extracellular fluid? The pH does not change appreciably. The pH increases. The pH decreases.The pH of normal urine is 6.30, and the total phosphate concentration ([PO43−] + [HPO4 2−] + [H2 PO4 −] + [H3PO4]) is 0.020 M. What is the minimum concentration of Ca2+ necessary to induce kidney stone formation?
- You need a buffer with a pH = 12. You have solid Na3PO4and 1.00 M HCl, and water. The buffer must have a total phosphate concentration of 0.750 M and have a total volume of 500 mL. Calculate the amount of Na3PO4(in grams), the volume of 1.00 M HCl, and volume of water necessary to make the desired buffer. The pKa values of H3PO4 are pKa1=2.14, pKa2=7.20, pKa3=12.37 What are the Grams of Na3PO4Consider the titration of 50.00 ml of a solution of 0.2574 M of the fully protonated form of the diprotic amino acid glycine (pKa1 = 2.34, pKa2 = 9.60) with 0.3786 M KOH. What is the pH after the addition of 33.99 mL of the KOH solution?A 0.735 g sample of wheat flour was analyzed by the Kjeldahl method. The ammonia formed by addition of concentrated base after digestion with H2SO4 was distilled into 50 mL of 0.10 M HCl. The excess HCl was then back titrated with 22.3 mL of 0.15 M NaOH. Calculate the percent protein in the wheat flour sample (6.25 g of cereal protein for every g of N).
- A sample of impure NaOH, which has been partially converted to Na2CO3 by exposure to CO2, is analyzed by titrating a 188.5 mg sample with 0.1065 M HCl. The volume required to reach phenolphtalein end point is 39.19 ml while the volume required to reach bromocresol green end point is 40.67 ml. Calculate the percentages of NaOH (MWt= 40 g/mole) and Na2CO3 (MWt=83 g/mole) in the sample.Calculate the volume, in liters, of 1.681 M KOH that must be added to a 0.117 L solution containing 9.98 g of glutamic acid hydrochloride (H₂Glu+Cl¯, MW = 183.59 g/mol) to achieve a pH of 10.18. Glutamic acid (Glu) is an amino acid with pKa values of pKal = 2.23, pK₁2 = 4.42, and PK₂3 = 9.95. volume: L NH, CÌ HC-CH₂-CH₂-C-OH C= O OH Glutamic Acid HydrochlorideExplain how the bicarbonate and phosphate buffer systems resist pH changes.
- What is the pH for a 100 ml solution of 1.0 M Benzoic Acid? If you added 10.5 grams of conjugate base (NaC6H5CO2) to the solution, what would the new pH be? How many grams of HCl would be needed to lower the pH of the buffer by .05? Step by step please. in attachmentConsider the titration of 17.50 mL of 0.459 M potassium propanoate, CH3CH2CO2K, with 0.107 M HNO3. What is the pH of the solution after 39.38 mL of the HNO3 has been added? (pKa of CH3CH2CO,H = 4.691)A 1.00 L phosphate buffer solution that contains 0.1270 moles of dihydrogen phosphate (H2PO4) and 0.0800 moles of hydrogen phosphate (HPO,2-) was prepared. The pKa of dihydrogen phosphate is 7.20 at 25 °C. Calculate the pH of the buffer at this temperature.