22. If 75 mls of 0.02 M HCI is added to 425 mls of 0.5 M glycine buffer at pH 10.4, what is the resultant pH? (pK1 for Gly= 2.2, PK2=9.4)
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- What mass of sodium glycolate (NaC2H3O3) should be added to 400.0 mL of 1.00 M glycolic acid to produce a buffer solution with a pH of 4.00? Ka = 1.47 x 10-4. Please indicate the full solutions.What mass of sodium glycolate (NaC2H3O3) should be added to 400.0 mL of 1.00 M glycolic acid to produce a buffer solution with a pH of 4.00? Ka = 1.47 x 10-42. A. If 100 mls of 0.03 M HCI is added to 400 mls of 0.5 M glycine buffer at pH 10.4, what is the resultant pH? (pK1 for Gly= 2.2, Pk2=9.4) Gly.4L X.5mol/L= .2 mol HCI.1LX.03mol/L = .003mol Glyº .02mol +.003 mol .023mol [HA] = .023/.5L =.046M, [A-] =.177/.5L = .354M pH = pka +log [A-]/[HA] pH = 9.4 +log.354/.046 = 10.3 [HCI] = [H+] = .003mol/.5L = .006M pH =2.2 Gly + H+ .18mol -.003mol .177mol end start B. What would the pH be if the same amount of HCl as in part A was added to 400 mls of water?
- 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 unitsCalculate the pH of a buffer that contains 0.15 M MOPS anionic form and 0.25M MOPS zwitterion. The pKa is 7.2200 microliters of a standard solution of 0.200 mg/mL caffeine was mixed with 4.8 mL of 50 mM sodium phosphate buffer, pH 3: methanol (60:40 v/v). What is the concentration of caffeine, in mg/mL, in this solution? Give your answer to two significant figures.
- You just made a 1.5M permanganate solution. What concentration is your potassium permanganate solution in percent? "K: 39.10 g/mole" "Mn: 54.94 g/mole" "O: 16 g/mole" "MW of KMnO4 is 158.04 g/mole" O a. 0.24% Ob. 20.1% O c. 15.8% O d. 23.7% O e. 2%You need to prepare an acetate buffer of pH 5.43 from a 0.621 M acetic acid solution and a 2.95 M KOH solution. If you have 730 mL of the acetic acid solution, how many milliliters of the KOH solution do you need to add to make a buffer of pH 5.43? The pKa of acetic acid is 4.76. Be sure to use appropriate significant figures.Describe the preparation of 2.00 L of 0.100 M glycine buffer, pH 9.0, from glycine and 1.00 M NAOH. What mass of glycine is required, and what volume of 1.00 NaOH is required? The appropriate pK, of glycine is 9.6.
- A 0.200 M solution of a weak monoprotic acid (HA) has a pH of 2.35. What is the value of K of this acid? a K =2.011e-4 a What is the percent ionization of this acid? Percent Ionization = .10 %Describe the preparation of 2.00 L of 0.100 M glycine buffer, pH 9.0, from glycine and 1.00 M NaOH. What mass of glycine is required, and what volume of 1.00 NaOH is required? The appropriate pKa of glycine is 9.6Calculate the pH of a buffer that contains 0.75 M acetic acid and 0.35 M acetate ion in 1 L solution. What will the pH of the buffer be upon the addition of 100.0 mL of 1.0 M HCI? (pKa of acetic acid 4.76)