Using the Henderson-Hasselbalch equation, calculate the pH of a buffer solution made from 0.20 M CH3COOH and 0.050 M CH3COO" that has pK3= %3D 4.7. 4.1 0.4 None of the answers is correct 2.5 5.3
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- 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 unitsA 35 mL of solution of hydrochloric acid is neutralized by 15 mL of 0.5 M potassium hydroxide. What is the concentration of hydrochloric acid? The balanced equation is HCI + KOH - H,O + KCI O 0.75 M O 0.25 M O 0.214 M O 0.786 MCalculate the pH of a buffer that contains 0.15 M MOPS anionic form and 0.25M MOPS zwitterion. The pKa is 7.2
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- 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.Calculate 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)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