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What is the pH of a 0.1 M solution of TRIS acid? What about the pH of a 0.1 M solution of TRIS base?

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The pH of the TRIS acid is  [tex]8.1 + log [\frac{A-}{0.1} ][/tex].

The pH of the TRIS base is  [tex]8.1 + log [\frac{B}{0.1} ][/tex].

pH of the TRIS acid

The pH of the TRIS acid is determined by applying Henderson - Hasselbalch equation as follows;

[tex]pH=pK_a + log \ [\frac{A^-}{HA} ][/tex]

where;

pKa of TRIS acid = 8.1

  • A-  is the concentration of the conjugate base
  • HA is the concentration of the weak acid

[tex]pH = 8.1 + log [\frac{A-}{0.1} ][/tex]

pH of the TRIS base

The pH of the TRIS base is determined by applying Henderson - Hasselbalch equation as follows;

[tex]pH=pK_a + log \ [\frac{B}{BH^+} ][/tex]

where;

  • pKa of TRIS acid = 8.1
  • B  is the concentration of the conjugate acid
  • BH is the concentration of the weak base

[tex]pH = 8.1 + log [\frac{B}{0.1} ][/tex]

Learn about pH of buffer solutions here: https://brainly.com/question/8687967

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