What would be the pH of the solution in Question 43 if you were to add 3.0 mL more of 1 M HCl?

Question 43

If you have 100 mL of a 0.10 M TRIS buffer at pH 8.3 (Table 2.8) and you add 3.0 mL of 1 M HCl, what will be the new pH?

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Table 2.8 Acid and Base Form of Some Useful Biochemical Buffers Name Acid Form N-tris[hydroxymethyl] aminomethane (TRIS) N-tris[hydroxymethyl] methyl-2- aminoethane sulfonate (TES) N 2-hydroxyethylpiperazine-N-2- ethane sulfonate (HEPES) 3 [N-morpholino]propane- sulfonic acid (MOPS) Piperazine-N,N- bis[2-ethanesulfonic acid] (PIPES) TRIS-H+ (protonated form) (HOCH₂),CNH; TES-H+ (zwitterionic form) (HOCH₂) CNH CH₂CH₂SO. HEPES-H* (zwitterionic form) HOCH₂CH.N NCH.CH.SO, NCH₂CH₂SO; ⇒ HOCH₂CH₂NNCH₂CH₂SO H MOPS-H+ (zwitterionic form) *NCH₂CH₂CH₂SO, H 2-PIPES-H+ (protonated dianion) O,SCH₂CH.N Base Form TRIS (free amine) (HOCH₂),CNH₂ TES (anionic form) (HOCH₂),CNHCH₂CH₂SO, HEPES (anionic form) NCH.CH.S NCH.CH.SO, H MOPS (anionic form) NCH CH₂CH₂SO, 2 PIPES (dianion) OSCH₂CH.NNCH₂CH.SO, O,SCH₂CH.N pk₂ 8.3 7.55 7.55 7.2 6.8