BMB 200 Study Guide - Midterm Guide: Essential Amino Acid, Amide, Isoelectric Point

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lemondog658

4 Feb 2020

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MSU

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Biochemistry and Molecular Biology

Course

BMB 200

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The negative decimal logarithm of the hydrogen ion concentration in a solution. The point at which an amino acid is electrically neutral. Rank the above solutions from most acidic to least acidic. 0. 01 m naoh > 0. 001 m naoh>0. 1m nacl > 0. 01m hcl > 0. 1 m hcl. 0. 1 m nacl > 0. 01 m naoh > 0. 001m naoh>0. 01m hcl > 0. 1 m hcl. 0. 1 m hcl > 0. 01m hcl > 0. 1 m nacl > 0. 001 m naoh>0. 01m naoh. 0. 001m naoh> 0. 01 m naoh > 0. 1 m nacl > 0. 1m hcl > 0. 01m hcl. 0. 1m hcl > 0. 01m hcl > 0. 001 m naoh> 0. 01 m naoh>0. 1m nacl. The ph is the point at which an amino acid is electrically neutral. An acid is a proton (hydrogen ion) acceptor. The ph is the positive decimal logarithm of the hydrogen ion concentration in solution. A ph of 10 indicates a strong acid.

Related Questions

Acetate buffer is often used as a buffer solution for protein studies at acidic pH (from 3.6 to 5.6). The dissociation reaction is: CH₃COOH <---> CH₃COO^- + H⁺

Here CH₃COOH (abbreviated as HOAc) and the acetate anion CH₃COO^- (abbreviated as OAc^-) are the conjugate acid-base pair.

a.) Suppose you prepared an acetate buffer containing 0.1M of HOAc and 0.1M of OAc^-. What are the [H⁺] and pH of this solution?

b.) Now you add 0.01M HCl to your acetate buffer. What are the [H⁺] and the pH after the HCl is added and the mixture reaches equilibrium?

c.) Suppose you add 0.01M HCl to a solution containing 0.18M of HOAc and 0.02M of OAc^-. What are the [H⁺] and the pH before the HCl is added, and after the HCl is added?

d.) Suppose you add 0.01M HCl to a solution containing 0.02M of HOAc and 0.18M of OAc^-. What are the [H⁺] and the pH before the HCl is added, and after the HCl is added?

a. For the titration of 25.0 mL of 0.1 M HCl (aq) with 0.1 M NaOH (aq), at what volume of NaOH (aq) should the equivalence point be reached and why? If an additional 3.0 mL of 0.1 M NaOH (aq) is then added, what is the expected pH of the final solution?

b. What is the initial pH expected for a 0.1 M solution of acetic acid? For the titration of 25.0 mL of 0.1 M acetic acid with 0.1 M NaOH (aq), at what volume of NaOH (aq) is the equivalence point reached? Is the pH at the equivalence point greater than, less than or the same as in problem #a above? Explain.

c. What is the initial pH expected for a 0.1 M solution of phosphoric acid (H3PO4)? For 25.0 mL of 0.1M H3PO4 (aq), what volume of 0.1 M NaOH (aq) is required to fully titrate all three protons to their end points?

d. In the titration of a weak acid with a strong base, how is the half equivalence point determined and what is its significance? How are the pKa and Ka of the weak acid determined from the half equivalence point?

BMB 200 Study Guide - Midterm Guide: Essential Amino Acid, Amide, Isoelectric Point

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