BMB 200 Study Guide - Midterm Guide: Essential Amino Acid, N-Terminus, Zwitterion

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lemondog658

24 Feb 2020

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MSU

Department

Biochemistry and Molecular Biology

Course

BMB 200

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professor

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Bmb 200 exam 1, fs 2019 form 1. The negative decimal logarithm of the hydrogen ion concentration in a solution. The point at which an amino acid is electrically neutral. Rank the solutions from most acidic to least acidic. 0. 1 m naoh > 0. 001 m naoh > 0. 1m nacl > 0. 001 m hcl > 0. 1 m hcl. 1 m nacl > 0. 001m naoh > 0. 001 m hcl > 0. 1 m hcl. 0. 001 m naoh > 0. 1 m naoh > 0. 1m nacl > 0. 3 m hcl > 0. 001m hcl. 0. 1 m hcl > 0. 001 m hcl > 0. 1m nacl > 0. 001 m naoh > 0. 1 m naoh. 0. 001m hcl > 0. 1 m hcl > 0. 1m naoh > 0. 1 m nacl > 0. 001 m naoh. The pi 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.

Related Questions

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?

_____1. Commercial vinegar was titrated with NaOH solution to determine the content of acetic acid, HC₂H₃O₂. For 20.0 milliliters of the vinegar 26.7 milliliters of 0.600-molar NaOH solution was required. What was the concentration of acetic acid in the vinegar if no other acid was present?

(A) 1.60 M
(B) 0.800 M
(C) 0.600 M
(D) 0.450 M
(E) 0.200 M

_____2. HSO₄^- + H₂O <===> H₃O⁺ + SO₄^2-

In the equilibrium represented above, the species that act as bases include which of the following?

I. HSO₄^-

II. H₂O

III. SO₄^2-

(A) II only
(B) III only
(C) I and II
(D) I and III
(E) II and III

_____3. Which of the following has the lowest pH?

(A) 0.1 M CuSO₄
(B) 0.1 M KOH
(C) 0.1 M BaCl₂
(D) 0.1 M HF
(E) 0.1 M HNO₃

_____4. What volume of 0.150-molar HCl is required to neutralize 25.0 millilters of 0.120-molar Ba(OH)₂?

(A) 20.0 mL
(B) 30 0 mL
(C) 40.0 mL
(D) 60.0 mL
(E) 80.0 mL

1)Mercury (II) hydroxide is quite insoluble in water (K_sp of Hg(OH)₂ = 3.0Ã10^-26 at 25Â°C.In which one of the following solutions would you expect Hg(OH)₂ to be even less soluble than it is in pure water? Why?

(a) 0.1 M NaCl (b) 0.1 M HCl (c) 0.1 M NaOH (d) 0.1 M NaCN

2)How will the solubility of calcium fluoride differ in acidic water compared to neutral water? Why?

(a) It will be more soluble in acidic water

(b) It will be less soluble in acidic water

Calculate the K_sp for Mg₃(PO₄)₂, given that its molar solubility is 3.57Â·10^-6 mol/L.

BMB 200 Study Guide - Midterm Guide: Essential Amino Acid, N-Terminus, Zwitterion

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