Bioorganic Chemistry 2nd Assessment
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Questions and Answers

What is the value of [H+] when 0.1 M HAc and 0.1 M NaAc are mixed in a specific ratio?

  • $4.0 \times 10^{-5}$
  • $1.8 \times 10^{-5}$ (correct)
  • $3.0 \times 10^{-5}$
  • $2.4 \times 10^{-5}$

What happens to the buffer capacity as the concentration of the components increases?

  • It becomes negligible
  • It remains constant
  • It increases (correct)
  • It decreases

What is the relationship between pH and pKa when the concentrations of acid and conjugate base are equal?

  • pH < pKa
  • pH = pKa (correct)
  • pH > pKa
  • pH is unrelated to pKa

According to the Law of Bouguer – Lambert – Beer, absorbance is directly proportional to which factors?

<p>Sample path length and concentration (B)</p> Signup and view all the answers

What general formula represents alkanes?

<p>C_nH_{2n+2} (C)</p> Signup and view all the answers

Which of the following terms describes the process of separating components of a mixture?

<p>Chromatography (A)</p> Signup and view all the answers

What is pH given that [H+] equals $1.8 \times 10^{-5}$?

<p>4.744 (C)</p> Signup and view all the answers

In potentiometry, what is established when a metal plate is immersed in a solution?

<p>Electrode potential (B)</p> Signup and view all the answers

What is the general formula for alkenes?

<p>CnH2n (C)</p> Signup and view all the answers

What functional group characterizes alcohols?

<p>−OH (C)</p> Signup and view all the answers

Which of the following compounds is classified as an alkyne?

<p>Ethyne (B)</p> Signup and view all the answers

What is the proper nomenclature change for aldehydes?

<p>Replace the -e with -al (B)</p> Signup and view all the answers

Which of the following is an example of a carboxylic acid?

<p>Acetic acid (B)</p> Signup and view all the answers

What functional group do amines contain?

<p>−NH2 (C)</p> Signup and view all the answers

In the nomenclature of esters, how are they named?

<p>By naming the alkyl group from the alcohol followed by -ate (A)</p> Signup and view all the answers

What is the unique feature of aromatic hydrocarbons?

<p>They contain benzene rings (B)</p> Signup and view all the answers

What does an Arrhenius acid produce in water?

<p>Hydrogen ions (H+) (A)</p> Signup and view all the answers

Which of the following compounds is considered a strong electrolyte?

<p>HCl (D)</p> Signup and view all the answers

If the concentration of H3O+ is 0.001 M, what is the pH of the solution?

<p>3 (A)</p> Signup and view all the answers

In what type of solution does the pH change only slightly upon the addition of a strong acid or base?

<p>Buffer solutions (A)</p> Signup and view all the answers

What is the calculation for pOH given the hydroxide ion concentration of 0.01 M?

<p>2 (D)</p> Signup and view all the answers

Which combination correctly represents a Bronsted-Lowry acid and base?

<p>Acid donates protons; base accepts protons (B)</p> Signup and view all the answers

What does the pH+pOH equal in any aqueous solution?

<p>14 (A)</p> Signup and view all the answers

If a buffer solution contains 0.1 mol of acetic acid and 0.1 mol of sodium acetate, what type of species is present?

<p>Weak acid with its salt (A)</p> Signup and view all the answers

What is the pH of a solution with [H3O+] = 0.01 M?

<p>2 (C)</p> Signup and view all the answers

If the pOH of a solution is 2, what is the corresponding pH?

<p>12 (A)</p> Signup and view all the answers

How do you calculate [H3O+] from a pH of 4.68?

<p>[H3O+] = 2.1 * 10^-5 (D)</p> Signup and view all the answers

What is the pH of a solution where [H3O+] = 2.25 * 10^-5 M?

<p>4.678 (C)</p> Signup and view all the answers

Why are aldehydes generally more reactive than ketones?

<p>Aldehydes contain a carbonyl carbon attached to hydrogen. (D)</p> Signup and view all the answers

What determines the behavior of amino acids in acid or base solutions?

<p>Their amino and carboxyl groups. (D)</p> Signup and view all the answers

What is tautomerism?

<p>An equilibrium between different compounds. (B)</p> Signup and view all the answers

Which statement is true about peptide bond formation?

<p>They involve a condensation reaction between two amino acids. (A)</p> Signup and view all the answers

Which method can be used to produce soap?

<p>Strong base + fat or oil (A), Fat + oil (C)</p> Signup and view all the answers

What is the role of a strong acid when mixed with weak acid salts?

<p>Displaces the weak acid and creates a buffer solution (C)</p> Signup and view all the answers

What defines a polyhydric alcohol?

<p>Contains multiple hydroxyl groups (A)</p> Signup and view all the answers

Which is a characteristic of unsaturated fatty acids in oil?

<p>Makes the fat more fluid at room temperature (A)</p> Signup and view all the answers

What is the Arrhenius definition of a base?

<p>Produces hydroxide ions in water (B)</p> Signup and view all the answers

What reaction occurs to produce an ester from a carboxyl group and an alcohol?

<p>Esterification in presence of an acid catalyst (A)</p> Signup and view all the answers

What is the primary characteristic of keto-enol tautomerism?

<p>Migration of a hydrogen atom and shifting of a double bond (A)</p> Signup and view all the answers

How can the concentration of hydrogen ions ($[H_3O^+]$) be calculated from pH?

<p>[H3O+] = 10^-pH (A)</p> Signup and view all the answers

Which is a characteristic of a Lewis acid?

<p>Accepts a pair of electrons (A)</p> Signup and view all the answers

Which reaction demonstrates the weak acidic nature of carboxylic acids?

<p>CH3COOH + NaOH → CH3COONa + H2O (B)</p> Signup and view all the answers

Which of the following is an example of a polyfunctional carboxylic acid?

<p>Lactic acid (C)</p> Signup and view all the answers

What distinguishes dicarboxylic acids from monocarboxylic acids?

<p>Dicarboxylic acids contain two carboxyl groups (D)</p> Signup and view all the answers

Which of the following best describes hydroxyl carboxylic acids?

<p>They contain both hydroxyl and carboxyl functional groups. (C)</p> Signup and view all the answers

What defines a chiral molecule?

<p>It has a carbon atom bonded to four different groups. (A)</p> Signup and view all the answers

Which of the following is NOT a type of acid mentioned?

<p>Hydroxyl acid (D)</p> Signup and view all the answers

Which chemical reaction is associated with decarboxylation?

<p>Malonic acid to acetic acid and CO2 (D)</p> Signup and view all the answers

Flashcards

Acid (Arrhenius)

A substance that produces hydrogen ions (H+) in water.

Base (Arrhenius)

A substance that produces hydroxide ions (OH-) in water.

pH

A measure of the concentration of hydrogen ions (H+) in a solution, ranging from 0 to 14.

pH calculation

Calculated using the formula: pH = -log[H+]

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Electrolyte

A substance that dissolves in water and conducts electricity.

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Buffer solution

A solution that resists changes in pH when small amounts of acid or base are added.

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Dissociation constant (Ka)

A measure of the extent to which a weak acid dissociates into ions in water.

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Buffer composition

Consists of a weak acid and its conjugate base or a weak base and its conjugate acid.

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Buffer Capacity

The amount of acid or base a buffer can withstand without significantly changing its pH.

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Buffer Range

The pH range over which a buffer works effectively.

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pH of a Buffer

The calculation of pH when dealing with a buffer solution, using the Henderson-Hasselbalch equation

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Spectroscopy

The analysis of the interaction between matter and electromagnetic radiation to determine structure or chemical changes.

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Law of Beer-Lambert

Absorbance of light is directly proportional to the concentration and path length of the sample.

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Potentiometry

Electrochemical method for measuring potential differences without current flow.

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Chromatography

Method to separate components of a mixture based on different interactions with the stationary and mobile phases.

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Alkanes

Organic compounds with only single bonds, no functional groups; also called saturated hydrocarbons.

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Alkynes General Formula

The general formula for alkynes is CnH2n−2, where 'n' represents the number of carbon atoms in the molecule.

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Alcohol Functional Group

The functional group in alcohols is -OH, often called the hydroxyl group.

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Ether Functional Group

Ethers contain an oxygen atom bonded to two carbon atoms, represented as -O-.

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Aldehyde Functional Group

Aldehydes have a carbonyl group (-CHO) at the end of the carbon chain.

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Amine Functional Group

Amines have nitrogen atoms bonded to one or more carbon atoms, represented by -NH2 or similar structures.

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Aromatic Hydrocarbons

These contain benzene rings, examples include benzene and toluene.

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Ketone Functional Group

Ketones have a carbonyl group (C=O) located within the carbon chain.

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Ester Functional Group

Esters have a functional group represented as -COOR, with an oxygen joining the carbonyl carbon to an alkyl group.

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Sulfide bridge

A covalent bond formed between the sulfur atoms of two cysteine amino acids.

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Polyhydric alcohols

Alcohols containing multiple hydroxyl (-OH) groups. They can react with copper (II) to form a bright blue complex or reduce copper (II) to copper (I) or copper metal.

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Arrhenius acid

A substance that produces hydrogen ions (H+) when dissolved in water.

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Arrhenius base

A substance that produces hydroxide ions (OH-) when dissolved in water.

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Brønsted-Lowry acid

A substance that donates protons (H+) to another substance.

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Brønsted-Lowry base

A substance that accepts protons (H+) from another substance.

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Lewis acid

A substance that accepts an electron pair.

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Lewis base

A substance that donates an electron pair.

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Keto-enol tautomerism

A reversible chemical equilibrium between a ketone (or aldehyde) and its enol form. This happens due to the migration of a hydrogen atom and the shifting of a double bond.

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Carboxylic acid properties

Carboxylic acids are weakly acidic, meaning they donate H+ ions in solution. They react with bases to form carboxylate salts, releasing water. For example, CH3COOH + NaOH → CH3COONa + H2O.

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Carboxylic acid preparation

Carboxylic acids can be prepared by oxidizing primary alcohols and aldehydes.

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Polyfunctional carboxylic acids

These acids have extra functional groups like hydroxyl (-OH) or keto (=O) attached to the molecule. Examples include lactic acid and citric acid.

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Heterofunctional carboxylic acids

These acids have different functional groups, like carboxyl and amino groups. Oxo acids, like pyruvic acid, are important in metabolic pathways.

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Dicarboxylic acids

Dicarboxylic acids have two carboxylic acid groups. Examples include saturated oxalic acid and succinic acid, and unsaturated maleic and fumaric acids.

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Dicarboxylic acid reactions

Dicarboxylic acids can undergo decarboxylation (losing CO2), salt formation (with bases), and ester formation (with alcohols). These reactions occur at either one or both carboxyl groups.

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Chirality

A molecule is chiral if it has a carbon atom bonded to four different groups. These molecules exist as non-superimposable mirror images called enantiomers.

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Calculating [H3O+]

The process of determining the hydronium ion concentration [H3O+] from a given pH value by reversing the pH calculation; [H3O+] = 10^(-pH).

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What makes a phospholipid head polar?

Phospholipid heads are polar due to the presence of a phosphate group and the attached functional group.

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Peptide Bond Formation

The formation of a peptide bond between two amino acids occurs through a condensation reaction involving the carboxyl group of one amino acid and the amino group of another.

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Tautomerism

A type of isomerism involving the rapid interconversion of two isomers, called tautomers, through migration of a hydrogen atom and a shift in the position of a double bond.

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Amino Acid Behavior in Solutions

Amino acids are amphoteric, meaning they can act as both acids and bases, depending on the pH of the solution. Their behavior is determined by the ionization of their amino and carboxyl groups.

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Study Notes

Bioorganic Chemistry 2nd Assessment

  • Acids and Bases:

    • Arrhenius: Acids donate hydrogen ions (H+) in water; bases donate hydroxide ions (OH-) in water.
    • Brønsted-Lowry: Acids are proton donors; bases are proton acceptors.
    • Lewis: Acids accept electron pairs; bases donate electron pairs.

  • Electrolytes and Non-Electrolytes:

    • Electrolytes: Compounds that break into ions and conduct electricity in solutions. Examples include HCl, NaCl, H₂SO₄, KOH, salts.
    • Non-Electrolytes: Compounds that do not break into ions and do not conduct electricity in solutions. Examples include CO₂, alcohols, sugars, organic solvents.

Dissociation Constant, Hydrogen Ions, and pH Calculations

  • pH 7: Concentration of H₃O⁺ = OH⁻
  • pH below 7: Higher concentration of H₃O⁺ than OH⁻.
  • pH above 7: Higher concentration of OH⁻ than H₃O⁺.
  • pH Calculation: pH = -log[H₃O⁺]
  • pOH Calculation: pOH = -log[OH⁻]
  • pH + pOH = 14.00
  • [H₃O⁺] Calculation: [H₃O⁺] = 10⁻ᵖᴴ

Buffer Solutions

  • Buffer solutions: Solutions that resist changes in pH upon addition of small amounts of strong acid or base.
  • Buffer composition: Contains a weak acid and its conjugate base (or a weak base and its conjugate acid).
  • Buffer Capacity: Buffer capacity is affected by the concentrations of acid and conjugated base components. Increasing concentrations results in a higher buffer capacity.

Spectroscopy and Law of Bouguer-Lambert-Beer

  • Spectroscopy: Branch of physics that studies absorption or scattering of electromagnetic radiation.
  • Law of Bouguer-Lambert-Beer: The sample path length (and concentration) is directly proportional to absorbance of light.

Functional Groups in Organic Compounds

  • Hydrocarbons (No functional group):

    • Alkanes: Contain only single bonds (CnH₂n+₂).
    • Alkenes: Contain one or more double bonds (CnH₂n).
    • Alkynes: Contain one or more triple bonds (CnH₂n-₂).
    • Aromatic Hydrocarbons: Contain benzene rings (e.g., benzene C₆H₆, toluene C₇H₈).

  • Compounds with Oxygen Functional Groups:

    • Alcohols: Contain the -OH (hydroxyl) group (e.g., ethanol CH₃CH₂OH).
    • Phenols: Contain -OH group attached to an aromatic ring (e.g., phenol C₆H₅OH).
    • Ethers: Contain -O- (e.g., diethyl ether CH₃CH₂OCH₂CH₃).
    • Aldehydes: Contain the -CHO (aldehyde) group at the end of the chain (e.g., formaldehyde HCHO, acetaldehyde CH₃CHO).
    • Ketones: Contain the -CO- (carbonyl) group within the chain (e.g., acetone CH₃COCH₃).
    • Carboxylic Acids: Contain the -COOH (carboxyl) group (e.g., acetic acid CH₃COOH).
    • Esters: Contain the -COOR group (e.g., ethyl acetate CH₃COOCH₂CH₃).

  • Compounds with Nitrogen Functional Groups:

    • Amines: Contain -NH₂, -NHR, -NR₂ (e.g., methylamine CH₃NH₂, dimethylamine (CH₃)₂NH).
    • Amides: Contain -CONH₂, -CONHR, -CONR₂ (e.g., acetamide CH₃CONH₂).
    • Nitro Compounds: Contain the -NO₂ group (e.g., nitrobenzene C₆H₅NO₂).

  • Compounds with Halogen Functional Groups: -General formula: R-X (where X = F, Cl, Br, I).

  • Compounds with Sulfur Functional Groups:

    • Thiols: Contain -SH group.
    • Sulfides: Contain -S-S- bond.

  • Compounds with Phosphorus Functional Groups:

    • Example: Organophosphates like ATP.

Lipids, Fatty Acids, and Other Topics

  • Lipids: Organic compounds containing hydrocarbons
  • Fatty Acids: Carbon chains with a methyl group at one end and a carboxyl group at the other. Can be saturated or unsaturated.
  • Triacylglycerols (Triglycerides): Fats and oils formed by esterification.
  • Amino Acids: Building blocks of proteins, containing an amino group (-NH₂) and a carboxyl group (-COOH).
  • Essential Amino Acids: Amino acids that cannot be synthesized by the body and must be obtained from the diet.

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Bioorganic Chemistry 2nd Assessment PDF

Description

Test your knowledge on acids, bases, electrolytes, and pH calculations in Bioorganic Chemistry. This assessment covers definitions, properties, and equations critical to understanding these concepts. Prepare to tackle questions on both theoretical and practical applications.

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