Table of contents

1. Introduction to Biochemistry4h 34m
2. Water3h 23m
3. Amino Acids8h 10m
4. Protein Structure10h 4m
5. Protein Techniques14h 5m
6. Enzymes and Enzyme Kinetics13h 38m
7. Enzyme Inhibition and Regulation 8h 42m
8. Protein Function 9h 41m
9. Carbohydrates7h 49m
10. Lipids5h 49m
11. Biological Membranes and Transport 6h 37m
12. Biosignaling9h 45m
Review 1: Nucleic Acids, Lipids, & Membranes2h 47m
Review 2: Biosignaling, Glycolysis, Gluconeogenesis, & PP-Pathway3h 12m
Review 3: Pyruvate & Fatty Acid Oxidation, Citric Acid Cycle, & Glycogen Metabolism2h 26m
Review 4: Amino Acid Oxidation, Oxidative Phosphorylation, & Photophosphorylation1h 48m

2. Water

Biochemistry

2. Water

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Multiple Choice

If two nutrient solutions are maintained at the same pH, which of the following statements is correct?

They must contain the same types and concentrations of dissolved salts.

They have identical buffering capacities.

They have the same concentration of hydrogen ions ($[H^+]$).

They have the same total ionic strength.

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Verified step by step guidance

Understand the concept of pH: pH is a measure of the concentration of hydrogen ions ($[H^+]$) in a solution. It is defined as $\text{pH} = -\log_{10}([H^+])$. Solutions with the same pH have the same $[H^+]$, regardless of other factors like dissolved salts or buffering capacity.

Clarify the role of dissolved salts: The types and concentrations of dissolved salts in a solution do not directly determine the pH. Salts may influence ionic strength or other properties, but pH is specifically tied to $[H^+]$. Therefore, solutions with the same pH do not necessarily have identical dissolved salts.

Explain buffering capacity: Buffering capacity refers to a solution's ability to resist changes in pH when acids or bases are added. Two solutions with the same pH may have different buffering capacities depending on the presence and concentration of buffer components (e.g., weak acids and their conjugate bases).

Discuss ionic strength: Ionic strength is a measure of the total concentration of ions in a solution, calculated as $I = \frac{1}{2} \sum c_i z_i^2$, where $c_i$ is the molar concentration of each ion and $z_i$ is its charge. Solutions with the same pH do not necessarily have the same ionic strength, as ionic strength depends on all ions present, not just $[H^+]$.

Conclude with the correct statement: The correct answer is that solutions with the same pH have the same concentration of hydrogen ions ($[H^+]$). This is the defining characteristic of pH and is independent of other solution properties like buffering capacity, dissolved salts, or ionic strength.