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vagabundo [1.1K]
2 years ago
9

What is the effect of the presence of double bonds in plant lipids?

Biology
1 answer:
Anna71 [15]2 years ago
7 0

Answer: Option C.

C)the tails of plant lipids cannot pack as tightly together as animal ones

Explanation:

The tails of plant lipids cannot pack as tightly together as animal ones because the double bond in plant lipids make the hydrocarbon chains to bend making them no to pack tightly together which cause a reduction in van der Waals interaction between the fatty acids. The length of the double bond also affect the melting point of fatty acids . If the hydrocarbon chain is long, melting point will be high .

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Respiratory component :
2. Respiratory Component: The second line of dense is rapid consisting of the control the carbonic acid concentration in the ECF by changing the rate and depth of breathing by hyperventilation or hypoventilation. This blows off or retains carbon dioxide (and thus carbonic acid) in the blood plasma as required

3.Metabolic component : third line of defense is slow, best measured by the base excess,eand mostly depends on the renal system which can add or remove bicarbonate ions to or from the ECF.Bicarbonate ions are derived from metabolic carbon dioxide which is enzymatically converted to carbonic acid in the renal tubular cells.There, carbonic acid spontaneously dissociates into hydrogen ions and bicarbonate ions.When the pH in the ECF falls, hydrogen ions are excreted into urine, while bicarbonate ions are secreted into blood plasma, causing the plasma pH to rise.The converse happens if the pH in the ECF tends to rise: bicarbonate ions are then excreted into the urine and hydrogen ions into the blood plasma.




Buffers usually consist of a weak acid and its conjugate base; this enables them to readily absorb excess H+ or OH–, keeping the system’s pH within a narrow range.

Maintaining a constant blood pH is critical to a person’s well-being. The buffer that maintains the pH of human blood involves carbonic acid (H2CO3), bicarbonate ion (HCO3–), and carbon dioxide (CO2). When bicarbonate ions combine with free hydrogen ions and become carbonic acid, hydrogen ions are removed, moderating pH changes. Similarly, excess carbonic acid can be converted into carbon dioxide gas and exhaled through the lungs; this prevents too many free hydrogen ions from building up in the blood and dangerously reducing its pH; likewise, if too much OH– is introduced into the system, carbonic acid will combine with it to create bicarbonate, lowering the pH.
Example: Antacids, which combat excess stomach acid, are another example of buffers.


ECF =Extra cellular fluid




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<h2><u>A</u><u>nswer:</u></h2>

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