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Sagot :
Step 1 - Understanding how blood keeps its pH roughly constant
In our blood there's a buffering system. A buffering system consists of a group of molecules which can undergo reactions in presence of acids or bases, quickly consuming them.
When a solution is buffered, its pH can remain constant as long as we add small quantities of acid or bases. In our blood, the buffering involves the anion bicarbonate, HCO3(-), as well as carbonic acid, H2CO3.
In the presence of acids, HCO3(-) quickly neutralizes it:
[tex]\text{HCO}^-_3+H^+\to H_2CO3[/tex]In the presence of bases, it is H2CO3 who acts:
[tex]H_2CO_3+OH^-\to H_2O+HCO^-_3[/tex]Note that bicarbonate restitues carbonic acid, while carbonic acid restitutes bicarbonate. This way our blood remains its pH almost intact.
Step 2 - Choosing the right alternatives
The correct alternatives, based on what we have seen, are:
Blood can absorb small amounts of acids or bases without harmful effects
Blood contains buffers to help neutralize acids
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