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Maksim231197 [3]
3 years ago
5

How do you compare the nuclear membrane and the cell membrane?

Chemistry
2 answers:
Mademuasel [1]3 years ago
8 0

ANSWER:

they're both protective covering, the nuclear membrane is a covering for the nucleas while the cell membrane is the covering for the whole cell the nucleus (which is the control center of the cell) decides what comes in and out of the cell.

~batmans wife dun dun dun...aka ~serenitybella

iragen [17]3 years ago
5 0
A. Both the cell membrane and the nuclear membrane are protective coverings.
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In the induced fit model of enzymes, a substrate associates itself with which part of an enzyme?
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Active site of the enzyme.

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3 years ago
Hydrobromic acid, HBr, is a strong acid. Hydrofluoric acid, HF, is a weak acid. If you prepared equal
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HBr and HF are both monoprotic Arrhenius acids—that is, in aqueous solution, they dissociate and ionize to give hydrogen ions. A strong acid ionizes completely; a weak acid ionizes partially.

In this case, HBr, being a strong acid, would ionize completely in water to yield H+ and Br- ions. However, HF, being a weak acid, would ionize only to a limited extent: some of the HF molecules will ionize into H+ and F- ions, but most of the HF will remain undissociated.

pH is, by definition, a measurement of the concentration of hydrogen ions in solution (pH = -log[H+]). A higher concentration of hydrogen ions gives a lower pH, while a lower concentration of hydrogen ions gives a higher pH. At 25 °C, a pH of 7 indicates a neutral solution; a pH less than 7 indicates an acidic solution; and a pH greater than 7 indicates a basic solution.

If we have equal concentrations of HBr and HF, then the HBr solution will have a greater concentration of hydrogen ions in solution than the HF solution. Consequently, the pH of the HBr solution will be less than the pH of the HF solution.

Choice A is incorrect: Strong acids like HBr dissociate completely, not partially.

Choice B is incorrect: While the initial concentration of HBr and HF are the same, the H+ concentration in the HBr solution is greater. Since pH is a function of H+ concentration, the pH of the two solutions cannot be the same.

Choice C is correct: A greater H+ concentration gives a lower pH value. The HBr solution has the greater H+ concentration. Thus, the pH of the HBr solution would be less than that of the HF solution.

Choice D is incorrect for the reason why choice C is correct.

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QUESTION 1 (POLL)
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They stay the same

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