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Help on bio hw (seems more like chem tho?)


Vivian

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I'm in bio but I have to do chem questions for hw... 

 

 

v = subscript 

^=superscript

 

 

The amino group reacts with Hv2O:

 

-NHv2 +Hv2O ---->      -NHv3^+ + OH^-

                      <--------

 

Is the amino group acidic or basic? Is it weak or strong?

 

 

 

Explanations would be nice b/c I do not get this at all.  :cry:  :cry:

 

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I'm in bio but I have to do chem questions for hw... 

 

 

v = subscript 

^=superscript

 

 

The amino group reacts with Hv2O:

 

-NHv2 +Hv2O ---->      -NHv3^+ + OH^-

                      <--------

 

Is the amino group acidic or basic? Is it weak or strong?

 

 

 

Explanations would be nice b/c I do not get this at all.  :cry:  :cry:

 

Shouldn't NH3+ be NH4+ if there's a superscript of "+"?  Otherwise, NH3 would have no charge (they should have only lone pairs). In any case, the amino group would be basic, since it has just deprotonated water, forming NH3 and H2O being deprotonated, forms the conjugate base of OH-.

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Shouldn't NH3+ be NH4+ if there's a superscript of "+"?  Otherwise, NH3 would have no charge (they should have only lone pairs). In any case, the amino group would be basic, since it has just deprotonated water, forming NH3 and H2O being deprotonated, forms the conjugate base of OH-.

It must be an error on the hw.

 

I also have another question:

If I have

-COOH ---->     H^+ + -COO^- 

            <--------

 

Would this be a partially ionized weak acid? If this is right, could you explain it like how you did with the previous question b/c that  helped a lot.

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It must be an error on the hw.

 

I also have another question:

If I have

-COOH ---->     H^+ + -COO^- 

            <--------

 

Would this be a partially ionized weak acid? If this is right, could you explain it like how you did with the previous question b/c that  helped a lot.

 

Yes, this would be a partially ionized weak acid, simply because ions of the weak acid (-COO^- and H+) tend to recombine to reform the molecules of the acid.  H^+ will react with -COO^- to form -COOH at the same time that -COOH is getting deprotonated, so that's why this is an equilibrium reaction and why -COOH is only partially ionized. In other words, -COOH is not a strong enough acid to drive the reaction almost to completion to produce mostly H+ and -COO^-.

Nitrogen bonds to three atoms to be neutral. Its not possible for it to be neutral as NH2

 

Yes, NH2 should have a "-" charge.

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Y'all are all freaking amazing. TYSM  :rlytearpls:  :rlytearpls:  :rlytearpls:  :rlytearpls:  :rlytearpls: 

 

Yes, this would be a partially ionized weak acid, simply because ions of the weak acid (-COO^- and H+) tend to recombine to reform the molecules of the acid.  H^+ will react with -COO^- to form -COOH at the same time that -COOH is getting deprotonated, so that's why this is an equilibrium reaction and why -COOH is only partially ionized. In other words, -COOH is not a strong enough acid to drive the reaction almost to completion to produce mostly H+ and -COO^-.


 

Yes, NH2 should have a "-" charge.

 

 

Nitrogen bonds to three atoms to be neutral. Its not possible for it to be neutral as NH2

 

 

the amino is basic : he is taking a H+

 

edit : but this equation is weird.

It is more NH2- + H2O = NH3 + OH-

or NH3 + H2O = NH4+ + H3O+

 

 

that amino is pretty strong

it has a negative charge which will strongly attract protons (H+)

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