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noname [10]
3 years ago
5

For an amino acid such as aspartic acid, what impact would you expect a neighboring carboxylic acid to have on the apparent pKa

value of the side chain?
Chemistry
1 answer:
tekilochka [14]3 years ago
7 0

Answer:

The apparent pKa value for aspartic acid increases

Explanation:

The apparent pKa value for aspartic acid increases.  Due to the presence of one negative in close proximity to another negative charge, it causes charge-to-charge repulsion which in turn leads to the increase in pKa values.

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I'm not 100% sure of the answer. Explanations are highly appreciated.
PolarNik [594]

Answer:

The correct answer is

B.

\Delta H=2(1072)+498 -4(799)

Explanation:

Enthalpy of reaction :

It is the amount of energy released/absorbed when one mole of the substance is formed from the reactant at a constant pressure.

The enthalpy of a reaction can be calculated using :

\Delta H=\Delta H_{reactants}-\Delta H_{products}

2CO+O_{2}\rightarrow 2CO_{2}

\Delta H_{reactants}=2(C\equiv O)+O=O

\Delta H_{reactants}=2(1072)+498

H_{products}=2(2\times C=O)

H_{products}=4\times 799

\Delta H=\Delta H_{reactants}-\Delta H_{products}

\Delta H=2(1072)+498 -4(799)

units = \frac{kJ}{mole}

Please note that :

The carbon monoxide , CO should be taken as C triple bond O. Not C=O .

So , the bond energy =1072 is used

\Delta H=2(1072)+498 -4(799)

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Answer:

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Hopefully this helps you!!!!

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