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1 year ago

How do the equations differ for the neutralization reaction between a strong acid/strong base and a weak acid/strong base

Chemistry

1 answer:

Hunter-Best [27]1 year ago

6 0

The dissociation of a weak acid/base in solution is not complete.

<h3>Strong acid and strong base</h3>

A strong acid is an acid that dissociates completely in solution. A strong base is a base that dissociates completely in solution.

A weak acid do not dissociate completely in solution and a weak base do not dissociate completely in solution.

The equation of the dissociation of a strong acid/base goes to completion while that of a weak acid or base is reversible with the equilibrium position lying closer to the left hand side.

Learn more about strong acids: brainly.com/question/9278149

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Answer:

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2 years ago

Suppose that a certain biologically important reaction is quite slow at physiological temperature (37 oC) in the absence of a ca

Oksi-84 [34.3K]

Answer:

30 kJ

Explanation:

Arrhenius equation is given by:

$k=Aexp(-Ea/RT)\\$

Here, k is rate constant, A is Pre-exponential factor, Ea is activation energy and T is temperature.

taking natural log of both side

ln k = ln A - Ea/RT

In Arrhenius equation, A, R and T are constant.

Therefore,

$ln\frac{k_2}{k_1} =\frac{Ea_1-Ea_2}{RT}$

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$\frac{k_2}{k_1} =1\times 10^5$

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3 years ago

A reasonable pka for a weak base is: 10.3 0.9 5.8 7.4 13.1

andriy [413]

Answer:

0.9

Explanation:

The pka represents the force by which the molecules need to dissociate for the acids ,

Hence , lower the pka stronger will be the acid and that therefore will dissociate completely and vice versa , for a weak acid higher the pka .

And in case of a base , it will be completely reversed , lower pKa , weaker base ,

and higher pKa , stronger base .

From the data of the question ,

0.9 is the lowest value of the pKa , hence , weakest base .

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