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3 years ago

If hydrofluoric acid is a stronger acid than acetic acid, which statement is most likely true?

Chemistry

1 answer:

Alchen [17]3 years ago

4 0

Answer: The statement conjugate base of hydrofluoric acid is weaker than that of acetic acid is most likely true.

Explanation:

A strong acid upon dissociation gives a weak conjugate base. This can also be said as stronger is the acid, weaker will be its conjugate base or vice-versa.

Hydrofluoric acid is a strong base as it dissociates completely when dissolved in water.

For example, $HF \rightleftharpoons H^{+} + F^{-}$

The conjugate base is $F^{-}$ which is a weak base.

Acetic acid is a weak acid as it dissociates partially when dissolved in water. So, the conjugate base of acetic acid is a strong base.

$CH_{3}COOH \rightarrow CH_{3}COO^{-} + H^{+}$

Thus, we can conclude that the statement conjugate base of hydrofluoric acid is weaker than that of acetic acid is most likely true.

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Answer:

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Explanation:

Solution:

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Suspension:

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Aleksandr-060686 [28]

Explanation:

It is known that formula for area of a sphere is as follows.

A = $4 \pi r^{2}$

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= 3.14 $m^{2}$

$T_{a}$ = (27 + 273.15) K = 300.15 K

T = (77 + 273.15) K = 350.15 K

Formula to calculate the net charge is as follows.

Q = $esA(T^{4} - T^{4}_{a})$

where, e = emissivity = 0.85

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A = surface area

Hence, putting the given values into the above formula as follows.

Q = $esA(T^{4} - T^{4}_{a})$

= $0.85 \times 5.6703 \times 10^{-8} Wm^{-2} K^{-4} \times 3.14 \times ((350.15)^{4} - (300.15)^{4})$

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Answer:

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Explanation:

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MariettaO [177]

Answer:

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Explanation:

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