Acids and Bases (Lecture 7) Flashcards

1
Q

If Kc ≫ 1, where does the equilibrium lie?

A

to the right, and vice versa

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2
Q

In Kc calculations what is disregarded?

A

solids and pure liquids

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3
Q

What is Le Chatelier’s Principle?

A

“If a system at equilibrium is disturbed by a change in temperature, pressure, or the concentration of one of the components, the system will shift its equilibrium position so as to counteract the effect of the disturbance.”1

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4
Q

What is a Brønsted–Lowry acid?

A

a proton donor

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5
Q

What is a Brønsted–Lowry base?

A

a proton acceptor

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6
Q

How do acids behave in solution?

A

Acids dissociate in solution into a proton and a conjugate base.
Water acts as a Brønsted–Lowry base forming a hydronium ion.

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7
Q

What happens to strong acids and bases in aqueous solution?

A

They fully dissociate.

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8
Q

Is the conjugate base of a strong acid weak or strong?

A

The conjugate base of a strong acid shows negligible basicity.

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9
Q

Is the conjugate base of a a substance with negligible

acidity weak or strong?

A

The conjugate base of a substance with negligible acidity is a strong base.

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10
Q

Is the conjugate base of a weak acid weak or strong?

A

The conjugate base of a weak acid is a weak base.

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11
Q

In an acid base equilibrium, if water is a stronger base by far, what happens to the acid?

A

K&raquo_space; 1 and the acid is completely dissociated

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12
Q

In an acid base equilibrium, if water is less strong or equivalent to the conjugate base, what happens to the acid?

A

K < 1 and the acid is incompletely dissociated

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13
Q

What is the k value for a strong acid (in an acid base equilibrium)? How will it behave in solution?

A

K&raquo_space; 1 and it is completely dissociated in solution

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14
Q

In every acid/base reaction, what does the equilibrium favour?

A

The transfer of the proton from the stronger acid to the stronger base to form the weaker acid and the weaker base.

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15
Q

What is the prime indicator of acid strength?

A

the extent of dissociation

we use the dissociation constant Ka as a measure of acid strength

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16
Q

How are Ka and acid strength linked?

A

The larger the value of Ka the stronger the acid.