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Acid-Base Equilibria Questions and Answers
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Acid-Base Equilibria Questions and Answers Bronsted-Lowry Acid & Base: -Bronsted-Lowry Acid is the proton donor -Bronsted-Lowry Base is the proton acceptor Conjugate Acid & Base: -Conjugate Acid is formed from a Bronsted-Lowry Base accepting a proton -Conjugate Base is formed from a...

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  • October 2, 2024
  • 31
  • 2024/2025
  • Exam (elaborations)
  • Questions & answers

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  • acid base equilibria questions and answers
  • bronsted lowry acid base bronsted lowry acid
  • an arrhenius acid can be identified because their

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Acid-Base Equilibria Questions and
Answers
Bronsted-Lowry Acid & Base:

-Bronsted-Lowry Acid is the proton donor
-Bronsted-Lowry Base is the proton acceptor

Conjugate Acid & Base:

-Conjugate Acid is formed from a Bronsted-Lowry Base accepting a proton
-Conjugate Base is formed from a Bronsted-Lowry Acid donating a proton

Lewis Acid & Base:

-Lewis Acid is an electron pair acceptor
-Lewis Base is an electron pair donor

Arrhenius Acid & Base:

-Acid produces an excess of H+ ions when it dissociates in an aqueous solution
-Base produces an excess of OH- ions when it dissociates in an aqueous solution -
answer Describe the differences between the following pairs:

-Bronsted-Lowry Acid & Bronsted-Lowry Base

-Conjugate Acid & Conjugate Base

-Lewis Acid & Lewis Base

-Arrhenius Acid & Arrhenius Base

An Arrhenius acid can be identified because their formula begins with an H.

An Arrhenius base can be identified because their formula ends with an OH. - answer
How can you identify whether or not an acid or base is an Arrhenius one?

An aqueous solution that resists changes in pH upon the addition of an acid or base.

It is made either from a weak acid and its salt, which consists of the conjugate base and
a cation, or from a weak base and its salt, which consists of the conjugate acid and an
anion. - answer What is a buffer solution?

,How is a buffer solution made?

If a strong base is added, the acid in the buffer will neutralize the OH- ions.

If a strong acid is added, the base in the buffer will neutralize the H3O+ ions. - answer
What will happen if a strong base is added to a buffer solution? What about a strong
acid?

10:1
1:10 - answer A buffer is considered to be effective when the HA/A- ratio ranges
anywhere between __________ or _____________

By increasing the number of moles of the buffer in comparison to the moles of the
strong acid/base. - answer How can the effectiveness of a buffer be strengthened?

Bicarbonate buffer system - answer The ________________ is a system in our
blood that helps us maintain a physiological level of pH using carbonic acid and
bicarbonate ions

Bicarbonate ions (HCO3-)
Carbonic acid (H2CO3)
Acidic

Carbonic acid (H2CO3)
Bicarbonate ions (HCO3-)
Basic - answer When an acidic substance enters our blood stream, the
________________ neutralizes the H3O+ ions, forming ________________ and water.
This prevents the blood from becoming _________________.


When a basic substance enters our blood stream, the ______________________
neutralizes the OH- ions, forming _________________ and water. This prevents the
blood from becoming __________________.

The bicarbonate buffer system. - answer The reaction shown is an example of what?

Stop working
Denature
Disable - answer If our blood reaches a pH below physiological pH, the cells of our
body will _______ _________________. Enzymes will _________________, which will
___________ their catalytic abilities

100% ionization
Right-side

,Products - answer When a strong acid/base undergoes equilibria, it undergoes
_________________, which means that the total concentration of the acid turns into
products.

Because of this, equilibrium will lean to the __________-side of the reaction, favoring
the _______________.

Conjugate base

Conjugate acid - answer The stronger the acid, the weaker the _______________
will be.

The stronger the base, the weaker the ______________ will be.

Ionization
Protonated
Left-side
Reactants - answer When a weak acid undergoes equilibria, it does not undergo
complete _______________. Weak acids are not able to donate their protons well, so it
will stay mostly _______________.

Because of this, equilibrium will lean towards the __________-side of the reaction, in
favoring the ________________.

Greater

Less - answer A solution would be considered acidic if the concentration of
hydronium ions is _____________ than the concentration of hydroxide ions.

A solution would be considered basic if the concentration of hydronium ions is
_____________ than the concentration of hydroxide ions.

Less than

Greater than - answer A solution would be acidic if it had a pH that is ________ than
7.

A solution would be basic if it had a pH that is _______________ than 7

[H3O+]

[OH-] - answer In acid-base calculations:

pH = -log_______

pOH = -log_______

, 14 - answer In acid-base calculations:

pH + pOH = _________

Strong acids - answer Examples of __________ ____________ includes the
following:

-HClO4 (perchloric acid)
-HCl (hydrochloric acid)
-HBr (hydrobromic acid)
-HI (hydroiodic acid)
-H2SO4 (sufuric acid)
-HNO3 (nitric acid)

Strong bases - answer Examples of __________ ___________ includes the
following:

-NaOH (sodium hydroxide)
-KOH (potassium hydroxide)
-Ca(OH)2 (calcium hydroxide)
-Mg(OH2) (magnesium hydroxide)

Weak acids - answer Examples of ___________ ____________ includes the
following:

-HF (hydrofluoric acid)
-CH3COOH (acetic acid)
-CH3OH (methanol)

Weak bases - answer Examples of ____________ ____________ includes the
following:

-NH3 (ammonia)
-C6H5NH2 (aniline)

Stronger

Stronger - answer The higher the Ka, the ____________ the acid.

The higher the Kb, the _____________ the base.

Lower

Higher - answer The ____________ the pKa, the stronger the acid.

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