Acids and Bases II | Chemistry | Quiz

A hydronium ion is:

Negatively charged

Able to act as a base

Is created when water takes on a proton

All of the above
In a solution where a reversible reaction is at equilibrium, both the forward and reverse reactions:

Speed up

Slow down

Stop

Continue at the same rate
In a container of pure water at equilibrium:

There are water molecules, hydronium ions, and hydroxide ions

There are only water molecules and hydronium ions

There are only water molecules

There are only hydroxide ions and hydronium ions
From this equilibrium reaction: H3PO4 + H2O <-> H3O+ + H2PO4 <-> H3O+ + HPO4 2 We can see that:

H2PO4 is a strong acid

H2PO4 is amphoteric

Water is a strong base

H3PO4 is amphoteric.
In the reaction: CH3COOH + H¬2O <-> CH¬3COO + H3O+ CH¬3COO is:

A conjugate acid

A conjugate base

In equilibrium with H3O+

Acting as a proton
6. Once 5 moles of hydroiodic acid, HI, is mixed into 1L water, there are only products, and no HI remains. HI -> H3O+ + I- We consider HI to be a strong acid because:

H3O+ is created by the dissociation of HI

The concentration of H3O+ will be 5 molar

All the HI dissociates.

The HI and I- are in equilibrium
The equilibrium reaction: H3O+ <-> H2O <-> H+ + OH- is important to acid-base chemistry because:

Acid base reactions are always equilibrium reactions

Acids and bases are only found in water

Water determines the pH of a solution

It shows how water can act as both an acid and a base
According to the Bronsted-Lowry definition, NH¬3 is:

A base, because, when it is mixed with water, an OH- ion is created in the resulting solution

A base, because it accepts an H+ ion

An acid, because water donates an H+ ion

An acid, because it contains three hydrogen atoms
9. While studying the acid-base reactions of the bicarbonate system, Danish chemist Soren Sorenson noticed that adding a weak acid and its sodium salt made a solution that resists changes in pH. What explains this buffering phenomenon?

The weak acid does not change the pH of the water to any significant degree

The dissolved salt of the weak acid releases a weak conjugate base which can absorb excess protons

The dissolved salt of the weak acid releases a positive ion that acts as a base and can absorb excess protons

The dissolved sodium of the salt exists in equilibrium with any added protons.
Sorenson’s work helped Henderson understand what about the bicarbonate system in the body?

That bicarbonate is a weak acid

That bicarbonate ions, as the weak conjugate base of carbonic acid, and can absorb protons released by bodily processes.

That the bicarbonate system is an equilibrium between carbonic acid, bicarbonate ions, and carbonate ions.

That carbonic acid exists in the body in equilibrium with water