1.What is the concentration in mM of a solution that contains 100mL of water and

Question

1.What is the concentration in mM of a solution that contains 100mL of water and 60mg of acetic acid? (molecular weight of acetic acid is 60g/mol) _____________

2. The pKa of acetic acid is 4.75. This means that at pH 4.75, acetic acid will be:

Half-dissociated

Fully associated

Fully dissociated

Fully charged

3. The Henderson-Hasselbalch equation can help us:
Select one or more:

Figure out the pKa of a weak acid

Calculate pH of a solution based on the strength of the acid

Calculate the pH of a solution based on the pKa and ratio of the conjugate base and its weak acid

Mix a buffer to the desired pH using a weak acid and its conjugate base

All of the choices are correct

4. What is a hydrogen bond?

A bond between hydrogen and carbon in an hydrocarbon

A bond between hydrogen and oxygen in a water molecule

A covalent bond between a hydrogen bond donor and acceptor

A noncovalent interaction between a hydrogen bond donor and acceptor

Explanation / Answer

1.)

volume = 100 mL = 0.1 L

mass of acetic acid = 60 mg = 0.06 g

molar mass of acetic acid = 60 g/mol

moles of acetic acid = 0.06 / 60 = 0.001

Concentration = moles / volume

                        = 0.001 / 0.1

                        = 0.01 M

                        = 10 mM

Concentration = 10 mM

2) answer : fully dissociated

pH = pKa + log [salt/acid]

4.75 = 4.75 + log [salt/acid]

[salt/acid] = 1

so [salt] = [acid]

3) answer : All of the choices are correct

4) answer : A noncovalent interaction between a hydrogen bond donor and acceptor

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