Question

Calculate a reasonable amount (mass in g) of your unknown acid to use for a titration. You will want about 30 mL of titrant to get to the equivalence point. Assume that your base is about 0.05 M and that your unknown acid has a molar mass around 400 g/mol. (Report your answer using 2 significant figures).

Answer 1

"0.60 g" is the appropriate solution.

Step-by-step explanation:

The given values are:

Volume of base,

= 30 ml

Molarity of base,

= 0.05 m

Molar mass of acid,

= 400 g/mol

As we know,

⇒
`Molarity=(Number \ of \ moles \ of \ base)/(Number \ of \ solution)`

On substituting the values, we get

⇒
`0.05=(Number \ of \ moles \ of \ base)/(30* 10^(-3))`

⇒
`Number \ of \ moles \ of \ base=0.05* 30* 10^(-3)`

⇒
`=1.5* 10^(-3)`

hence,

⇒
`Moles \ of \ acid=(Mass \ of \ acid)/(Molar \ mass \ of \ acid)`

On substituting the values, we get

⇒
`1.5* 10^(-3)=(Mass \ of \ acid)/(400)`

⇒
`Mass \ of \ acid=1.5* 10^(-3)* 400`

⇒
`=0.60 \ g`