Question

A 20 ml sample of 0.200 M potassium carbonate is added to 30,0 mL of 0.400 barium nitrate. barium carbonate precipitates. calculate the concentration of barium ions when precipitation is complete. assume reactions is 100% efficient.

Answer 1

Answer: The concentration of barium ions is 0.24 M

Step-by-step explanation:

To calculate the number of moles for given molarity, we use the equation:

`\text{Molarity of the solution}=\frac{\text{Moles of solute}* 1000}{\text{Volume of solution (in mL)}}` .....(1)

• For barium nitrate:

Molarity of barium nitrate solution = 0.200 M

Volume of solution = 20 mL

Putting values in equation 1, we get:

`0.200M=\frac{\text{Moles of barium nitrate}* 1000}{20}\\\\\text{Moles of barium nitrate}=(0.200* 20)/(1000)=0.04mol`

• For potassium carbonate:

Molarity of potassium carbonate solution = 0.400 M

Volume of solution = 30.0 mL

Putting values in equation 1, we get:

`0.400M=\frac{\text{Moles of potassium carbonate}* 1000}{30}\\\\\text{Moles of potassium carbonate}=(0.400* 30)/(1000)=0.012mol`

The chemical equation for the reaction of potassium carbonate and barium nitrate follows:

`K_2CO_3(aq.)+Ba(NO_3)_2(aq.)\rightarrow BaCO_3(s)+2KNO_3(aq.)`

By Stoichiometry of the reaction:

1 mole of potassium carbonate reacts with 1 mole of barium nitrate

So, 0.012 moles of potassium carbonate will react with =
`(1)/(1)* 0.012=0.012mol` of barium nitrate

As, given amount of barium nitrate is more than the required amount. So, it is considered as an excess reagent.

Thus, potassium carbonate is considered as a limiting reagent because it limits the formation of product.

By Stoichiometry of the reaction:

1 mole of potassium carbonate produces 1 mole of barium carbonate

So, 0.012 moles of potassium carbonate will produce =
`(1)/(1)* 0.012=0.012mol` of barium carbonate

The chemical equation for the ionization of barium carbonate follows:

`BaCO_3\rightarrow Ba^(2+)+CO_3^(2-)`

1 mole of barium carbonate produces 1 mole of barium ions and 1 mole of carbonate ions

Moles of barium ions = 0.012 moles

Volume of solution = (20 + 30) mL = 50 mL

Putting values in equation 1, we get:

`\text{Concentration of }Ba^(2+)\text{ ions}=(0.012* 1000)/(50)\\\\\text{Concentration of }Ba^(2+)\text{ ions}=0.24M`

Hence, the concentration of barium ions is 0.24 M