Question

suppose a solution containing 4.50g of sodium phosphate is mixed with a solution containing 3.75g of barium nitrate. how many grams of barium phosphate can be produced?

Answer 1

Answer:- The amount of barium phosphate that can be produced is 2.87 g.

Solution:- It's a stoichiometry problem. So, we need to write the balanced equation and do the calculations with the help of that.

the reaction is double replacement and takes place as:

`2Na_3PO_4(aq)+3Ba(NO_3)_2(aq)\rightarrow 6NaNO_3(aq)+Ba_3(PO_4)_2(s)`

Given, mass of sodium phosphate = 4.50 g

mass of barium nitrate = 3.75 g

Let's calculate the moles for both of these.

moles of sodium phosphate =
`4.50g((1mol)/(163.94g))`

moles of sodium phosphate = 0.0274

moles of barium nitrate =
`3.75g((1mol)/(261.34g))`

moles of barium nitrate = 0.0143

Now we will calculate the grams of barium phosphate using the calculated moles of each reactant and see which one gives limited amount of it.

Calculations for grams of barium phosphate from moles of sodium phosphate:

`0.0274mol Na_3PO_4((1mol Ba_3(PO_4)_2)/(2mol Na_3PO_4))((601.92g)/(1mol))`

= 8.25 g
`Ba_3(PO_4)_2`

Calculations for grams of barium phosphate from moles of barium nitrate:

`0.0143mol Ba(NO_3)_2((1mol Ba_3(PO_4)_2)/(3mol Ba(NO_3)_2))((601.92g)/(1mol))`

= 2.87 g
`Ba_3(PO_4)_2`

Barium nitrate gives the limited amount of barium phosphate. So, the amount of barium phosphate that can be produced is 2.87 g.