The solubility of #Ba(NO_3)_2# is 130.5 g/L at #0^o C#. How many moles of dissolved salt are present in 4.0 L of a saturated solution of #Ba(NO_3)_2# at #0^oC#?
1 Answer
Explanation:
The problem provides you with the solubility of barium nitrate,
The first thing to do here is recognize the fact that the solubility of barium nitrate tells you how many grams of the salt can be dissolved in one liter of water at
In this case, barium nitrate is said to have a solubility of
Use the compound's molar mass to convert the mass of barium nitrate to moles
#130.5 color(red)(cancel(color(black)("g"))) * ("1 mole Ba"("NO"_3)_2)/(261.34color(red)(cancel(color(black)("g")))) = "0.4993 moles Ba"("NO"_3)_2#
Now, you know that
#4.0 color(red)(cancel(color(black)("L water"))) * ("0.4993 moles Ba"("NO"_3)_2)/(1color(red)(cancel(color(black)("L water")))) = color(green)(|bar(ul(color(white)(a/a)color(black)("2.0 moles Ba"("NO"_3)_2)color(white)(a/a)|)))#
The answer is rounded to two sig figs, the number of sig figs you have for the volume of water.