Na2CO3 + xH2O
How do I work out the value of x when 2.558g of Na2CO3 loses 1.61g H2O upon heating at 125 degrees, leaving 0.948g Na2CO3?
The molar masses given are NaCO3=106.0 H2O=18.02

Na_2CO_3 + xH_2O

2.558g of Na_2CO_3 loses 1.61g H_2O upon heating at 125 degrees, leaving 0.948g Na_2CO_3?

The molar masses given are Na_CO_3=106.0\,\, H_2O=18.02


Na_2CO_3\cdot xH_2O = Na_2CO_3 + xH_2O

Note, you're starting from a hydrate going to the free molecules. For every molecule of Sodium Carbonate in the original hydrate, you get one mole of sodium carbonate (dry) + x moles of water. Start with the right side:

0.948 \, g \, Na_2CO_3 \,\div\, \frac {106.0\,g}{mole} =8.94\times 10^{-3}\,moles\,of\,Na_2CO_3

2.558\,g\,of\,hydrate - 0.948\,g\,of\,Na_2CO_3 = 1.61\,g\,of\,H_2O

1.61\,g\,of\,H_2O \,\div\, \frac {18.02\,g}{mole}=8.93\times 10^{-2}\,moles\,of\,H_2O

We take the number of moles of Na2CO3 and divide that into the number of moles of H2O:

\frac {x}{1} = \frac {8.93\times 10^{-2}}{8.94 \times 10^{-3}} \approx 10

We note that x will always be some small, integer. Thus, we can round off 9.9888143 \approx 10