Answer:
[tex]Na_2CO_3.7H_2O[/tex]
Explanation:
Mass of the hydrated salt = x
Mass lost is 54.3% of x. So,
Mass of water lost = 0.543x
Mass of the dehydrated salt = x - 0.543x = 0.457 x
The moles of the dehydrated salt is :
Amount = 0.457 x
Molar mass of [tex]Na_2CO_3[/tex] = 106 g/mol
The formula for the calculation of moles is shown below:
[tex]moles = \frac{Mass\ taken}{Molar\ mass}[/tex]
Thus, moles are:
[tex]moles= \frac{0.457\times x}{106\ g/mol}[/tex]
[tex]moles= 0.004311\times x\ mol[/tex]
The moles of water is :
Amount = 0.543x
Molar mass of [tex]H_2O[/tex] = 18 g/mol
The formula for the calculation of moles is shown below:
[tex]moles = \frac{Mass\ taken}{Molar\ mass}[/tex]
Thus, moles are:
[tex]moles= \frac{0.543\times x}{18\ g/mol}[/tex]
[tex]moles= 0.030166\times x\ mol[/tex]
The simplest ration of the two are:
[tex]Na_2CO_3:H_2O[/tex] = 0.004311x : 0.030166x = 1 : 7
The formula is [tex]Na_2CO_3.7H_2O[/tex]
