To find x, we need to calculate the mass of water lost during heating, and to find the experimental mass percent of water in the hydrate, we need to compare the mass of water lost to the total mass of the hydrate.
First, let's find the mass of water lost during heating:
Mass of washing soda (Na2CO3 X xH2O) = 2.714 g
Mass of anhydrous sodium carbonate (Na2CO3) after heating = 1.006 g
To calculate the mass of water lost, we subtract the mass of anhydrous sodium carbonate from the initial mass of washing soda:
Mass of water lost = Mass of washing soda - Mass of anhydrous sodium carbonate
= 2.714 g - 1.006 g
= 1.708 g
Now, to find x, we need to determine the number of moles of water lost and the number of moles of anhydrous sodium carbonate:
The molar mass of water (H2O) = 2 * atomic mass of hydrogen + atomic mass of oxygen
= 2 * 1 g/mol + 16 g/mol
= 18 g/mol
The molar mass of anhydrous sodium carbonate (Na2CO3) = 2 * atomic mass of sodium + atomic mass of carbon + 3 * atomic mass of oxygen
= 2 * 23 g/mol + 12 g/mol + 3 * 16 g/mol
= 106 g/mol
Now, we can calculate the number of moles of water lost:
Number of moles of water = Mass of water lost / molar mass of water
= 1.708 g / 18 g/mol
≈ 0.095 moles
Similarly, we can calculate the number of moles of anhydrous sodium carbonate:
Number of moles of sodium carbonate = Mass of anhydrous sodium carbonate / molar mass of anhydrous sodium carbonate
= 1.006 g / 106 g/mol
≈ 0.0095 moles
The ratio between the number of moles of water lost and the number of moles of anhydrous sodium carbonate gives us the value of x in the formula Na2CO3 X xH2O:
x = number of moles of water lost / number of moles of anhydrous sodium carbonate
= 0.095 moles / 0.0095 moles
= 10
Therefore, x = 10.
Now, let's calculate the experimental mass percent of water in the hydrate:
Experimental mass percent of water = (Mass of water lost / Mass of washing soda) * 100
= (1.708 g / 2.714 g) * 100
≈ 63.05%
Therefore, the experimental mass percent of water in the hydrate is approximately 63.05%.