0.7g of a sample of Na2CO3.xH2O were dissoled in water and the volume made up to 100ml . 20ml of this solution
required 19.8ml of 0.1 N HCl for complete neutralization . Find the value of x .
ans = ~2
We will get the chemical equation to be:
Na2CO3. xH2O + 2HCl → 2NaCl + (x + 1)H2O + CO2
We calculate the strength of the given solution as 0.7/(100/1000) g/L = 7 g/L
Also, n1 M1 V1 =n2 M2 V2 ---(i)
n1 = acidity of Na2CO3 , M1= molarity of Na2CO3 solution and V1= volume of Na2CO3 solution
n2 = basicity of HCl , M2 = molarity of HCl and V2 = volume of HCl
As we know for monobasic substances, molarity= normality, so equation (i) becomes
2* M1 * 20= 1*0.1*19.8
⇒ M1 = 0.0495M
Molarity= strength / molar mass of solute
⇒ Molar mass= strength/ molarity
⇒ molar mass of Na2CO3. xH2O = 7/0.0495
⇒ molar mass of Na2CO3. xH2O = 141.414g
As, this molar mass= molar mass of Na2CO3 + mass of number of molecules of water in it
Molar mass of anhydrous Na2CO3 = 106
Molar mass of water= 18
So, 106+ 18x= 141.414
⇒x= 1.976≈ 2