The weight of H2C2O4.2H2O required to prepare 500 ml of 0.2N solution is
a)126g
b)12.6g
c)63g
d)6.3g
6.3
I want answer sir
To find the weight of H2C2O4.2H2O required to prepare a 500 ml of 0.2N (Normality) solution, we need to follow these steps:
Step 1: Calculate the molar mass of H2C2O4.2H2O.
The molar mass of H2C2O4.2H2O can be calculated by adding the individual atomic masses of its constituent elements. The atomic masses are as follows:
H (hydrogen) = 1 g/mol
C (carbon) = 12 g/mol
O (oxygen) = 16 g/mol
So, the molar mass of H2C2O4.2H2O can be calculated as:
(2*1 g/mol) + (2*12 g/mol) + (4*16 g/mol) + (2*1 g/mol) + (2*16 g/mol) = 126 g/mol.
Step 2: Calculate the number of moles of solute required.
To calculate the number of moles, we'll use the formula:
Number of moles = Normality (N) * Volume (in liters)
Here, the Normality (N) is 0.2N and the Volume is 500 ml, which is equivalent to 0.5 liters.
Number of moles = 0.2 * 0.5 = 0.1 moles.
Step 3: Calculate the weight of H2C2O4.2H2O required.
To calculate the weight of the compound, use the formula:
Weight = Number of moles * Molar mass
Weight = 0.1 moles * 126 g/mol = 12.6 grams.
So, the weight of H2C2O4.2H2O required to prepare 500 ml of 0.2N solution is 12.6 grams.
Therefore, the correct answer is option b) 12.6 g.