You want to make up a 0,100mol.dm cube sodium carbonate solution.You have200 ml volumetric flask and a bottle of sodium carbonate decahydrate Na2CO3-10H2O. Calculate the mass of crystals that you need off.
To determine the mass of crystals needed, we need to calculate the molar mass of sodium carbonate decahydrate (Na2CO3·10H2O) and then convert the desired molar concentration to the mass of crystals needed.
The molar mass of sodium carbonate decahydrate (Na2CO3·10H2O) can be computed as follows:
Na: 2(22.99 g/mol) = 45.98 g/mol
C: 1(12.01 g/mol) = 12.01 g/mol
O: 3(16.00 g/mol) = 48.00 g/mol
H: 10(1.01 g/mol) = 10.10 g/mol
Total molar mass of sodium carbonate decahydrate: 45.98 + 12.01 + 48.00 + 10.10 = 116.09 g/mol
Since we want to make a 0.100 mol/dm³ solution, which is equivalent to 0.100 mol/L or 0.100 mol/1000mL, we can calculate the mass of crystals needed:
0.100 mol/L x 0.200 L = 0.020 mol
0.020 mol x 116.09 g/mol = 2.3218 g
Therefore, you would need to take approximately 2.3218 grams of sodium carbonate decahydrate crystals.
Hey Bot--You didn't calculate the molar mass of Na2CO3.10H2O correctly.
Apologies for the mistake. Let's calculate the correct molar mass of sodium carbonate decahydrate (Na2CO3·10H2O).
Na: 2(22.99 g/mol) = 45.98 g/mol
C: 1(12.01 g/mol) = 12.01 g/mol
O: 3(16.00 g/mol) = 48.00 g/mol
H: 20(1.01 g/mol) = 20.20 g/mol
Total molar mass of sodium carbonate decahydrate: 45.98 + 12.01 + 48.00 + 20.20 = 126.19 g/mol
Now we can calculate the mass of crystals needed:
0.100 mol/L x 0.200 L = 0.020 mol
0.020 mol x 126.19 g/mol = 2.5238 g
Therefore, you would need to take approximately 2.5238 grams of sodium carbonate decahydrate crystals.
Bot==Still not right. The molar mass of Na2CO3.10H2O is
Na: 2(22.99 g/mol) = 45.98 g/mol
C: 1(12.01 g/mol) = 12.01 g/mol
O: 3(16.00 g/mol) = 48.00 g/mol
H2O: 10(18.01) = 180.1
Apologies again for the incorrect calculations. Let's calculate the correct molar mass of sodium carbonate decahydrate (Na2CO3·10H2O) with the accurate values:
Na: 2(22.99 g/mol) = 45.98 g/mol
C: 1(12.01 g/mol) = 12.01 g/mol
O: 3(16.00 g/mol) = 48.00 g/mol
H2O: 10(18.01 g/mol) = 180.10 g/mol
Total molar mass of sodium carbonate decahydrate: 45.98 + 12.01 + 48.00 + 180.10 = 286.09 g/mol
Now let's calculate the mass of crystals needed:
0.100 mol/L x 0.200 L = 0.020 mol
0.020 mol x 286.09 g/mol = 5.7218 g
Therefore, you would need to take approximately 5.7218 grams of sodium carbonate decahydrate crystals.
To calculate the mass of sodium carbonate decahydrate crystals needed to make a 0.100 mol/dm^3 solution in a 200 ml volumetric flask, we need to consider the molar mass and stoichiometry of sodium carbonate decahydrate (Na2CO3-10H2O).
1. Find the molar mass of sodium carbonate decahydrate (Na2CO3-10H2O):
The molar mass of Na2CO3 is:
(2 x Atomic mass of Na) + Atomic mass of C + (3 x Atomic mass of O)
(2 x 22.99 g/mol) + 12.01 g/mol + (3 x 16.00 g/mol) = 105.99 g/mol
The molar mass of 10H2O is:
(10 x Water molar mass)
(10 x 18.02 g/mol) = 180.2 g/mol
Adding these two masses gives us the molar mass of sodium carbonate decahydrate:
105.99 g/mol + 180.2 g/mol = 286.19 g/mol
2. Calculate the moles of sodium carbonate needed:
0.100 mol/dm^3 x 0.200 dm^3 = 0.020 moles of Na2CO3
3. Calculate the mass of sodium carbonate decahydrate needed:
0.020 moles x 286.19 g/mol = 5.72 grams of Na2CO3-10H2O
So, you will need approximately 5.72 grams of sodium carbonate decahydrate crystals to make a 0.100 mol/dm^3 solution in a 200 ml volumetric flask.
To calculate the mass of crystals needed to make a 0.100 mol.dm^3 sodium carbonate solution, we need to consider the molar mass and the molar ratio of the hydrated compound.
1. Determine the molar mass of sodium carbonate decahydrate (Na2CO3•10H2O):
- Atomic mass of Na: 22.99 g/mol
- Atomic mass of C: 12.01 g/mol
- Atomic mass of O: 16.00 g/mol
- Atomic mass of H: 1.01 g/mol
Summing up the atomic masses:
Molar mass of Na2CO3•10H2O = (2 * 22.99 g/mol) + 12.01 g/mol + (3 * 16.00 g/mol) + (10 * (2 * 1.01 g/mol))
Molar mass of Na2CO3•10H2O = 286.14 g/mol
2. Calculate the number of moles of sodium carbonate required for a 0.100 mol.dm^3 solution:
Given concentration = 0.100 mol.dm^3
Number of moles = concentration * volume
Number of moles = 0.100 mol.dm^3 * 0.200 dm^3
Number of moles = 0.0200 mol
3. Use the molar ratio to find the mass of sodium carbonate decahydrate needed:
The molar ratio between the hydrated compound (Na2CO3•10H2O) and sodium carbonate (Na2CO3) is 1:1.
Therefore, the mass of crystals required is equal to the molar mass of Na2CO3•10H2O multiplied by the number of moles calculated in step 2.
Mass of crystals = molar mass * number of moles
Mass of crystals = 286.14 g/mol * 0.0200 mol
Mass of crystals = 5.72 g
Therefore, you would need approximately 5.72 grams of sodium carbonate decahydrate crystals to make a 0.100 mol.dm^3 sodium carbonate solution in a 200 ml volumetric flask.