8.058g x 10-2 kg of washing soda na2co3 10h20 is dissolved in water to obtain 1L of a solution of density 1077.2kg/m3. Calculate the molarity, molality and mole fraction of na2c03 in the solution?

who helps

Well, well, well, it seems like you've stumbled upon the great Clown Bot for help! Fear not, for I shall answer your question with utmost humor and wit.

To calculate the molarity, my friend, we need to know the number of moles of Na2CO3 present. We can calculate this by dividing the mass of Na2CO3 by its molar mass. The molar mass of Na2CO3 is approximately 105.99 g/mol.

So, let's crunch some numbers! 8.058g x 10^-2 kg of Na2CO3 is equal to 8.058 x 10^-2 kg × (1000 g/1 kg) = 80.58 g.

Now, divide this mass by the molar mass of Na2CO3: 80.58 g / 105.99 g/mol. The result is approximately 0.7604 mol of Na2CO3.

Since we have 1 liter of solution, the molarity can be calculated by dividing the number of moles (0.7604 mol) by the volume in liters (1 L). So, the molarity is 0.7604 M.

Moving on to molality! Molality is calculated by dividing the number of moles of solute (0.7604 mol) by the mass of the solvent in kilograms. In this case, we have 10.772 kg of water, which is equal to 10.772 kg × (1000 g/1 kg) = 10772 g.

So, the molality is 0.7604 mol / 10.772 kg = 0.07056 mol/kg.

Lastly, let's find the mole fraction. The mole fraction of Na2CO3 can be calculated by dividing the number of moles of Na2CO3 by the sum of the moles of Na2CO3 and H2O.

The number of moles of H2O can be calculated by dividing the mass of water (10.772 kg) by its molar mass (18.015 g/mol). After crunching these numbers, we get approximately 597.7144 mol of water.

Now, divide the number of moles of Na2CO3 (0.7604 mol) by the sum of the moles of Na2CO3 and H2O (0.7604 mol + 597.7144 mol).

The mole fraction of Na2CO3 is 0.7604 mol / (0.7604 mol + 597.7144 mol) = 1.27 x 10^-3.

So, there you have it! The molarity of Na2CO3 is 0.7604 M, the molality is 0.07056 mol/kg, and the mole fraction is 1.27 x 10^-3. Now go forth and conquer your chemical calculations, my friend!

To calculate the molarity, molality, and mole fraction of Na2CO3 in the given solution, let's follow these steps:

Step 1: Convert the mass of Na2CO3 to moles.
- The given mass is 8.058g x 10^-2 kg.
- The molar mass of Na2CO3 is 105.99 g/mol.
- Convert the mass to grams: 8.058g x 10^-2 kg = 80.58g.
- Convert grams to moles: 80.58g / 105.99 g/mol = 0.759 moles.

Step 2: Calculate the volume of the solution.
- The given volume is 1L.

Step 3: Calculate the molarity.
- Molarity (M) is the moles of solute divided by the volume of solution in liters.
- Molarity (M) = Moles / Volume(L).
- M = 0.759 moles / 1L = 0.759 M.

Step 4: Calculate the molality.
- Molality (m) is the moles of solute divided by the mass of the solvent in kilograms.
- Molecular mass of H2O = 18.02 g/mol.
- Mass of solvent = density x volume.
- Mass of solvent = 1077.2 kg/m3 x 1L x (1000g/1kg) = 1077.2 g.
- Mass of solvent = 1077.2 g + (10 x 18.02 g) = 1257.2 g.
- Molality (m) = Moles / Mass of solvent (kg).
- Molality (m) = 0.759 moles / (1257.2 g x 1 kg/1000 g) = 0.603 m.

Step 5: Calculate the mole fraction.
- The mole fraction (X) is the moles of Na2CO3 divided by the total moles in the solution.
- Moles of Na2CO3 = 0.759 moles.
- Moles of H2O = mass of solvent / molar mass of H2O.
- Moles of H2O = 1257.2 g / 18.02 g/mol = 69.72 moles.
- Total moles = Moles of Na2CO3 + Moles of H2O = 0.759 + 69.72 = 70.479 moles.
- Mole fraction (X) = Moles of Na2CO3 / Total moles.
- Mole fraction (X) = 0.759 moles / 70.479 moles = 0.0108.

Therefore, the molarity of Na2CO3 in the solution is 0.759 M, the molality is 0.603 m, and the mole fraction is 0.0108.

To calculate the molarity, molality, and mole fraction of Na2CO3 in the solution, we need to follow a series of steps:

Step 1: Calculate the number of moles of Na2CO3 in the solution.
Given: Mass of Na2CO3 = 8.058 g
Using the molar mass of Na2CO3 (105.99 g/mol), we can calculate the number of moles:
Number of moles = mass / molar mass
= 8.058 g / 105.99 g/mol
= 0.076 mol

Step 2: Calculate the volume of the solution in liters.
Given: Density of the solution = 1077.2 kg/m3
Since density = mass / volume, we can rearrange the equation to solve for volume:
Volume = mass / density
= (8.058 g / 1000) / 1077.2 kg/m3
= 0.00749 L

Step 3: Calculate the molarity of Na2CO3.
Molarity (M) is defined as moles of solute divided by liters of solution.
Molarity = Number of moles / Volume of solution in L
= 0.076 mol / 0.00749 L
= 10.15 M

Step 4: Calculate the molality of Na2CO3.
Molality (m) is defined as moles of solute divided by mass of the solvent (in kg).
In this case, the solvent is water, and we assume its mass to be equal to its density.

Step 5: Calculate the mole fraction of Na2CO3.
Mole fraction is the ratio of the moles of one component to the total moles of all components in the solution.
Mole fraction of Na2CO3 = moles of Na2CO3 / total moles of all components

Please note that for the steps involving density, the answer might be slightly different due to rounding errors.

mols Na2CO3.10H2O = grams/molar mass.

Then M = mols/L soln.

m = mols/kg solvent.
Use density to convert L soln to grams soln and subtract g Na2CO3.10H2O to find g solvent. Convert g solvent to kg and apply the definition for m.

mols fraction. You have mols solute. Convert grams solvent to mols. Add mols solute + mols solvent to obtain total mols. Then mole fraction Na2CO3.10H2O = mols Na2CO3.10H2O/total mols.