What is the solubility of X in mol/dm3 if 25cm3 of its saturated solution contains 4.0g of X (Molar mass of X=60)
mols X in 25 cc = 4.0/60 = 0.0667
Then 0.0667 mols x (1000/25) = ?
that gives you mol/cm^3
adjust for 1dm = 10cm
No, that gives you mols/L which is mols/dm^3.
0.0667 mols/25 cc. Convert to 1000 cc (1 dm^3) as above.
ouch. You are correct. Dunno what I was thinking.
Very poor. I don't understand what going on
To find the solubility of X in mol/dm³, we first need to understand the concept of solubility. Solubility is defined as the maximum amount of solute that can dissolve in a given amount of solvent at a specific temperature and pressure.
In this case, we are given that 25 cm³ of X's saturated solution contains 4.0 g of X. We also know the molar mass of X is 60 g/mol.
To find the solubility in mol/dm³, we need to convert the grams of X to moles using the molar mass formula:
Molar mass (g/mol) = Mass (g) / Moles (mol)
Rearranging this equation, we can solve for the number of moles:
Moles (mol) = Mass (g) / Molar mass (g/mol)
Substituting the given values:
Moles (mol) = 4.0 g / 60 g/mol
Moles (mol) ≈ 0.0667 mol
Next, we convert the volume from cm³ to dm³, as solubility is typically reported in mol/dm³. Since 1 dm³ is equal to 1000 cm³:
Volume (dm³) = Volume (cm³) / 1000
Volume (dm³) = 25 cm³ / 1000
Volume (dm³) = 0.025 dm³
Now, we can calculate the solubility using the formula:
Solubility (mol/dm³) = Moles (mol) / Volume (dm³)
Substituting the values we found:
Solubility (mol/dm³) = 0.0667 mol / 0.025 dm³
Solubility (mol/dm³) ≈ 2.67 mol/dm³
Therefore, the solubility of X in mol/dm³ is approximately 2.67 mol/dm³.