Answer:
a) If the solvent-solute interactions in a mixture are <u>stronger than</u> the solvent-solvent interactions and the solute-solute interactions, a homogeneous solution forms.
b) If the solvent-solute interactions in a mixture are <u>weaker than</u> the solvent-solvent interactions and the solute-solute interactions, the formation of a homogeneous solution is uncertain.
Explanation:
The solubility of solute in given solvent mainly depends upon the intermolecular interactions between the solvent and the solute. If the solute is surrounded and solvated by the solvent then the solute will dissolve in that solvent. Therefore, in order to dissolve the solute must form stronger interactions with the solvent as compared to the solute solute interactions or solvent solvent interactions.
Example:
When NaCl is added to water the partial negative oxygen of water is attracted to Na⁺ of NaCl and the partial positive hydrogen of water is attracted to Cl⁻ of NaCl. These new interactions between the NaCl ions and water are stronger than the interactions between water molecules and NaCl molecules themselves hence, results in solubility of NaCl in water.
On the other hand, if NaCl is added to Hexane (C₆H₁₄) it fails to make strong interactions with the solvent molecules resulting in insolubility of NaCl in hexane.
Answer:
c. 39
Explanation:
You round the number 39.098 to make it easier. Since you can't round it up to forty because the number after the 9 in-front of the decimal is a over i is unable to be rounded up
For a 100-g compound, we would have 2 g H, 32.7 g S, and 65.3 g O. We then divide each of these masses by their molar masses:
2 g H / 1.01 g/mol = 1.98 mol H
32.7 g S / 32.07 g/mol = 1.0196 mol S
65.3 g O / 16.00 g/mol = 4.08125 mol O
We then divide each amount of moles by the smallest of them, which is the 1.0196 from S:
1.98 mol H / 1.0196 mol S = 1.94 H ~ 2 H
1.0196 mol S / 1.0196 mol S = 1 S
4.08125 mol O / 1.0196 mol S = 4 O
So the empirical formula of the compound is H2SO4.
