Question

Part 2 - Molecular View of Solubility 6. Sketch a particulate diagram for aqueous solutions of each of these substances (include a few molecules of water as the solvent). Provide an explanation for your sketch. Include a chemical equation in your explanation if applicable. Finally, predict whether the solution will conduct electricity, and explain briefly Substance Explanatics Electrolytic Properties Sketch Since it's Tonic compound conduct. lit seperates to ins. selements onizes AgCI due to strong ion dipole p and carries eletthons force, conduct it's imit compowrid. H and nos seperates and ioniter water. mokin produce attractira ion-dipole HNO foru. CaCl2 CH,OH KOH 7. What factors determine how well a substance dissolves in water? 8. What factors determine how well a substance conducts electricity?

Answer 1

1) AgCl: AgCl is spearingly soluble in water. Hence most of AgCl will be insoluble in water and very little amount will dissolve to give dissociated Ag+ and CI-ions. AgCl Electrolytic properties: As there are ions of Ag+ and Cl- present in the solution, the solution will show conductance. H2O 2) HNO3: is an ionic compound and strong acid hence it dissociates completly to give H+ and NO3- ions. HNO3 there wont be any HNO3 molecules • H+ Electrolytic properties: NO3- As there are high number of ions of H+ H20 and NO3- present in the solution, the solution will show high conductivity. 3) CaCl2: it is highly soluble in water and give Ca2+ and Cl-ions. CaCl2 Ca2+ Electrolytic properties: CI- As there are high number of ions of H+ and NO3- present in the solution, the solution will show high conductivity. H2O

4) CH3OH: This is a polar covalent compound. Practically, it does not dissociate as such in to the water. CH3OH Electrolytic properties: As there are no ions produced there 40 will not be any conductunce. Water and alcohol molecules from strong hydrogen bonding hence alcohol molecules are surrounded by water molecules. H2O 5) KOH: It is strong electrolyte and dissociates completely in the water. • KOH there wont be any KOH molecules • K+ Electrolytic properties: • OH- As there are high number of ions of K+ and OH- present in the solution, the solution will show high conductivity. H20 6) HF is a weak electrolyte and hence very small ammount of HF will be dissociated to give H+ and F. HF Electrolytic properties: • H+ As there are some ions of H+ and F- . F present in the solution, the solution will H2O show some conductivity.

7) Factors affecting the solubility in water:

Polarity, ionic and covalent nature, dissociation constant. Water being polar compound more polar substances are more soluble in water. Ionic compounds are more soluble in water. The compound with higher dissociation constant will have higher solubility.

9) Conductance is mainly dependant on the dissociation of the ionic compound.

Higher the dissociation constant, the higher the conductivity of that aqueous solution.