Chemistry, 02.09.2019 19:30 makinzy03

The solubility increase when the temperature increases between ionic compounds.

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Strong solute-solvent attractions increase solubility of ionic compounds. Ionic compounds are most soluble in polar solvents like water, because the ions of the solid are strongly attracted to the polar solvent molecules.

COMMON-ION EFFECT

Ionic compounds are less soluble is solvents that contain a common ion. For example, CaSO₄ is slightly soluble in water.

CaSO₄(s) ⇌ Ca²⁺(aq) + SO₄²⁻(aq)

If the water already contains calcium ions or sulfate ions, the position of equilibrium moves to the left and the solubility decreases (Le Châtelier’s Principle).

TEMPERATURE

Increasing the temperature usually increases the solubility of an ionic compound because the solution process is usually endothermic.

CaSO₄(s) + heat ⇌ Ca²⁺(aq) + SO₄²⁻(aq)

Le Châtelier’s Principle predicts that increasing the temperature (adding heat) will shift the position of equilibrium to the right. The compound will become more soluble. From a webpage i found this from https://socratic.org/questions/what-factors-affect-solubility-of-ionic-compounds

Answer from: Quest

For cyclohexane compounds drawn in a chair conformation: -axial bonds are vertical -equatorial bonds are parallel to two bonds within the ring. thus, as i assume the chair conformation is drawn: -the x group is in an axial position, as are the five other vertical bonds. -three axial bonds are on the top face of the ring -the other three axial bonds are on the bottom face the position of the second substituent on each ring carbon is equatorial. gauche groups must be on an adjacent carbon such as carbon 6 and carbon 2, and also gauche groups are rotated by 60 degrees relative to each other. drawing the newman projections for c1–c2 and c1–c6 aids in visualizing the groups that are gauche to the y group on c1. click this link and watch some academic videos that may you more understand the topic

Answer from: Quest

what are the statements