Question 1

Why are water molecules arranged around sodium and chloride ions?

Accepted Answer

Water is polar, so its oxygen end carries partial negative character and its hydrogen ends carry partial positive character. The oxygen end is oriented toward Na⁺, while a hydrogen end is oriented toward Cl⁻, producing ion–dipole attractions.

Question 2

How is the dissolved amount calculated in the lab?

Accepted Answer

The lab uses a 0.700 mol represented NaCl sample in 85 mL of water. At the selected temperature, a listed NaCl solubility value gives the equilibrium mass in 85 g of water; dividing by the 58.44 g mol⁻¹ molar mass gives the equilibrium moles. The model lattice then shows the corresponding representative fraction while undissolved solid remains.

Question 3

Does stirring increase the equilibrium solubility of a solid?

Accepted Answer

Stirring improves contact and mixing, so equilibrium is reached faster. It does not change the final equilibrium concentration governed by the solute, solvent, and temperature.

Question 4

How does Ksp apply to a sparingly soluble ionic salt?

Accepted Answer

For MaXb(s) ⇌ aM(aq) + bX(aq), the solubility product is Ksp = [M]a[X]b. This expression is used for a sparingly soluble salt, while the NaCl example in the scene demonstrates hydration and equilibrium using its listed solubility data.

Solubility, Lattice & Hydration 3D Lab

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