Use Le Châtelier's Principle to predict how this equilibrium system will respond to the changes you will make: CH3COOH(aq) LaTeX: \Leftrightarrow⇔ CH3COO-(aq) + H+(aq) How will adding sodium acetate ( CH3COONa) initially change the concentrations of CH3COOH, CH3COO-, and H+? How will the equilibrium system respond to this change?

The equilibrium will shift to the left.

Explanation:

If sodium acetate is added to acetic acid, the dissociation of the acetic acid is suppressed. The equilibrium position shifts to the left and the hydrogen ion concentration decreases due to decreased ionization of the acid. This common ion solution becomes less acidic than pure acetic acid.

This is so because of common ion effect. The acetate ion already present from the dissociation of acetic acid is also present in the sodium acetate. The presence of a common ion usually shifts the equilibrium position towards the left.

NaCH3CO2 (s) → Na + (aq) + CH3CO2 −(aq)

CH3CO2H(aq) ⇌ H +(aq) + CH3CO 2− (aq)

1. for the first question, we must find the mass of the anhydrous salt, mgso₄. the molar mass for mgso₄·7h₂o is 246.47 g/mol, while that of mgso₄ is 120.37 g/mol.7.834 g mgso₄·7h₂o * 1 mol mgso₄·7h₂o/246.47 g * 1 mol mgso₄/1 mol mgso₄·7h₂o * 20.37 g mgso₄/mol = 0.647 g mgso₄

2. mass of water = mass of sample - mass of anhydrous salemass of water = 7.834 - 0.647 = 7.19 gpercent water in hydrate = 7.19/7.834 * 100 = 91.74%

dynamic equilibrium is the answer.