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)

the correct name for the n3 ion is azide. azide is a polyatomic anion with a -1 charge and is written as n3 -1. it consists of three nitrogen atoms bonded together. hope i . let me know if you need anything else.

it is to be noted that an alpha particle is an helium nucleus. so it contains 2 protons 2 neutrons and has a mass number of 4. when alpha decay particles are ejected from the nucleus it gets transformed into an atom which has atomic number less than 2 and a mass number less than 4.

an equation that could represent alpha decay is radium 226 decay of alpha particle forms radon 222.

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