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)

when the volume of gas is   changed from   717.73 ml   to 852 ml   the temperature will   change   from 315   c to 452   c

    calculation

this is calculated using the charles law formula

that is,   v1/t1 = v2/t2

          v1=?

        t1 = 315 c   into   kelvin = 315 +273 = 588 k

        v2 = 852   ml

        t2 = 425c + 273 =698 k

make v1   the subject of the formula ( by   multiplying both side by t1)

  v1=( v2 xt1) / t2

v1= (852 ml   x 588 k)/ 698 k= 717.73 ml

since electrons are negative the answer is neagtaive