Question

The behaviors of four different solutes when dissolved in water are indicated by the four equations below. Match each of the resulting solutions to its expected behavior in a conductance apparatus like the one shown to the left, if the solute is present at a concentration of 0.2 M Battery Anode positive electrode Cathode (negative electrode HNO3(aq) + H20(L) =H30+ (aq) + NO2 (aq) – HNO3 (4) + H2O(l) → H30+ (aq) – NO, (aq) Ca(OH)2 (3) +- Ca?+ (aq) +2011+ (aq) HOCH,CH,OH() - HOCH,CH,OH(aq) evious Ne

Answer 1

1) HNO2 + H2O $\rightleftharpoons$ H3O+ + NO2 - ; Would produce dim light

Because they dissociate partially hence less conducting.

2) HNO3 + H2O -> H3O+ + NO3-. : Would produce bright light

Because they dissociate completely hence more conducting.

3) Can(OH)2 -> Ca2+ + 2OH- ; Would produce bright light.

Because they dissociate completely hence more conducting.

4) HOCH2CH2OH -> HOCH2CH2OH ; Would not cause the bulb to light.

Because it is non conducting solution.