If molecule of NaCl is heavier than a molecule of NaOH and NaOH is heavier than a molecule of HCl, can you explain the different conductivites you observed for these compounds?
You have presumably calculated conductivities so that it is the conductivity of a volume of electrolyte containing 1 mole of dissolved substance?
As each of the compounds have different RMM then the conductivities will reflect this.
nh3 has high b.p. than phz give resion
Certainly! The conductivity of a compound is determined by the presence of ions and their ability to move freely in a solution. In the case of NaCl, NaOH, and HCl, all three compounds can dissociate into ions when dissolved in water because they are soluble ionic compounds.
NaCl dissociates into Na+ and Cl- ions. NaOH dissociates into Na+ and OH- ions. HCl dissociates into H+ and Cl- ions.
The difference in conductivity arises from the number of ions produced when these compounds dissolve in water. Since NaCl, NaOH, and HCl have different chemical formulas, they will produce different numbers of ions in solution.
When NaCl dissolves, it forms one Na+ ion and one Cl- ion per formula unit. NaOH, on the other hand, produces one Na+ ion and one OH- ion per formula unit. Similarly, HCl forms one H+ ion and one Cl- ion per formula unit.
NaCl produces only two ions per formula unit, NaOH produces two ions per formula unit, and HCl produces two ions per formula unit as well. Therefore, the conductivity of NaCl, NaOH, and HCl in water would be similar since they all produce the same number of ions.
However, it is important to note that the concentration of the compounds may also affect conductivity. Higher concentrations of the compounds will result in a higher number of ions in solution, leading to higher conductivity.
So, while the molecular weight of the compounds may be different, their ionic compositions and ability to dissociate into ions are what primarily determine their conductivities in solution.