why, when 0.025 M HNO3 and 0.025 MAl(NO3)3 (noting that Al(NO3)3 solid is a hydr

Question

why, when 0.025 M HNO3 and 0.025 MAl(NO3)3 (noting that Al(NO3)3 solid is a hydrate - Al(NO3)3*9H2O) were diluted to 100 mL distilled water, their conductivities do not match the isomolar trend - the more ions dissociating, the more the solution will conduct?

my values: HNO3 - 7.80ms and Al(NO3)3 - 6.10ms

HNO3 has 2 dissociating ions whereas Al(NO3)3 has 4, which should result in a higher conductance value.

Would this have something to do with aluminum nitrate being paired with water as a solid?

Explanation / Answer

the answer is very simple HNO3 will have higher conductivity than Al(NO3)3

this is because of the fact that dissociation constant of HNO3 is greater than Al(NO3)3

which means that when same moles of both solutions are mixed in water number of ions given by HNO3 is larger than number of ions given by Al(NO3)3

and ions are responsible for cunductivity in aqueous solution

to understand better for example

1 mole HNO3 will give (assumed value just to understand) 3 ions and 1mole of Al(NO3)3 will give 2 ions hence conductivity of Al(NO3)3 is less

Related Questions

Navigate

• Browse (All)
• Browse W
• Subjects

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.