error 112 destroyer

[recyrb]

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2010 destroyer, gen chem

it asked which of the following would increase Ksp
of Ag3PO4


addition of a common ion
raise ph
lower ph
add common ion

it says only temperature can change K-------Ka-kb-kw Ksp
i though that much about rate constants and Ka Kb Kw

but if we add common ion- we reduce Ksp,
I thought if we increase pH that would remove some of the PO4, thus shifting right and making the the solid more soluble

is this just an error in the answer key?

thanks

 

[CHCH]

2010 destroyer, gen chem

it asked which of the following would increase Ksp
of Ag3PO4


addition of a common ion
raise ph
lower ph
add common ion

it says only temperature can change K-------Ka-kb-kw Ksp
i though that much about rate constants and Ka Kb Kw

but if we add common ion- we reduce Ksp,
I thought if we increase pH that would remove some of the PO4, thus shifting right and making the the solid more soluble

is this just an error in the answer key?

thanks

I don't think Ksp change, if you change the conc of reactant.
If you change the conc of reactant, that will change the rate of the reaction not Ksp.

Rate=Ksp[reactant]

I hope that will help

 

[bharat008]

Well i was thinking that if you decrease the pH (increase H+ concentration) then it would react with PO4- and decrease its concentration which would shift the reaction to right and make the AgPO4 more soluble.

Is that right or wrong??

 

[YoonS]

1

 

[anonymouse1]

Well i was thinking that if you decrease the pH (increase H+ concentration) then it would react with PO4- and decrease its concentration which would shift the reaction to right and make the AgPO4 more soluble.

Is that right or wrong??

what you said is correct but that changes the amount that would dissolve, but not the Ksp. The Ksp is a constant that ONLY changes with temperature.

 

[bharat008]

what you said is correct but that changes the amount that would dissolve, but not the Ksp. The Ksp is a constant that ONLY changes with temperature.

Just to make sure, when we have common ions in the solution that would shift the rxn to left and make it less soluble; but even this wouldn't effect Ksp. Ksp only changes with temperature and nothing else...

Can you differentiate between the increase/decrease in solubility vs. the Ksp (solubility product constant)?? I think i don't understand the difference between them..

Thanks

 

[anonymouse1]

Just to make sure, when we have common ions in the solution that would shift the rxn to left and make it less soluble; but even this wouldn't effect Ksp. Ksp only changes with temperature and nothing else...

Can you differentiate between the increase/decrease in solubility vs. the Ksp (solubility product constant)?? I think i don't understand the difference between them..

Thanks

increase and decrease in solubility is how much, in moles/grams..etc, an product will dissolve in solution.

the Ksp, is constant that defines the proportional relationship between the solid and the liquid dissolved concentrations of a substance.

pm me if you need dat tutoring.

 

[ScratchMan]

Same concept with Keq vs Q.
Q > K rxn goes towadr left.
Q < K rxn goes toward right.
Keq can not be changed by concentration changes.

Qsp > Ksp : rxn goes toward left. Pecipitation. Low solubility.
Qsp < Ksp: rxn goes toward right. High solubility.
Ksp cant be changed by concentraion change.

Chad said.....

 

[recyrb]

thanks all!

i just assumed that once you have more concentration of a product that is proportional to the amount that has dissolve, which is defined by the Ksp, in my head, meaning the Ksp would go up because in this particular solution. i assume that Ksp are determine in H20 but i appreciate all info ty