Would precipitation occur when 500 mL of a 0.02M solution of AgNO3 is mixed with 500 mL of a 0.001M solution of NaCl? Show your work.

Question

anonymous · Answer

What do you think? How would you start this problem?

anonymous · Answer

I'm not sure how to solve this problem. I was hoping you could explain it. @ghuczek

somy · Answer

well first off, write the reaction between the two compounds and get the products

anonymous · Answer

@Somy How would you write the reaction between the two compounds?

somy · Answer

$\sf AgNO_3 + NaCl → $ 
exchange of ions 
so Ag takes Cl and Na takes NO3 
thus 
 $\sf AgNO_3 + NaCl → AgCl + NaNO_3 $ 
look at number of each atom on each side 
there is no need to balance it as its already balanced

somy · Answer

so now check the solubility of products of reaction you get

somy · Answer

Wiki: http://prntscr.com/6g54l5 http://prntscr.com/6g54rl as you can see AgCl is insoluble in water thus it will precipitate

somy · Answer

now do they want you to work out how much precipitation will occur?

vincent-lyon.fr · Answer

The question is Will precipitation occur (or not).
So you need to work out the solubility product for AgCl

anonymous · Answer

I'm still not sure what I have to do as far as showing my work. Like I've tried solving this problem myself and I'm pretty sure the answer is yes a precipitation will occur, but the problem is I need to explain how I got that answer. Show my work. Like I'm not sure what do for that part. Can one of your guys help me still?

vincent-lyon.fr · Answer

Suppose no precipitation occurs and work out the concentrations of Ag+ and Cl- it would imply.

matt101 · Answer

I think you might find this helpful: http://openstudy.com/study#/updates/5509d8f7e4b08972d3f49f1a