Silver chloride (#AgCI#) is relatively insoluble in water. At 25 C, #1.3 x 10^3# L of water is needed to dissolve 2.5 g of #AgCl#. What mass (in milligrams) of #AgCl# will dissolve in 1.0 L of water?

1 Answer
anor277
Sep 5, 2016

Approx. #2*mg#

Explanation:

#"Solubility"# #=# #"Moles of solute"/"Volume of solution"#.

For silver chloride we are given that: #2.5*g# wil dissolve in over #1# #m^3# of water.

And thus, #"Solubility"# #=# #(2.5*g)/(143.32*g*mol^-1)xx1/(1.3xx10^3*L)# #=# #1.34xx10^-5*mol*L^-1#.

And thus silver chloride solute in 1L of saturated water #=# #1.34xx10^-5*mol*L^-1xx143.32*g*mol^-1xx1L# #~=# #2*mg#

Typically, you are quoted a #K_"sp"# for these insoluble salts. #K_"sp "AgCl=1.77xx10^-10#. #K_"sp"# values can be shown to depend on the molar solubilities.

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