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Let's consider the saturated solution of silver chloride ( #AgCl#), where an exists between the dissolved ions and undissolved silver chloride according to the following reaction: #AgCl_((s)) rightleftharpoons Ag_((aq))^(+) + Cl_((aq))^(-)# Since this is an equilibrium reaction, we can write the equilibrium constant for it: #K = ([Ag^(+)]*[Cl^(-)])/([AgCl])#. Now, the concentrations of solids are either unknown or assumed to be constant, so this reaction becomes #K * [AgCl] = K_(sp) = [Ag^(+)]*[Cl^(-)]# The magnitude of #K_(sp)# directly indicates the solubility of the salt in water, since #K_(sp)# is derived from the concentrations of ions in equilibrium reactions. Thus, higher concentrations of ions mean greater solubility of the salt. When trying to write the equation for #K_(sp)#, you need to know how to break the compound into ions (identify the monoatomic and polyatomic ions), how many moles of each ion are formed, and the charge on each ion. In a saturated solution the solid is in equilibrium with its ions e.g: #CaCO_(3(s))rightleftharpoonsCa_((aq))^(2+)+CO_(3(aq))^(2-)# The expression for #K_(sp)# is: #K_(sp)=[Ca_((aq))^(2+)][CO_(3(aq))^(2-)]# We don't include the concentration of the solid as this is assumed constant. So if we know the concentration of the ions you can get #K_(sp)# at that particular temperature. Using #K_(sp)# enables you to find the limit of concentration before a solid forms. 7/27/2018 0 Comments CopyNook download freeBy The NOOK Tablet allows you to host many file types in its storage space. You want to make sure the files are in the right format, then you are able to transfer them through a USB connection from your computer to your NOOK Tablet for viewing. Prepare files for the NOOK Tablet What if you have files on your desktop or laptop computer that you want to use on your NOOK Tablet, but the files are stored in the wrong format? 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