For ksp of silver sulfate (ag2so4) at 1. 2 ✕ 10-5, the solubility of silver sulfate is mathematically given as
x = 5.26*10^{-4}
<h3>What is the
solubility of silver
sulfate in 0.15 M AgNO3?</h3>
Generally, the equation for the Chemical reaction is mathematically given as
Ag2SO4 ⇄ 2Ag+ + SO4 2-
Therefore
Ksp = [Ag+ ]2 *[SO4 2-]
1.2*10-5 = ( 0.15 +2x)2*(x)
x = 5.26*10^{-4}
In conclusion, the solubility of silver sulfate is
x = 5.26*10^{-4}
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Answer: The balanced equation for the given reaction is
.
Explanation:
A chemical equation which contains same number of atoms on both reactant and product side.
For example, 
Here, number of atoms on reactant side are as follows.
Number of atoms on product side are as follows.
To balance this equation, multiply
by 2 on reactant side and multiply
by 2. Hence, the equation will be re-written as follows.

Here, number of atoms on reactant side are as follows.
Number of atoms on product side are as follows.
Now, there are same number of atoms on both reactant and product side. So, this equation is balanced.
Thus, we can conclude that the balanced equation for the given reaction is
.