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Two copper(I) salts of the organic acids HA and HB, slightly soluble in water, form a saturated solution in buffer of a given pH. 

 What will be the concentration of Cu+ cations in the solution if the solubility products of the two salts are Ks(CuA) and Ks(CuB) and the ionisation constants of the acids are Ka(HA) and Ka(HB)?  

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Equations for the total amounts of substances of the particles A, B, and Cu are as follows: 

a = n(A) + n(HA) + n(CuA) 

b = n(B) + n(HB) + n(CuB) 

m = n(Cu+) + n(CuA) + n(CuB) 

The amounts of precipitates are eliminated from the equations: 

a + bm = n(A) + n(HA) + n(B) + n(HB) n(Cu+ ) = 0 

because, when forming a system of both solid salts, the total number of particles A and B (a + b) must be equal to the total number of cations Cu+, i. e. to the value of m. When the amounts of substances are divided by the volume of the solution, we get concentrations, and thus:

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