Complete the Ka2 expression for H2CO3 in an aqueous solution. Ka2 = 4.69 x 10^-11 = ___
We know that
Ka = [Products]/[Reactants]
Given
H2CO3 + H2O -> HCO3- + H3O+
therefore
Ka = [HCO3-][H3O+]/[H2CO3][H2O]
The concentration of water is too big and any changes in concentration are negligible, therefore we can drop [H2O] and get:
Ka= 4.69x10-11 = [HCO3-][H3O+]/[H2CO3]
Complete the Ka2 expression for H2CO3 in an aqueous solution. Ka2 = 4.69 x 10^-11 =...
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determine the molar solubility (S) of Ag2CO3 in a buffered solution with a pH of 3.519 using the systematic treatment of equilibrium. Ksp (Ag2CO3) = 8.46x10^-12 ; Ka1 (H2CO3) = 4.45x10^-7 ; Ka2 (H2CO3) = 4.69 x 10^-11
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