A groundwater contains 2×10-3 M of Ca²+, has a pH of 6, and an alkalinity of 10-3 eq/L. CaCO3(s) Ca²+ + CO²²¯ Kso = 10-8.34 a) Would you expect CaCO3(s) to precipitate from this groundwater? Provide calculations to support your answer.
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Can you explain how the alpha values were calculated.
![A groundwater contains 2×10-3 M of Ca²+, has a pH of 6, and an alkalinity of 10-³
eq/L.
CaCO3(s) → Ca²+ + CO²²¯
Kso = 10-8.34
a) Would you expect CaCO3(s) to precipitate from this groundwater? Provide
calculations to support your answer.
σ0 = 0.666 90.334
σ₂ = 1.67 × 10-5
Атры
AT PH = 6
CT, CO₂ ~ [HCO₂"]
2
ALK ~ [HCO₂]
-3
10
=
2.
=
3×103 M
0.334
[CO₂ ²²] = α₂ CT, CO₂ = 1.67×105.3×10-3
8
= 5×10
10 < Kso
Q = [Ca 2+ ] [co₂²] = (2×10-³) (5×10- 8) = 10"
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