Problem: Calculate the solubility of barium carbonate, BaCO3, in pure water. Ksp = 2.0 × 10–9A) 1.3 × 10–3 MB) 3.2 × 10–5 MC) 2.2 × 10–5 MD) 4.5 × 10–5 ME) 4.0 × 10–18 M

FREE Expert Solution

For this problem, we’re being asked to calculate the solubility of barium carbonate, BaCO3


Since the BaCO3 is an ionic compound, it forms ions when dissociating in water. The dissociation of BaCO3 in water is as follows:


The carbonate ion, CO32, has a charge of –2. Calcium is in Group 2A so its charge is +2:

BaCO3(s)  Ba2+(aq) + CO32(aq)



We can construct an ICE table for the dissociation of BaCO3

Remember that solids are ignored in the ICE table and Ksp expression.


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Problem Details

Calculate the solubility of barium carbonate, BaCO3, in pure water. Ksp = 2.0 × 10–9

A) 1.3 × 10–3 M

B) 3.2 × 10–5 M

C) 2.2 × 10–5 M

D) 4.5 × 10–5 M

E) 4.0 × 10–18 M

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What scientific concept do you need to know in order to solve this problem?

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