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katrin2010 [14]
3 years ago
6

Solid barium sulfate dissolves into its respective ions at 25°C. Suppose that in a particular solution, [Ba2+ ] = 1.76 x 10-3 M.

Find the value of Ksp.
Chemistry
2 answers:
ale4655 [162]3 years ago
5 0
BaSO₄(s) ⇄ Ba²⁺(aq) + SO₄²⁻(aq)

Ksp=[Ba²⁺][SO₄²⁻]

[Ba²⁺]=[SO₄²⁻]

Ksp=[Ba²⁺]²

Ksp=(1.76*10⁻³)² =3.0976×10⁻⁶ ≈3.1×10⁻⁶
Ne4ueva [31]3 years ago
3 0

Answer:

The value of solubility product of barium sulfate is 3.09\times 10^{-6}.

Explanation:

BaSO_4\rightarrow Ba^{2+}+SO_4^{2-}

                         S         S

1 mole of barium sulfate dissociates into 1 mole of barium ion and one mole sulfate ion.

So, [Ba^{2+}]=[SO_4^{2-}]=S

[Ba^{2+}]=S=1.76\times 10^{-3} M

The solubility product the barium sulfate will be given by:

K_{sp}=S\times S=S^2

K_{sp}= (1.76\times 10^{-3})^2=3.09\times 10^{-6}

The value of solubility product of barium sulfate is 3.09\times 10^{-6}.

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