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Abhisar

  • one year ago

The solubility product of BaSO4 at 25 C is 10^-9. What would be the concentration of H2SO4 necessary to precipitate BaSO4 from a solution of 0.01 M Ba+2 ions

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  1. Abhisar
    • one year ago
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    I am calculating it to be \(\sf 10^{-7}\)

  2. Abhisar
    • one year ago
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    But the answer says \(\sf 10^{-6}\)

  3. Abhisar
    • one year ago
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    Any idea @Photon336 ?

  4. Abhisar
    • one year ago
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    @Rushwr ?

  5. Photon336
    • one year ago
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    \[ksp = x ^{2} = [Ba ^{2+}][So4^{2-}]\] \[\frac{ [10^-9] }{ [0.01] } = 10^{-7}\] by eyeballing this I believe that's when it's saturated. so it would have to be more than that 10^-6 @abishar I agree with @rushwr

  6. Abhisar
    • one year ago
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    Oh Right!!!!!!!!!!!!!

  7. Photon336
    • one year ago
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    I think that's the concentration when it's saturated that means that it won't precipitate at this concentration , @rushwr what do you think?

  8. Abhisar
    • one year ago
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    I get it now, it should be anything greater than \(\sf 10^{-7}\) and hence \(\sf 10^{-6}\)

  9. Abhisar
    • one year ago
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    Thanx both of you c: Appreciate it..

  10. Photon336
    • one year ago
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    Absolutely, anytime

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