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anonymous

  • one year ago

How many liters of 0.85 M HCl solution would react completely with 3.5 moles Ca(OH)2? Ca(OH)2(s) + 2 HCl(aq) yields CaCl2(aq) + 2 H2O(l) 1.5 L HCl(aq) 8.2 L HCl(aq) 2.1 L HCl(aq) 6.0 L HCl(aq)

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  1. anonymous
    • one year ago
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    @Nnesha

  2. anonymous
    • one year ago
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    @e.mccormick

  3. JFraser
    • one year ago
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    See the molar ratio from the balanced reaction? Telling you every time you use 1 mole of calcium hydroxide, you need \(two\) miles of HCl to react fully with it

  4. anonymous
    • one year ago
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    @jfraser so c

  5. JFraser
    • one year ago
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    No. The problem says you start with 3.5 moles of calcium hydroxide, so how many moles of HCl will fully react with that much? (Twice as much)

  6. JFraser
    • one year ago
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    The balanced reaction tells us \(ratios\), not absolute amounts

  7. anonymous
    • one year ago
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    @jfraser so d would be correct?

  8. JFraser
    • one year ago
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    You're jumping. Stop jumping. If you have to use 3.5 moles of calcium hydroxide, you must also use 7 moles of HCl. But the question is asking about the \(volume\) of HCl solution needed. The \(concentration\) of the HCl is 0.85mol/L

  9. anonymous
    • one year ago
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    oh so b @jfraser thanks

  10. JFraser
    • one year ago
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    Each 1L of solution contains only 0.85 moles of HCl \[7mol HCl * \frac{1L HCl}{0.85mol HCl}\]

  11. JFraser
    • one year ago
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    Ye

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