Problem: If 340 mL of 0.0824 M aqueous Ba 2+ and 230 mL of 0.253 M aqueous H + are reacted, how many mol of liquid H2O is produced?Ba(OH)2(aq) + 2HClO4(aq) → Ba(ClO4)2(aq) + 2H2O(l)

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We’re being asked to calculate the moles of H2O formed in the reaction of 340 mL of 0.0824 M Ba2+ and 230 mL of 0.253 M H+.


From the problem, the given balanced equation is:

Ba(OH)2(aq) + 2 HClO4(aq)  Ba(ClO4)2(aq) + 2 H2O(l)


Recall that molarity is the ratio of the moles of solute and the volume of solution (in liters)

In other words:


Molarity (M) =moles of soluteLiters of solution


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Problem Details

If 340 mL of 0.0824 M aqueous Ba 2+ and 230 mL of 0.253 M aqueous H + are reacted, how many mol of liquid H2O is produced?

Ba(OH)2(aq) + 2HClO4(aq) → Ba(ClO4)2(aq) + 2H2O(l)

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