# 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)

###### FREE Expert Solution
90% (352 ratings)
###### FREE Expert Solution

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:

90% (352 ratings)
###### 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)

Frequently Asked Questions

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

Our tutors have indicated that to solve this problem you will need to apply the Solution Stoichiometry concept. You can view video lessons to learn Solution Stoichiometry. Or if you need more Solution Stoichiometry practice, you can also practice Solution Stoichiometry practice problems.

What is the difficulty of this problem?

Our tutors rated the difficulty ofIf 340 mL of 0.0824 M aqueous Ba 2+ and 230 mL of 0.253 M aq...as medium difficulty.

How long does this problem take to solve?

Our expert Chemistry tutor, Sabrina took 7 minutes and 18 seconds to solve this problem. You can follow their steps in the video explanation above.