Determine the **ΔH **by calculating for the heat involved using the **calorimetry equation **** **and * stoichiometry*.

For this problem, follow these steps:

1. Find mass of solution

2. Find the change in temperature

3. Find heat (Q)

4. Calculate moles of H_{2}O produced

5. Find heat released

In a constant-pressure calorimeter, 70.0 mL of 0.320 M Ba(OH) _{2} was added to 70.0 mL of 0.640 M HCl. The reaction caused the temperature of the solution to rise from 22.94°C to 27.30°C. If the solution has the same density and specific heat as water (1.00 g/mL and 4.184 J/g·°C, respectively), what is ΔH for this reaction (per mole of H_{2}O produced)? Assume that the total volume is the sum of the individual volumes.

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