volume H2O is 55.0 + 55.0 = 110.0 and that is 110.0g
q = mass H2O x specific heat H2O x (Tfinal-Tinitial)
mols Ba(OH)2 = M x L = approx 0.017 but you need a better number than that and that produces twice that number of mols or approx 0.034.
Ba(OH)2 + 2HCl ==> BaCl2 + 2H2O
Then q from above is the amount of heat produced for 0.034 mols.
q/0.034 gives you q/mol H2O. Convert to kJ/mol
In a constant-pressure calorimeter, 55.0 mL of 0.310 M Ba(OH)2 was added to 55.0 mL of 0.620 M HCl. The reaction caused the temperature of the solution to rise from 22.23 °C to 26.45 °C. If the solution has the same density and specific heat as water, what is ΔH for this reaction (per mole of H2O produced)? Assume that the total volume is the sum of the individual volumes.
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