[CardinVo]

Please help me solving this problem. My instructor did not do a great job in explaining it.

A 100ml sameple of 1.0M NaOH is mixed with 65.0 ml of 1.0M H2SO4. The initial temperature of each solution is 25.0 Celsius degree. After adding NaOH to the solution, the temperature increases. Assume the density of the solution is 1.0g/ml, the specific heat of the mixed solution is 4.18 J/(g. C), and no heat is lost to the surroundings. Find the final temperature of the solution.

I would appreciate any help.

[Borek]

You have to show your attempts at solving the question to receive help. This is a forum policy.

Not enough data - you probably should check neutralization enthalpy at the end of the book.

[CardinVo]

I did use the heat of reaction and formation per mole to find the enthalpy change of the reaction. Then I calculated the q of the solution using the provided information. the weird thing was that i got a negative number of temperature, the number was also high about 108 celcius degree. I wasn't sure if I did it right so I hope someone could help me solving it. I did try my best tho.