When 25.0 mL of 1.00 M HCl (0.025 mol)is mixed with exactly 25.0 mL of NaOH (0.025 mol) in a calorimeter, the temperature of the solution increased from 25.00 °C to 27.30 °C.

(a) Is the reaction exothermic or endothermic?
(b) If the specific heat of the solution is 4.18 J/ g·°C, density = 1.0 g/mL, what is:

To determine whether the reaction is exothermic or endothermic, we need to analyze the change in temperature. If the temperature of the solution increases, it means that heat is being released. In this case, the temperature increased from 25.00 °C to 27.30 °C, so the reaction is exothermic.

To find the values requested, we can use the formula:

q = m * c * ΔT

Where:
q = heat absorbed or released by the solution (in Joules)
m = mass of the solution (in grams)
c = specific heat of the solution (in J/ g·°C)
ΔT = change in temperature (in °C)

(a) Heat released by the solution (q):

First, we need to determine the mass of the solution. Since the volume is given as 25.0 mL and the density is 1.0 g/mL, the mass would be 25.0 g (mass = volume * density).

So, m = 25.0 g

Substituting the values into the formula, we have:
q = (25.0 g) * (4.18 J/ g·°C) * (27.30 °C - 25.00 °C)

(b) The total heat released by the reaction (q) can be calculated as shown above.