A student determined the H of neutralization of nitric acid (HN03) mixed with NaOH solution, using the procedure described in this experiment. Fifty milliliters of 1.00M HN03 was added to 50.5 mL of 1.00M NaOH solution, and the following time-temperature data were recorded.
A student determined the Hneutzn of nitric acid (HN03) mixed with NaOH solution, using the proce- dure described in this experiment. Fifty milliliters of
temp., c C
24.7
time, min
11.0
temp., "C
31.2
24.8
12.0
31.1
24.9
13.0
31.0
14.0
30.9
30.2
15.0
30.8
31.2
16.0
30.7
31.5
17.0
30.6
31.5
18.0
30.5
31.4
19.0
30.4
31.2
20.0
30.3
31.2
1.00M HN03 was added to 50.5 mL of 1.00M NaOH solution, and the following time-temperature data were recorded.
To determine the enthalpy of neutralization (Hneutzn) of nitric acid (HN03) mixed with NaOH solution, you can use the time-temperature data recorded during the experiment. The enthalpy of neutralization is the heat released or absorbed when an acid reacts with a base to form a salt and water.
Here's how you can proceed:
1. Calculate the initial and final temperatures of the reaction. The initial temperature is the temperature of the reactants before they are mixed, and the final temperature is the highest temperature reached during the reaction. From the data given, the initial temperature is 24.7°C and the final temperature is 31.5°C.
2. Calculate the temperature change (ΔT) by subtracting the initial temperature from the final temperature. In this case, ΔT = 31.5°C - 24.7°C = 6.8°C.
3. Determine the total heat exchanged (q) during the reaction using the equation q = m * C * ΔT, where m is the mass of the solution and C is the specific heat capacity of the solution. Since the volumes of both the nitric acid and NaOH solutions are given, you can use the density of water (1 g/mL) to assume the mass of the solution is equal to its volume. The density of a 1.00M HN03 solution is approximately 1.00 g/mL. Therefore, the mass of the solution is 50 g (50 mL * 1.00g/mL).
4. Next, you need to determine the specific heat capacity of the solution (C). This value depends on the concentration of the solution and can be assumed to be approximately the same as that of water (4.18 J/g°C).
5. Substitute the values into the equation q = m * C * ΔT to calculate the heat exchanged. In this case, q = 50 g * 4.18 J/g°C * 6.8°C = 1420 J.
6. Finally, use the equation Q = -Hneutzn to find the enthalpy of neutralization. Since the heat released by the reaction (q) is negative, make sure to assign a negative sign to Hneutzn. So, Hneutzn = -1420 J.
Therefore, the enthalpy of neutralization of the nitric acid (HN03) mixed with NaOH solution is -1420 J.