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# Determine Determining the final temperature from acid base neutralization equation and moles

50 ml of 0.2 M solution of HCl$$\ce{HCl}$$ is mixed with 75 ml of 0.2 M solution of NaOH$$\ce{NaOH}$$ in a constant pressure calorimeter. The acid base neutralization which occurs can written as:

$$\ce{H+_{(aq)} + OH^{-}_{(aq)} -> H2O_{(l)}}$$

$$\Delta H = -57\ \mathrm{kJ}$$

Calculate the final temperature of the reaction mixture (assume the heat capacity of the calorimeter is negligible).

How can I do this problem without an initial temperature!?

# Determine final temperature from acid base neutralization equation and moles

50 ml of 0.2 M solution of HCl is mixed with 75 ml of 0.2 M solution of NaOH in a constant pressure calorimeter. The acid base neutralization which occurs can written as:

$$\ce{H+_{(aq)} + OH^{-}_{(aq)} -> H2O_{(l)}}$$

$$\Delta H = -57\ \mathrm{kJ}$$

Calculate the final temperature of the reaction mixture (assume the heat capacity of the calorimeter is negligible).

How can I do this problem without an initial temperature!?

# Determining the final temperature from acid base neutralization equation and moles

50 ml of 0.2 M solution of $$\ce{HCl}$$ is mixed with 75 ml of 0.2 M solution of $$\ce{NaOH}$$ in a constant pressure calorimeter. The acid base neutralization which occurs can written as:

$$\ce{H+_{(aq)} + OH^{-}_{(aq)} -> H2O_{(l)}}$$

$$\Delta H = -57\ \mathrm{kJ}$$

Calculate the final temperature of the reaction mixture (assume the heat capacity of the calorimeter is negligible).

How can I do this problem without an initial temperature?

3 added 9 characters in body

50 ml ml of 0.2 M M solution of HCl is mixed with 75 ml ml of 0.2 M M solution of NaOH in a constant constant pressure calorimeter. The acid base neutralization which occurs can written as:

$$\ce{H+_{(aq)} + OH-_{(aq)} -> H2O_{(l)}}$$$$\ce{H+_{(aq)} + OH^{-}_{(aq)} -> H2O_{(l)}}$$

$$\triangle H = - 57 kJ$$$$\Delta H = -57\ \mathrm{kJ}$$

Calculate the final temperature of the reaction mixture (assume the heat capacity of the calorimeter is negligible).

How can I do this problem without an initial temperature!?

50 ml of 0.2 M solution of HCl is mixed with 75 ml of 0.2 M solution of NaOH in a constant pressure calorimeter. The acid base neutralization which occurs can written as:

$$\ce{H+_{(aq)} + OH-_{(aq)} -> H2O_{(l)}}$$

$$\triangle H = - 57 kJ$$

Calculate the final temperature of the reaction mixture (assume the heat capacity of the calorimeter is negligible.

How can I do this problem without an initial temperature!?

50 ml of 0.2 M solution of HCl is mixed with 75 ml of 0.2 M solution of NaOH in a constant pressure calorimeter. The acid base neutralization which occurs can written as:

$$\ce{H+_{(aq)} + OH^{-}_{(aq)} -> H2O_{(l)}}$$

$$\Delta H = -57\ \mathrm{kJ}$$

Calculate the final temperature of the reaction mixture (assume the heat capacity of the calorimeter is negligible).

How can I do this problem without an initial temperature!?

2 added 19 characters in body; edited tags

50 ml of 0.2 M solution of HCl is mixed with 75 ml of 0.2 M solution of NaOH in a constant pressure calorimeter. The acid base neutralization which occurs can written as:

H+(aq) + OH- (aq) -> H2O(l)
deltaH = - 57 kJ$$\ce{H+_{(aq)} + OH-_{(aq)} -> H2O_{(l)}}$$

$$\triangle H = - 57 kJ$$

Calculate the final temperature of the reaction mixture (assume the heat capacity of the calorimeter is negligible.

How can I do this problem without an initial temperature!?

50 ml of 0.2 M solution of HCl is mixed with 75 ml of 0.2 M solution of NaOH in a constant pressure calorimeter. The acid base neutralization which occurs can written as:

H+(aq) + OH- (aq) -> H2O(l)
deltaH = - 57 kJ

Calculate the final temperature of the reaction mixture (assume the heat capacity of the calorimeter is negligible.

How can I do this problem without an initial temperature!?

50 ml of 0.2 M solution of HCl is mixed with 75 ml of 0.2 M solution of NaOH in a constant pressure calorimeter. The acid base neutralization which occurs can written as:

$$\ce{H+_{(aq)} + OH-_{(aq)} -> H2O_{(l)}}$$

$$\triangle H = - 57 kJ$$

Calculate the final temperature of the reaction mixture (assume the heat capacity of the calorimeter is negligible.

How can I do this problem without an initial temperature!?

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