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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?

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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!?

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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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