a 100.0 mL sample of 0.300M NaOH is mixed with a 100.0mL sample of 0.300 M HNO3

Question

a 100.0 mL sample of 0.300M NaOH is mixed with a 100.0mL sample of 0.300 M HNO3 in a coffee cup calorimeter. If both solutions were initially at 35.00 degrees Celsius and the temperature of the resulting solution was recorded as 37.00 degrees celsius, determine the ?H rxn (in units of kJ/mol NaOH) for the neutralization reaction between aqueous NaOH and HCl. Assume 1) that no heat is lost to the calorimeter or the surroundings, and 2) that the density and the heat capacity of the resulting solution are the same as water.

Explanation / Answer

i notice that you gave the data for thisreaction:
NaOH& HNO3 --> NaNO3 &H2O

then asked for the reuslts for this reaction
NaOH & HCl --> NaCl & H2O

we cna solve this request because both reactions have the same dH reaction
since both reactiona have the same net ionic equation:
OH- & H+ --> H2O
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0.1000 L sample of 0.300 mol / litre NaOH = a 0.0300 mole experiment

we make the assumption that this 200 ml experiment has a solution of the same density as water,
so 200 ml equals 200 grams of solution

we also make the assumption that the specific heat for this solution is the same as for water, @ 4.184 J/g-C

these are normal assumptions

find heat
dH = mCdT
dH = (200 g)(4.184 J/g-C)(2.0 C rise)
dH = - 1673.6 Joules .... energy was released

find ?H

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