A student enters the lab and conducts Part A of the Experiment. The student uses 25.00 mL of 2.112 M HCl, and adds NaOH in excess as instructed. If the ΔH of the neutralization reaction is known to be -57,320 J/mol H2O, what is the total theoretical heat released (in Joules)?

 3026.5 J

Explanation:

To calculate the number of moles for given molarity, we use the equation:

    .....(1)

Molarity of solution = 2.112 M

Volume of solution = 25.00 mL

Putting values in equation 1, we get:

a)

The balanced chemical reaction is:

As is the limiting reagent , it limits the formation of product. is the excess reagent.

1 mole of HCl produces = 1 mole of

0.05280 mole of HCl produces = moles of

Given :

Energy released when 1 mole of is produced = 57320 J

Thus Energy released when 0.05280 moles of is produced =

Thus 3026.5 J is the total theoretical heat released

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when [oh-] is 10-5  m, and [h3o+] is 10-9  m, the poh is 5 and ph is 9. again in both cases the sum of ph and poh is 14. however, the hydrogen ion concentration is not always going to be equal to exactly 1 x 10 raised to a negative number. for example, we skipped over the value of 2.0 x 10-7.