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AerospaceEng
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Homework Statement
When 10.00 mL of a solution of strong acid is mixed with 100.00 mL of a solution of weak base in a coffee-cup calorimeter, the temperature rises from 22.8 oC to 26.8 oC. Determine q for the acid-base reaction, assuming that the liquids have densities of 1.00 g/mL and the same heat capacities as pure water.
Homework Equations
total volume V=110.0mL
change in temperature delta T = 4
mass m = 110.0g
heat capacity for water C=75.291J/(mol[itex]\circ[/itex]C
q = nC[itex]\Delta[/itex]T
q = mC[itex]\Delta[/itex]T
The Attempt at a Solution
so I used the formula
q = mC[itex]\Delta[/itex]T
because with the information given i couldn't find the number of moles and because only the molar heat capacity is given to use i had to find the mass based heat capacity and I found it to be C = 4181.3J/KgK
and then found q = 460J
which then the computer told me it was wrong.
It seemed odd that i had to go find the heat capacity rather than use the one provided. So I feel already there's my first mistake. But i know the formula is right so I can't see why it wouldn't work. However clearly my chemistry isn't that strong so perhaps I'm missing something. Any guidance would be appreciated! Thanks