In a coffee-cup calorimeter, 100.0 mL of 1.0 M NaOH and 100.0 mL of 1.0 M HCl are mixed. Both solutions were origi- nally at 24.68C. After the reaction, the nal temperature is 31.38C. Assuming that

asked by @vanessai1 • 11 months ago • Chemistry • 5 pts

all the solutions have a density of 1.0 g/cm3 and a speci c heat capacity of 4.18 J/8C ? g, calcu- late the enthalpy change for the neutralization of HCl by NaOH. Assume that no heat is lost to the surroundings or to the calorimeter.

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Hi Vanessa! The way that the problem was stated made it a little bit confusing but really, all you have to look at is the volume of each solution! You don't need the molarities to calculate the heat released (Temperature increased). You just have to get the mass by multiplying the total volume by the density. Also, since it was assumed that no heat is lost to the calorimeter, we wouldn't need a value for Cp of the calorimeter. The solution is posted below. I hope this helps! enter image description here

answered by @leot1 • 11 months ago
  • WHAT does the p stand for in the equation.I am only familiar with q=mc delta T BreAnn commented 3 months ago