I came across a question in my gen chem textbook where they want you to find the heat capacity of a calorimeter, because it isnt always negligible. Well, that is beside the point because I am stumped on part of the question that doesn't really deal with that. It says:
Consider an experiment in which we combine 50.0 mL of 0.250 M HCl (aq) with 50.0 mL of 0.250 M NaOH. The calorimeter and both solutions are initially at 23.50*C and the density and specific heat of both solutions are the same as that of water (1.000g/mL and 4.184 J/g*C, respectively). We can determine the amount of heat the reaction will generate using moles of reactant and heat of neutralization blah blah blah...
Guys, I CANNOt understand why the combined densities are the same as that of water. It makes sense intuitively because they will basically become water, but looking at it this way:
HCl: (0.250 M)(.050 L) = 0.0125 mol
NaOH: (0.250 M)(.050 L) = 0.0125 mol
0.0125 mol HCl = 0.456 g HCl
0.0125 mol NaOH = 0.5 g NaOH
0.456 + 0.5 = 0.956 g
This is 0.956 grams per 0.1 L, which is 10 g/L, or **0.01 g/mL** and this is NOT the density of water. PLEASE HELP ME HERE LOL
Thanks
Consider an experiment in which we combine 50.0 mL of 0.250 M HCl (aq) with 50.0 mL of 0.250 M NaOH. The calorimeter and both solutions are initially at 23.50*C and the density and specific heat of both solutions are the same as that of water (1.000g/mL and 4.184 J/g*C, respectively). We can determine the amount of heat the reaction will generate using moles of reactant and heat of neutralization blah blah blah...
Guys, I CANNOt understand why the combined densities are the same as that of water. It makes sense intuitively because they will basically become water, but looking at it this way:
HCl: (0.250 M)(.050 L) = 0.0125 mol
NaOH: (0.250 M)(.050 L) = 0.0125 mol
0.0125 mol HCl = 0.456 g HCl
0.0125 mol NaOH = 0.5 g NaOH
0.456 + 0.5 = 0.956 g
This is 0.956 grams per 0.1 L, which is 10 g/L, or **0.01 g/mL** and this is NOT the density of water. PLEASE HELP ME HERE LOL
Thanks