50.0 mL of a solution of HCl is combined with 100.0 mL of 1.15 M NaOH in a calorimeter. The reaction mixture is initially at 22.4°C and the final temperature after reaction is 31.2°C. What is the molarity of the HCl solution? You may assume that there is an excess of base (so all of the HCl has reacted), that the specific heat of the reaction mixture is 0.96 cal/g°C, and that the density of the reaction mixture is 1.02 mg/mL. The heat of neutralization of HCl and NaOH is 13.6 kcal/mol.
2 answers
How do I set this problem up?
HCl + NaOH ==> NaCl + H2O
q = heat generated = mass solution x specific heat solution x (Tfinal-Tinitial)
mass solution is 150 mL x 1.02 g/mL(NOTE: I think this is a typo and should be 1.02 g/mL and not 1.02 mg/mL)
That's q for how many mols?
That's 13.6 kcal/mol x #mols = q
Solve for # mols.
Then M = mols/L. You know mols and you know L (0.05), solve for M.
q = heat generated = mass solution x specific heat solution x (Tfinal-Tinitial)
mass solution is 150 mL x 1.02 g/mL(NOTE: I think this is a typo and should be 1.02 g/mL and not 1.02 mg/mL)
That's q for how many mols?
That's 13.6 kcal/mol x #mols = q
Solve for # mols.
Then M = mols/L. You know mols and you know L (0.05), solve for M.
2 answers