1.Suppose 100.0 mL of 1.00 M HCl and 100.0 mL of 1.00 M NaOH, both initially at 25.0oC, are mixed in a Thermos flask. When the reaction is complete, the temperature is 31.8oC. Assume the solutions have the same heat capacity and density as pure water.
Compute the heat released (in kJ).
Use your value to evaluate the molar heat of the neutralization reaction:
H3O+ + OH- 2H2O(l)
2.What is the maximum volume (in L) of 2.7 M HCl(aq) that the buffer prepared from 5.2 g of NH2CH2CO2H and 1.35 L of 0.15 M NH2CH2CO2Na can tolerate without showing a pH change greater than 0.13 units? pKa(NH2CH2CO2H) = 9.88.
3.How many grams of solid NaOH must be added to the buffer solution described below to change the pH by 0.13 units? Na2CO3 is added to the 0.500 M HCl solution to make 1.5 L of a buffer solution at pH = 9.76 and at a total concentration of 0.324 M.