A student mixes 0.400 L of 0.5M HCl with 0.250 L of 1.00 M NaOH. What would the Molar concentration of NaCl of the new solution be? What would the pH of the new solution be? If the solution were diluted 10-fold (to 5.75 L) what would the pH be?
I did this:
Moles HCl = (Moles of HCl/Liter of HCl solution) X Volume HCl solution
(0.5moles of HCl/1 liter of HCl) X 0.400 L HCl solution
1.25 moles of HCl
But I have no idea if I'm evenon the right track....
The other problem that I have is:
Calculate the energy released (using bond energies) from 155 g of hexenoic acid
C-C 345 kJ/mol
C=C 615 kJ/mol
C-H 415 kJ/mol
C-O 360 kJ/mol
C=O 805 kJ/mol (For carbon dioxide)
C=O 750 kJ/mol (For everything else)
O-H 460 kJ/mol
O=O 494 kJ/mol
I found that 155g of Hexenoic Acid is equal to 2.418 moles, but I don't know where to go from here? Do I just put kJ/2.418 and then divide?