0.1 M HCl is a stong-conductor and 0.1 M
HC2H3O2 is a weak-conductor.
Explain the difference in conductivity between 0.1 M HCl and 0.1 M
HC2H3O2. Relate the difference to
the terms strong acid and weak acid.
In class we discussed proton motive force, which is a
concentration gradient of hydrogen ions across a cell membrane to
create potential energy. Briefly diagram, or verbally discuss, how
this proton motive force is established in eukaryotic cells. Your
explanation should show the general path traveled by the
electrons.
If 85.00 mL of 0.100 M HCl is mixed with 25.00 mL of 0.200 M
H2SO4 and 50.00 mL of 0.400 M NaOH. What is the resulting pH of the
final solution?
Please show all work and how the formulas are derived if
modified.
Use activity coefficients to find the concentration of hydrogen
ions in a solution of 75.0 mM butanoic acid (C3H7COOH) and 0.05 M
NaCl. The ionization constant of butanoic acid is Ka = 1.52 × 10-5.
Take the size of C3H7COO– to be 500 pm.
What is the pH of this solution? Include activity coefficients in
your calculation.
What is the fraction of dissociation of butanoic acid in this
solution?
Calculate the concentration of all species present (H2SO4,
HSO4^-, H^+, SO4^-2) in a 0.285 M H2SO4 solution. The diprotic acid
equilibrium is :
H2SO4 <--> H^+ + HSO4^- Ka = very large
HSO4^- <---> H^+ + SO4^-2 Ka = 1.2 x 10^-2
Please explain why and when we use +x and -x. I am very confused
on this.
what is the new PH of a solution if 10ml of 0.1 M Hcl is added
to 150ml of a buffer system that is 0.1M Benzoic acid and 0.1M
sodium benzoate ( the Ka of benzoic acid is 6.3X10^-5). Thanks