- #1
APCalculus
- 2
- 0
Hypochlorous acid, HOCl, is a weak acid in water. The Ka expression for HOCl is shown below:
[H3O+][OCl-]/ [HOCl]= 3.2 X 10^-8
1) write a chemical equation showing how HOCl behaves as an acid in water.
i got: HOCl + H2O = H3O + OCl
2) calculate the PH of a 0.175 M solution of HOCl.
i got:
HOCl + H2O = H3O + OCl
Initial: 0.175 0 0 0
Change: -x -x +x +x
Equilibrium: 0.175-x -x +x +x
am i doing it right? how do u calculate the PH from x?
3) write the net ionic equation for the reaction between the weak acid HOCl and the strong base NaOH.
I got: HOCl + NaOH = H3O +Na +OH
is it right?
4) In an experiment, 20 mL of 0.175 M of HOCl is placed in a flask and titrated with 6.55 mL of 0.435 M NaOH.
A)Calculate the number of moles of NaOH added.
I did: (6.55/1000) x (0.435 M) = 0.0025
B) Calculate [H3O+] in the flask after the NaOH has been added.
where do i start? i don't get what the question is asking.
C) Calculate [OH-] in the flask after the NaOH has been added.
where do i start? i don't get what the question is asking.
thank you.
[H3O+][OCl-]/ [HOCl]= 3.2 X 10^-8
1) write a chemical equation showing how HOCl behaves as an acid in water.
i got: HOCl + H2O = H3O + OCl
2) calculate the PH of a 0.175 M solution of HOCl.
i got:
HOCl + H2O = H3O + OCl
Initial: 0.175 0 0 0
Change: -x -x +x +x
Equilibrium: 0.175-x -x +x +x
am i doing it right? how do u calculate the PH from x?
3) write the net ionic equation for the reaction between the weak acid HOCl and the strong base NaOH.
I got: HOCl + NaOH = H3O +Na +OH
is it right?
4) In an experiment, 20 mL of 0.175 M of HOCl is placed in a flask and titrated with 6.55 mL of 0.435 M NaOH.
A)Calculate the number of moles of NaOH added.
I did: (6.55/1000) x (0.435 M) = 0.0025
B) Calculate [H3O+] in the flask after the NaOH has been added.
where do i start? i don't get what the question is asking.
C) Calculate [OH-] in the flask after the NaOH has been added.
where do i start? i don't get what the question is asking.
thank you.