Confusion on Friday's lecture  [ENDORSED]

Moderators: Chem_Mod, Chem_Admin

Anna De Schutter - 1A
Posts: 66
Joined: Wed Feb 21, 2018 3:01 am

Confusion on Friday's lecture

Postby Anna De Schutter - 1A » Sun Jun 10, 2018 4:36 pm

Hi!

For last Friday's lecture I wrote down in my notes that: Cl- is "good on its own" in a solution as shown by the equation HCl --> H+ + Cl-
I'm a bit confused by this though, how can we know Cl- won't affect the reaction through this equation? Is this also why Cl- doesn't affect the pH of water?

Thank you!!
Anna De Schutter - section 1A

Chem_Mod
Posts: 18400
Joined: Thu Aug 04, 2011 1:53 pm
Has upvoted: 435 times

Re: Confusion on Friday's lecture  [ENDORSED]

Postby Chem_Mod » Sun Jun 10, 2018 5:47 pm

As I discussed in class. Think of adding salt to water. :-)

Na+Cl- dissolves in water and each are stable as Na+ and Cl- solvated (surrounded) by water molecules.

There are no additional reactions and therefore both Na+ and Cl- do not change the pH of water.

Anna De Schutter - 1A
Posts: 66
Joined: Wed Feb 21, 2018 3:01 am

Re: Confusion on Friday's lecture

Postby Anna De Schutter - 1A » Sun Jun 10, 2018 11:54 pm

Thank you Dr. Lavelle! :)


Return to “Calculating pH or pOH for Strong & Weak Acids & Bases”

Who is online

Users browsing this forum: No registered users and 2 guests