Bronsted-Lowry acids and bases

Chemistry and homework help forum.

Organic Chemistry, Analytical Chemistry, Biochemistry, Physical Chemistry, Computational Chemistry, Theoretical Chemistry, High School Chemistry, Colledge Chemistry and University Chemistry Forum.

Share your chemistry ideas, discuss chemical problems, ask for help with scientific chemistry questions, inspire others by your chemistry vision!

Please feel free to start a scientific chemistry discussion here!

Discuss chemistry homework problems with experts!

Ask for help with chemical questions and help others with your chemistry knowledge!

Moderators: Xen, expert, ChenBeier

Post Reply
User avatar
Dhamnekar Winod
Distinguished Member
Distinguished Member
Posts: 257
Joined: Sat Nov 21, 2020 10:14 am
Location: Mumbai[Bombay] and Mumbai Suburb,, Maharashtra State,India

Bronsted-Lowry acids and bases

Post by Dhamnekar Winod »

Consider the example of dissolution of Na(s) in H2O(l) represented by the following equation:

\(Na(s) + H_2O(l) \rightleftharpoons NaOH(s) + H^+\). Now, In this case, which is conjugate acid and which is conjugate base?
Any science consists of the following process. 1) See 2)Hear 3)Smell,if needed 4)Taste, if needed 5)Think 6)Understand 7)Inference 8)Take decision [Believe or disbelieve, useful or useless, true or false, cause or effect, any other criteria]
User avatar
ChenBeier
Distinguished Member
Distinguished Member
Posts: 1542
Joined: Wed Sep 27, 2017 7:25 am
Location: Berlin, Germany

Re: Bronsted-Lowry acids and bases

Post by ChenBeier »

Its not working like this. The equation is not balanced according the charge.

2 Na + 2 H2O => 2 NaOH + H2 !!!!! No H+,

NaOH => Na+ + OH-
Post Reply