Chemistry 1024A/B Lecture Notes - Lecture 7: Strontium Hydroxide, Equilibrium Constant, Ph

• School: Western University
• Department: Chemistry
• Course: Chemistry 1024A/B
• Professor: Zhifeng Ding

Document Summary

I(cid:374) (cid:449)ater, (cid:374)ot all the (cid:373)ole(cid:272)ules are prese(cid:374)t as (cid:862)h2o(cid:863). Therefore, pure water represents a mixture of h2o molecules, h+ ions and oh- ions. The equilibrium constant of this process is called the ionization constant of water: if [h+] > [oh-], the solution is acidic, if [h+] = [oh-], the solution is neutral, if [h+] < [oh-], the solution is basic. The acidity (or basicity) of a solution is described by its ph value (power of the hydrogen ion) in mol/l!!! Chapter 7. 3 ph of strong acid and base solutions. Strong acids and bases are completely dissociated in water. When you try to calculate know, if for a strong acid (like hcl), the ph would equal zero and the poh would equal 14 and vice versa. Strong acids: hi, hbr, hclo4, hclo3, h2so4, hno3, hcl. An acid is a species that produces. A base is a species that produces ions in water ions in water.