pH and pOH

Today, we learned more about the pH and pOH.

pH can be defined as the negative logarithm of the hydronium ion concentration, or
pH=-log[H3O]
pOH can be defined as the negative logarithm of the hydroxide ion concentration, or
pH=-log[OH]

remember: pH + pOH = 14.

to learn more about the calculations with pH and pOH, ms. K went over Acid-Base Assignment #6 , numbers 1-4. The answers for these problems are posted below this post.

After going over the calculations for this problems, ms. K handed us RELATIVE STRENGTHS OF ACIDS and ACID DISSOCIATION CONSTANT. On the second worksheet we learned the difference between Ka and Kb.

Ka is the acid dissociation constant or ionization constant. The larger the Ka, the stronger the acid and therefore there's more product and thats there's greater dissociation. The smaller the Ka, the less the product and therefore weaker acid.

Kb is the base dissociation constant. It reflects the strength of a base. the higher the base, the higher the value of Kb will be.

We also went over how to CALCULATE THE DISSOCIATION CONSTANT. Its almost the same as how to calculate the equilibrium constant, by setting up an ic table. Also, Ka and Kb has no units, just like Kc.

LAB IS DUE TODAY.

the next scribe is LARLYN:))