H3O+=1x10^-14/1.36x10^-2. H3O+=7.35x10^-13. pH=(-H3O+)=-log(7.5x10^-13). pH=12.13. Explain step...


H3O+=1x10{eq}^{-14} {/eq}/1.36x10{eq}^{-2} {/eq}.

H3O+=7.35x10{eq}^{-13} {/eq}.

pH=(-H3O+)=-log(7.5x10{eq}^{-13} {/eq}).


Explain step by step.

Relationship of Ion Concentrations and Water:

When a reaction produces water as a product or is in aqueous solution, there is an equilibrium relationship between the equilibrium of hydrogen (hydronium) ions and hydroxide ions. This is the case seen with acid-base reactions. The equilibrium relationship is called the ion-product constant for water, Kw, and is {eq}K_w\:=\:[H^+][OH^-]\:=\:[H_3O^+][OH^-]\:=\:1\times 10^{-14} {/eq}.

Answer and Explanation:

Although we must make an assumption here that one of the values is the hydroxide ion concentration (1.36 x 10-2), the first step is a rearrangement of...

See full answer below.

Become a member to unlock this answer! Create your account

View this answer

Learn more about this topic:

Hydronium Ion: Definition & Formula

from College Chemistry: Homework Help Resource

Chapter 5 / Lesson 24

Related to this Question

Explore our homework questions and answers library