Talk:Weak base

Percentages

Is percentage protonated the same as percentage ionised? Copperman 15:06, 29 May 2006 (UTC)

Tasting a base

Moved to Base page discussion where it belongs.

Chemperson 23:10, 25 April 2007 (UTC)

Ammonia

Ammonia is a weak base??? —Preceding unsigned comment added by 71.197.152.41 (talk) 00:29, 12 March 2009 (UTC)

Weak Base, Water

Your first question will might be, well what is a weak base? In chemistry, a weak base is a chemical base that does not ionize fully in an aqueous solution. As Brønsted–Lowry bases are proton acceptors, a weak base may also be defined as a chemical base in which protonation is incomplete. This results in a relatively low pH compared to strong bases. Bases range from a pH of greater than 7 (7 is neutral, like pure water) to 14 (though some bases are greater than 14).

In this topic we will be discussing about WATER being a "weak base." We will be talking about the dissociation reaction (breaking into ions) The dissociation constant of K value (and describe what this means) Its phase at room temperature Its reaction with weak bases and acids as well with strong bases and acids. The conjugate acid or base from the weak acid/base reaction Its formula Molar Mass Structure Safety hazards with water And Everyday uses

• First lets talk about The dissociation reaction in water. ~When water dissociates, one of the hydrogen nuclei leaves its electron behind with the oxygen atom to become a hydrogen ion, while the oxygen and other hydrogen atoms become a hydroxide ion. Since the hydrogen ion has no electron to neutralize the positive charge on its proton, it has a full unit of positive charge and is symbolized as H+. The hydroxide ion retains the electron left behind and thus has a full unit of negative charge, symbolized by OH-. The hydrogen ion (proton) does not wander long by itself before it attaches to the oxygen atom of a second un-ionized water molecule to form a hydronium ion (H3O +)

• The dissociation constant of K value. ~The base dissociation constant K measures a base relative strength. With this it can help you find out either you base is string or weak and it can also help you find if either your acid is also weak or strong.

• Its phase at room temperature. ~When water temperature reaches 100 ∘C 100 ∘C, the molecules get so excited that the hydrogen atoms lose the bonds to the oxygen atom and therefore the water starts to become gas. You can also just leave water out randomly and see how it starts to become gas, but this process will take a couple of days with no help of heat.

• Its reaction with weak bases and acids as well with strong bases and acids. ~Acids and bases exist as conjugate acid-base pairs. The term conjugate comes from the Latin stems meaning "joined together" and refers to things that are joined, particularly in pairs, such as Brnsted acids and bases. Water can help when using chemicals it may help dilute it. It can be used with acids or it can just simply also be used just as a base.

• Its formula. ~It is simply H2O. So this is saying that for every 2 hydrogen's you add in you also get 1 oxygen with it.

• Molar Mass. ~18.01528 g/mol

This was a talk from Me David and I honestly hope this while help you out in any chemistry questions you might have over weak bases.

~ SOURCES ~ https://www.bpcc.edu/sciencealliedhealth/slm/chem107/Acid-Base/mobile_pages/Acid-Base3.html

http://imnh.isu.edu/digitalatlas/hydr/basics/main/chmtxt.htm — Preceding unsigned comment added by Papi David (talk • contribs) 16:55, 20 April 2017 (UTC) thank you

https://www.boundless.com/chemistry/textbooks/boundless-chemistry-textbook/acids-and-bases-15/strength-of-bases-110/base-dissociation-constant-461-613/

Equations ad Nauseam

The lead section has a good number of equations and in-depth explanations of concepts such as calculating an equilibrium constant and what-not that should probably be moved to a page about the broad subject of pH, or moved to a less prominent section, to look more like an easily read and well-polished wikipedia article.

What really bothers me (aside from the lead section) is the section title "A Typical pH Problem." It strikes me as odd that the section here is being employed as a demonstration on how to use equations, and goes nowhere on discussing what a weak base actually is. Either way, even if it is relevant, the title of the section should be changed to something that doesn't scream homework.

This has given the page the look of a chemistry textbook, and the memories associated with that are not fun, and keep in mind chem textbooks are meant to be thick and have extraneous info so they sell for more money, while a Wikipedia page should be more readable than that, but of course doesn't need to be spoonfed like a children's book. As I would like to demonstrate a point, here is sort of what I think the lead section should sort of look like (from the wikipedia article on Acid Strength, the weak acid section; the first sentence was removed, as it only contributed to attach it to the previous elements in the page):

A weak acid is an acid that dissociates incompletely, releasing only some of its hydrogen atoms into the solution. Thus, it is less capable than a strong acid at donating protons. These acids have higher pKa than strong acids, which release all of their hydrogen atoms when dissolved in water. Examples of weak acids include acetic acid (CH3COOH), phosphoric acid (H3PO4), hydrofluoric acid (HF) and oxalic acid (H2C2O4).

Overall, the main problem I have with this page is the unwieldy number of equations that are useful, but simply not well placed, and my lack of knowledge on where they would fit in. Thank you to anyone who could give me pointers or get a solution in!

Badmonkey717 (talk) 21:54, 23 May 2017 (UTC)