Speghetti

Finally graduated with my bachelor's in mechanical engineering. Let's learn Japanese.

[japanesewords]

マスクを付ける

[japanesewords]

新たな始まり| aratana hajimari | new beginnings

[hereisrobspeghetti]

I also wrote an entry for our weekly wiki entry, which pretty much sums up a topic of something we discussed in class that week. Started out professional and slipped into obnoxiousness. I chose pH and pOH.

pH and pOH of Solutions The strength of an acid is determined solely on the quantity of [H+] ions in a solution.

Monoprotic Acids- a substance is called a monoprotic acid if it dissociates into a solution, such as water, and donates only one [H+] ion into said solution. (Such as HCl)

Polyprotic Acids- a substance is deemed a polyprotic acid if it dissociates into a solution and donates multiple [H+] ions into said solution. (Such as H2SO4) <--Super important to remember those multiple H+ ions in calculation! Calculation for pH

Example 1 MONOPROTIC What is the pH of an HCL solution with a molarity of 8.675309x10-3?? Plug that molarity into this super cool pH equation and get your pH value super fast! --> pH= -log[H+] ---> -log[8.675309x10-3]= 2.0617150 Does a solution at 2 on the pH scale seem acidic to you? IT SHOULD, BRO!!

Example 2 POLYPROTIC What is the pH of an H2SO4 solution with a molarity of 1.23321x10-4]?? WATCH OUT BRO,  ^^^ Peep those two sweet [H+] ions who are about to break it off with their main bae! Let's plug and chug again, but don't forget that these two bromancers are leaving the scene together. -->pH= -log[(2)(1.23321x10-4)]= 3.607933   A 3 ON THE pH scale is MAD ACIDIC BRO.

Example 3 "But mine is so basic" You've got a basic molecule, like NaOH ([OH-]) that you need to find the pH value for? No problem. Repeat the steps above, and subtract your calculated value by 14, which is the most basic you can get on a pH scale. Your answer should end up closest to the basic side of the pH scale (which is 14, if you have the memory of a goldfish, bro).

Example 4 "Bro, you didn't let me finish, I needed the pOH of NaOH *cough* which has a molarity of of 1.05x10-3 *cough*.

Bro, I'm so sorry bro, that was so rude of me bro. To find the pOH of a molecule, use the same equation, but now just realize that we're focusing on the dissociation of  [OH-] ions into a solution. Plug town--> pOH = -log[OH-] --> -log[1.05x10-3] = 2.979 "But bro, isn't a pOH value of about 3 still acidic?" NO BRO, you're fine! See, chemists like to waste college students' time, by flipping the amazingly perfect and understandable pH scale on its butt, so now the lower the number is on the pOH scale, the more basic it is. This is just their way of trying to keep toats amaze bros like you and me out of their labs by tricking us. Don't freak bro, we got this.

ONE LAST THING When calculating for your pH or pOH(so lame) values, make sure your significant figures AFTER the decimal reflect the amount of numbers in the molarity of the solution. We're dealing with logs here, and thems the brakes, kid.

Ex: What is the pH of BLAH with 1.234x10who cares M      your calculated pH value= 1.1234    <---4 in the molarity, so 4 after that decimal. -Rob Gomez

[hereisrobspeghetti]

Super proud of my response to this week's discussion board entry for Chem2!

Teacher's Required Question: How do the definitions of strong and weak when they refer to acids relate to equilibrium?                  

Robert Gomez                                                                                                      RE: Required Question                                

The strength of an acid refers to its speed of dissociating into ions when dissolved in water(H2O). The stronger the acid, the more completely it will dissociate into ions, whereas the weaker an acid, the more inconsiderable the dissociation.

Since stronger acids dissociate their ions into water almost completely (like extroverted romancers heading into a pool party), the hydronium ion concentration is essentially the same as the original acid concentration.

HA + (water) --> A- + H3O+ (it's essentially a complete reaction (all the lovers found love))

Proton transfer from weak acid to water molecules becomes balanced from proton transfer from hydronium to A-, so the hydronium concentration is much less than the original acid concentration. Weak acids also have a larger concentration of HA molecules after they've been introduced to water. The solution becomes balanced before all of the weak acid (HA) can be dissociated into ions. It's like a bunch of introverts arriving late to a party (that they were probably dragged into going to by their friends) and having no romantic opportunities to grab onto, because those who arrived promptly before them have already courted the lions and lionesses before they could.

It's like when I was 18.

Weak acids are like Rob Gomez when he was 18 (and all the way up to now).

HA + (water) <--> A- + H3O+ (it's essentially an equilibrium reaction)

^^ (see there is me with all the other losers (non-dissociated weak acid molecules) hanging by the H2O (drink cooler), stuck in party limbo (equilibrium))

I hope my answer has answered your poorly sentenced question.