New User Special Price Expires in

Let's log you in.

Sign in with Facebook


Don't have a StudySoup account? Create one here!


Create a StudySoup account

Be part of our community, it's free to join!

Sign up with Facebook


Create your account
By creating an account you agree to StudySoup's terms and conditions and privacy policy

Already have a StudySoup account? Login here

Chem week 5 notes

Star Star Star
1 review
by: Hanna Notetaker

Chem week 5 notes CHEM-10055-003-201580

Hanna Notetaker

Preview These Notes for FREE

Get a free preview of these Notes, just enter your email below.

Unlock Preview
Unlock Preview

Preview these materials now for free

Why put in your email? Get access to more of this material and other relevant free materials for your school

View Preview

About this Document

Week 5 of Chemistry notes. Covers acids and bases through molecular compounds
Bansidhar Datta (P)
Class Notes
25 ?




Star Star Star
1 review
Star Star Star
"this site is not very user friendly."
lori holcepl


Popular in Chemistry

This 13 page Class Notes was uploaded by Hanna Notetaker on Wednesday September 30, 2015. The Class Notes belongs to CHEM-10055-003-201580 at Kent State University taught by Bansidhar Datta (P) in Fall 2015. Since its upload, it has received 105 views. For similar materials see MOLECULES OF LIFE in Chemistry at Kent State University.


Reviews for Chem week 5 notes

Star Star Star

this site is not very user friendly.

-lori holcepl


Report this Material


What is Karma?


Karma is the currency of StudySoup.

You can buy or earn more Karma at anytime and redeem it for class notes, study guides, flashcards, and more!

Date Created: 09/30/15
Chemistry  week  5   9/  28   •   Water  is  amphiprotic,  can  donate  or  accept  protons   •   Water  can  be  acid  or  base   •   pH  +  pOH  =  14     + o   example:    H O  + 2H O     2               H3O  +  OH   §   arrows  going  both  ways  show:   •   equilibrium   •   rate  of  going  forward  is  equal  to  the  rate  of   reverse   •   dissolves     + – •   H O 3  =  OH       -­‐   o   pOH  =  -­‐  log  (OH )     + -­‐7   pH  =  -­‐  log  (3 O )   pOH=    -­‐log  10   -­‐7     pH=  -­‐  log  10   pOH=  7  x  log  10                      pH  =  7  x  log  10   pOH=  7     -­‐       pH=  7       (pH)  7  +  (pOH)  7  =  14       •   strong  acid  =  dissociates  in  water  100%     •   weak  acid=  dissociates  partly  in  water       + -­‐   HA  +  H 2           3               H O  +  A + -­‐ K equilibrium  =  3H O ]  [A ]       ß  product                    2HA]  [H O]                                      ß  reactant     K a  =  dissociation  constant  of  weak  acid  HA   K a  =  H O3]  [A ]                  [HA]       Conjugate  acids  &  bases   •   Acids  with  or  without  protons   •   Bases  with  or  without  hydroxide  group   •   Weak  acid  (HA)  /  conjugate  base  (A -­‐)   •   Base  (H2O)  /  conjugate  acid  (H3O)   •   The  weaker  the  acid  is,  the  stronger  the  conjugate  base  is   •   The  stronger  the  acid,  the  weaker  the  conjugate  base  is     Conjugate  Base   The  conjugate  base  is  made  when  the  acid  gives  away  a  proton   2   OH  =  conjugate  base  when  H2O  =  acid  because    H2O  gives  a   hydrogen  away  to  make  OH     Conjugate  Acid   =  base  w/  hydrogen  added  to  it     3                       Properties     Acids     Physical  properties:   •   Sour   •   Colorless   •   Odorless   •   Usually  liquid     Chemical  reactions  with:   Metals   o   Metals  that  react  with  an  acid  form  metal  hydroxide  gas   §   Example:  Na  +  HCl  =  NaCl  +  H   2 Metal  oxides   o   Metal  oxides  that  react  with   acids  make  salt  and  water   o   Example:  K  +  HBr 2  =  KBr  +  H O   2 4   Metal  hydroxides  (neutralization  reaction)   o   Metal  hydroxides  that  react  with  acid  make  a  Salt  and   water   o   Example:  NaOH  +  HNO  =3  NaNO  +3  H 2    Bases   •   Bitter   •   Slippery   •   Colorless   •   Odorless   •   Solid     Applications  of  neutralization  Reaction   o   Antacids:   o    Some  bases:  CaCO ,3  Mh(OH) , 2Al(OH) ,  3nd  NaHCO     o   some  examples:  milk  of  magnesia,  Maalox  mylanta,  tums     o   stomachs  contains  HCl,  if  there  is  too  much,  heartburn  can   occur,  so  antacids  are  taken  neutralize     o   example:  CaCo  +3  HCl  =  CaCl2  + 2  O 2 +  H O   §   HCl  =  in  stomach   §    CaCO3  =  tums     o   balances  out/  neutralizes  acid  in  stomach  to  relieve     o   NaHCO  =3  Sodium  Carbonate  =  baking  soda  =  very  strong   Applications  of  Acids:     o   Vinegar:  Acetic  acid,  CH COOH,  used  in  cooking,  preservatives   3 o   Boric  acid:  H BO ,  antiseptic,  for  eyes  especially   3 3 5   o   Phosphoric  acid:  H PO ,  in  3io  m4cromolecules  (proteins,  sugars,   lipids,  nucleic  acids)     o   Hydrochloric  Acid:  HCl,  used  in  stomachs  to  digest  food   Applications  of  Bases:   o   Ammonia:  NH ,  fertilizer3,  urea,  cleaning  revives  fainted  people   o   Magnesium  Hydroxide:  MgOH ,  laxative  (8%),  “milk2  of  magnesia”,   metal  plant  waste,  plastics-­‐  flame  retardant   Buffers=  a  solution  that  has  a  weak  acid  and  its  conjugate  base,  resists   change  when  a  little  amount  of  acid  or  base  is  added  to  it       Buffer  capacity=  strength  of  buffer   H O2  =least  buffer  capacity     HA/A  ratio  defines  the  capacity  of  the  buffer     + -­‐             Equilibrium-­‐  HA                  H    A Henderson  Hasselbach  equation:           HA  +  H O2         3         H O  +  A           pH  =  pKa  +  log  A-­‐               HA   When  pH  is  almost  equal  to  pKa,  it  is  a  good  buffer     9/30   Strong  acids  =  no  Ka  (they  dissociate  completely)   Weak  acid  =  has   a   -­‐ K a=  (H O)3  (A )          (HA)   6     Acids:     -­‐5   CH COOH3   Acetic  Acid     Ka=  1.8  x  10 weaker   -­‐4 HCOOH   Formic  Acid   Ka=  1.8  x  10   weak   H CO Carbonic  Acid   Ka=  4.3  x  10   -­‐7 weakest   2 3       •   The  lower  the  value  of  Ka,  the  weaker  the  acid   •   The  higher  the  pKa,  the  weaker  the  acid   pKa  =  -­‐log  Ka       HA  +  H O  2     H O 3  +  A   -­‐ By  switching  (     )  it  shows  that  they  balance       H2O  +  H2O       H3O  +  OH-­‐   K  equilibrium  =  (H3O+)  (OH-­‐)              (H2O)     -­‐3 + -­‐ -­‐14 H2O  +  acid  è  10    M       [H3O ]  [OH ]  =  10     -­‐3 -­‐14               10 x  [OH]=  10   -­‐14 -­‐11             or     [OH-­‐]  =  10  =10   -­‐3                     10   7   Weak  Acid  [HA]   HA  +  H2O       H3O  +  A -­‐   pH=  pKa  +log        A-­‐                    HA   1.  If  HA  =  10  [A-­‐]  then  pH=  pKa  =  A  =  pKa  +log(10 )   -­‐1 -­‐               10(A )   -­‐   2.  if  A  =  10  [HA]  then  pH=  pKa  +log  10  HA     =pKa  +log10     HA   =  pKa  +1     •   Water  =  BAD  BUFFER   •   Weak  acids  =  GOOD  BUFFER   •   If  pH  =  pKa  of  HA  =  best  buffer     Buffers  in  the  Human  Body   -­‐ OPEN  SYSTEM  (HCO  /  CO (d)  )3   2 •   Open  to  the  environment  and  physical  conditions   •   HCO  =  A-­‐         CO2=  HA       d=  dissolved   •   CO2  gas  goes  to  the  lungs,  its  dissolved  by  alveoli ,  water&  enzyme   à    H2CO  3 o   CO  (2)  à  CO  (d)2               2        CO2  (d)  +  H O 2  (l) 3 à  H CO  (l)   o   Equal  to:  H CO  2  + 3 H O    2         H O3  +  HCO   3 -­‐ o   (l)  =  liquid     (g)  =  g     -­‐ o   pH=  pKa   overall  +log  [HCO ]   3       2      CO 8   o   pH=  pKa   overall  +log  [HCO ]3       =    6.1  +log  (HCO3)        2       C             2                         [CO ][HA]       2-­‐ -­‐ CLOSED  SYSTEM  (HPO  /  H 4PO )   2 4 •   Inside  cells  (enzymatic  functions)   •   PO  àH PO   4 3 4   + H 3O +H O4   2  H P2 +H O4   3 pKa  =  2.12   + H 3O +H O4   2  H P2 +H O4   3     pKa  =  7.2         best  ot  of  2  equations  b/c  7.2  is  close  to  7.4  (7.4  =  pH  of  blood)   +   H 3O +H O4   2  H P2 +H O4   3   pKa  =  12.1         PLASMA  IN  OUR  BLOOD   •   pH  of  blood  =  7.4   -­‐ •   pH=  6.1  +log  HCO   3                            all  together  =  7.4       2    CO   •   conditions:   o   acidosis     §   if  CO2  in  blood  is  HIGH   §   pH  is  less  than  6.1   §   metabolic  acidosis     §    respiratory  acidosis=   9   •   CO2  cant  get  out,  too  much  of  the  CO2  in  the   blood,  windpipe  collapse=  Asthma  patient   o    Alkalosis   §   if  CO2  dissolves  in  blood  &there  is  a  LOW  amount  of   plasma     §   pH  =  greater  than  7.5   §   respiratory=   •   from  high  fever,  bleeding,  drug  use   •   metabolic=   o   enzymes     Indicators  of  pH   •   Larger  molecular  compounds  change  color  at  varying  pH  levels     o   Example:  paper  that  changes  color  at  different  pH  levels,  is   the  pH  level  is  less  than  7  the  litmus  paper  turns  red,  if  pH  is   bigger  than  7  it  turns  blue   §   Example:  pregnancy  test                     10   Naming  and  Molecular  Compounds     Compounds  w/  non  metals  and  metalloids     •   Number  of  electrons  on  the  outer  shell  of  non  metals  and   metalloids     •   Non  metals  +  non  metals  make  molecular  compounds     •   Non  metals=  C,  H,  O,  N,  F,  P,  S,  Cl,  Se,  Br,  I   •   Metalloids=  B,  Si,  As,  Sb,  Ge,  Te   •   PIC       H  has  one  valence  electron  that  will  for  bonds   H  is  a  atom,  2  makes  a  molecule     11       12                     13  


Buy Material

Are you sure you want to buy this material for

25 Karma

Buy Material

BOOM! Enjoy Your Free Notes!

We've added these Notes to your profile, click here to view them now.


You're already Subscribed!

Looks like you've already subscribed to StudySoup, you won't need to purchase another subscription to get this material. To access this material simply click 'View Full Document'

Why people love StudySoup

Bentley McCaw University of Florida

"I was shooting for a perfect 4.0 GPA this semester. Having StudySoup as a study aid was critical to helping me achieve my goal...and I nailed it!"

Anthony Lee UC Santa Barbara

"I bought an awesome study guide, which helped me get an A in my Math 34B class this quarter!"

Jim McGreen Ohio University

"Knowing I can count on the Elite Notetaker in my class allows me to focus on what the professor is saying instead of just scribbling notes the whole time and falling behind."


"Their 'Elite Notetakers' are making over $1,200/month in sales by creating high quality content that helps their classmates in a time of need."

Become an Elite Notetaker and start selling your notes online!

Refund Policy


All subscriptions to StudySoup are paid in full at the time of subscribing. To change your credit card information or to cancel your subscription, go to "Edit Settings". All credit card information will be available there. If you should decide to cancel your subscription, it will continue to be valid until the next payment period, as all payments for the current period were made in advance. For special circumstances, please email


StudySoup has more than 1 million course-specific study resources to help students study smarter. If you’re having trouble finding what you’re looking for, our customer support team can help you find what you need! Feel free to contact them here:

Recurring Subscriptions: If you have canceled your recurring subscription on the day of renewal and have not downloaded any documents, you may request a refund by submitting an email to

Satisfaction Guarantee: If you’re not satisfied with your subscription, you can contact us for further help. Contact must be made within 3 business days of your subscription purchase and your refund request will be subject for review.

Please Note: Refunds can never be provided more than 30 days after the initial purchase date regardless of your activity on the site.