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https://www.youtube.com/watch?v=JCAsOJYkn-s

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heres a lil happy diagram for your stress

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heres a lil happy diagram for your stress

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https://www.pinterest.com/pin/168603579774147179/

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yo lets stop being sad and look at quizlet ;)

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yo lets stop being sad and look at quizlet ;)

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KSP
https://quizlet.com/167953437/ap-chemistry-chapter-16-ksp-zumdahl-flash-cards/
TITRATION
https://quizlet.com/208810262/ap-chemistry-titration-flash-cards/
https://quizlet.com/216232420/ap-chemistry-titration-ap-chemistry-acids-and-bases-flash-cards/

:) :) :)

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- dissociation equations - know how to write these!!
-conversion
~ Solubility (g/L) -> Molar Solubility (mol/L) -> Molar concentration of ions -> Ksp ~

1. CALCULATE ONE [ ] OF ONE ION KNOWING THE OTHER
plug into ksp equasion and solve

2. CALCULATE KSP FROM SOLUBILITY
write dissociation equasion for refrence
plug and chug

3. CALCULATE SOLUBILITY FROM KSP
this is where the 4x^3 stuff comes in (quizlet is good for review)

4. CALCULATING THE EFFECT OF A COMMON ION ON SOLUBILITY
common ion affect
5% rule
then just draw diagram if needed for refrence and plug and chug

5. PREDICTING THE EFFECT OF PH ON SOLUBILITY
---metal hydroxides - youll have to solve for concentration
---salts containing basic anions - the solubility of slightly soluble salts containing basic anions increase as the [h+] increases (bc the pH is lowered). the more basic the anion, the more solubility is influenced by pH

6. DETERMINE IF A PRECIPITATE WILL FORM
ion product is Q
Ksp is K
If K<Q then there is a precipitate
If K>Q then there is not
Solid vs ions
solves for k and q then compare

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the point at which the stoichiometrically equivalent quantities of acid and base have been brought together

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1. Strong acid strong base
eq at 7 - salt that is produced has 2 spectator ions and is equally neutral
initial - less than 2
1/2 eq pt - ~2
final ph - greater than 7

2. Strong base strong acid
eq at 7 - salt that is produced has 2 spectator ions and is equally neutral
initial - 12-14
1/2 eq pt - same as inital
final ph - 2-0

3. Weak acid strong BASE
greater than 7 - CB hydrolyzes h20 producing oh-
initial -2-6
1/2 eq pt - pH = pKa of WA
final ph - 12-14

4. weak BASE strong acid
less than 7 - CA hydrolyzes h20 to produce h20+
initial - 12-8
1/2 eq pt - pH = pKa of the conjugate
final ph - about 2
see packet for diagrams and molecule ratios

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the extent of ionization  of a weak electrolyte is decreased by adding to the solution a strong electrolyte that as an ion in common with the weak electrolyte
-tie into Le Chatelier's Principle

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match ph at eq pt
changes color
signals equivalence point

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tools = buret, titrant, ph probe, aliquot, erlenmeyer flask

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the pH renge over which the buffer acts effectively

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the amount of acid or base the buffer can neutralize before the pH beings to change an appreciable degree

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Li+
Na+
K+
Rb+
Cl-
Br-
I-
No3-

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-a buffered solution is one that resists a change in its pH when either hydroxide ions or protons are added
-Will it act as a buffer?
1) is it a conjugate system
2) strong or weak acid - strong means no
-Affect of adding acid or base to buffer
~Weak acid consumes hydroxide to form a super weak base
~single sided arrows bc theres strong ions and they react completely
-preparing a buffer

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it is- the extent of ionization of a weak electrolyte is decreased by adding to the solution a strong electrolyte that has an ion in common with the weak electrolytes
-it is an application of leChatelier’s principle
-ice tables are still applicable yo yo yooo :)