Includes all of the explanations of for example buffer’s, lewis theory, strong bases, bronsted-lowry acids & bases (etc). These notes also include the formula’s/ways to calculate values with the IB asks for.
There is also all of the formulas of acid deposition also included. Some graphs are a...
Samenvatting Ib Course Book Chemistry 2014 - Scheikunde
Option D: Medicinal Chemistry (IB Chemistry)
Chapter 11 & 21, Measurements & Data Processing (IB Chemistry)
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VWO / Gymnasium
Scheikunde
6
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INDICATORS SALT HYDROLYSIS
LEWIS THEORY • an acid-base indicator is a weak acid which • an ionic salt is formed from the neutralisation reaction of an acid and base
• LEWIS ACID: an electron pair acceptor, electrophile dissociates to give an anion of a different colour
• LEWIS BASE: an electron pair donor, nucleophile •
•
the conjugate acids/bases are different colours
the colour of the indicator depends on the pH of the
int Mentalisatio Mt
+ <
pH CURVE solution • the ionic salt, MA, formed will dissociate in water
• s-shape curve • colour changes gradually over a pH range • HYDROLYSIS - splitting of a bond using water
• EQUIVALENCE POINT: midpoint of inflection • the pKa of an indicator = pH of its endpoint • the reaction of the salt will vary depending on the strength of the acid and
• pkA = pH at half equivalence —> the stage of the bases used in the neutralisation reaction
titration at which exactly half the amount of …. has been • the use of the different strengths of the acids and bases will directly influence
neutralised the type of salt hydrolysis and the pH of the final solution
pH curves can: • if the Ka is larger = solution will be acidic
• determine the pH of the acid by looking where the curve • if the Kb is larger = solution will be basic
starts on the axis • if Ka = Kb then the pH will be 7
• find the pH at the equivalence point •
• find volume of base at the equivalence point
• obtain the range of pH at the vertical section of the curve ACIDS & BASES FORMULAS SUMMARY
[Hg0t] pOH -logCOH]
BUFFERS pH=-log
=
STRONG ACID + STRONG BASE
.
WEAK BASE + STRONG ACID
·
PH polt
• is a solution which resists changes in pH when small amount of (OH-] 10
-
(H30 ] 10
+
·
·
= =
acid or base are added
(Hz0 ] kw/20H]
+ =
• used to keep the pH almost constant
·
• can consist of weak acid -conjugate base or weak base - ·
pH 14-pot
=
conjugate acid · kw = Ka kp
·
= 10-14
• Equilibrium is reestablished, ex ethanoate ate ions in the buffer 14
pku =
pka + pkp =
solution react with the added H+ to prevent the pH from
decreasing pKb -legkb
pKa -logka =
·
·
=
BUFFER REGION 10-plb
Kn
10-pha
=
Ka
·
• these are seen on a pH curve and represent the region where
=
WEAK ACID + STRONG BASE WEAK ACID + WEAK BASE
·
(BH
+
)(OH]
small addition in acid or base result in little change in the overall Het
<A k
·
=
·
Ka =
[B]
pH of the solution
↳ B +2 = BH
+
+ 04-
• ex;
+
↳ HAJA + H
+
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