Solvent system definition of acids and basesSourovPaul6
This PPT is about the solvent system definition of acids and bases in inorganic chemistry . This power point is useful to those who study chemistry in college and also useful for University students and also for PhD students
In chemistry, acids and bases have been defined differently by three sets of theories. One is the Arrhenius definition, which revolves around the idea that acids are substances that ionize (break off) in an aqueous solution to produce hydrogen (H+) ions while bases produce hydroxide (OH-) ions in solution.
Auto ionization of water-self ionization, It is an example of autoprotolysis, and exemplifies the amphoteric nature of water, intermolecular proton transfer that forms a hydronium ion (H3O+) and a hydroxide ion (OH – ):
Dissociation of water-Dissociation constant-K
Molar concentration of water, ion product for water (Kw)
pH, pka-Relating pH and pka with Henderson Hasselbalch equation, Examples for pH and pka problem,
Acids and Bases-Conjugate acids and conjugate base. dissociation constant of water.
Solvent system definition of acids and basesSourovPaul6
This PPT is about the solvent system definition of acids and bases in inorganic chemistry . This power point is useful to those who study chemistry in college and also useful for University students and also for PhD students
In chemistry, acids and bases have been defined differently by three sets of theories. One is the Arrhenius definition, which revolves around the idea that acids are substances that ionize (break off) in an aqueous solution to produce hydrogen (H+) ions while bases produce hydroxide (OH-) ions in solution.
Auto ionization of water-self ionization, It is an example of autoprotolysis, and exemplifies the amphoteric nature of water, intermolecular proton transfer that forms a hydronium ion (H3O+) and a hydroxide ion (OH – ):
Dissociation of water-Dissociation constant-K
Molar concentration of water, ion product for water (Kw)
pH, pka-Relating pH and pka with Henderson Hasselbalch equation, Examples for pH and pka problem,
Acids and Bases-Conjugate acids and conjugate base. dissociation constant of water.
Acids and bases buffers ARRHENIUS CONCEPT
THE LEWIS CONCEPT-THE ELECTRON DONOR ACCEPTOR SYSTEM
BRONSTED-LOWRY CONCEPT (PROTON TRANSFER
THEORY
buffer action
ph scale
buffer capacity
acid base balance
isotonicity method
isotonic soltions
buffer solutions in pharmaceutical preparations
Application of Statistical and mathematical equations in Chemistry Part 5Awad Albalwi
Application of Statistical and mathematical equations in Chemistry
Part 5
Strong Acids and Bases
Ph theory
Weak Acids and Weak Bases
Salts of Weak Acids and Bases theory
A buffer solution theory
POLYPROTIC ACID IONIZATION
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students that opportunity and have been hijacked to become venues for the promotion of terrorism, antisemitic harassment and intimidation, unlawful encampments, and in some cases, assaults and riots.
The House of Representatives will not countenance the use of federal funds to indoctrinate students into hateful, antisemitic, anti-American supporters of terrorism. Investigations into campus antisemitism by the Committee on Education and the Workforce and the Committee on Ways and Means have been expanded into a Congress-wide probe across all relevant jurisdictions to address this national crisis. The undersigned Committees will conduct oversight into the use of federal funds at MIT and its learning environment under authorities granted to each Committee.
• The Committee on Education and the Workforce has been investigating your institution since December 7, 2023. The Committee has broad jurisdiction over postsecondary education, including its compliance with Title VI of the Civil Rights Act, campus safety concerns over disruptions to the learning environment, and the awarding of federal student aid under the Higher Education Act.
• The Committee on Oversight and Accountability is investigating the sources of funding and other support flowing to groups espousing pro-Hamas propaganda and engaged in antisemitic harassment and intimidation of students. The Committee on Oversight and Accountability is the principal oversight committee of the US House of Representatives and has broad authority to investigate “any matter” at “any time” under House Rule X.
• The Committee on Ways and Means has been investigating several universities since November 15, 2023, when the Committee held a hearing entitled From Ivory Towers to Dark Corners: Investigating the Nexus Between Antisemitism, Tax-Exempt Universities, and Terror Financing. The Committee followed the hearing with letters to those institutions on January 10, 202
Instructions for Submissions thorugh G- Classroom.pptxJheel Barad
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3. Acid:Acid: a substance that produces H+
ions
(meaning H3O+
) in aqueous solution.
Base:Base: a substance that produces OH-
ions in aqueous solution.
10. Acid:Acid: a substance that produces H+
ions (meaning H3O+
)in aqueous
solution.
Base:Base: a substance that produces OH-
ions in aqueous solution.
This definition of an acid is a slight modification of the original Arrhenius definition (1884),
which was that an acid produces H+
in aqueous solution
11. Strong acid:Strong acid: dissociates and reacts completely with water to form H3O+
ions.
Strong base:Strong base: dissociates and reacts completely with water to form OH-
ions.
12. Many bases like KOH, NaOH, Mg(OH)2, and Ca(OH)2] disassociate in
water producing OH-
ions (basic solution):
Other bases produce OH-
by reacting with water molecules, here shown
for ammonia:
13. Weak acid:Weak acid: a substance that dissociates partially in water
to produce H3O+
ions.
acetic acid: 4 out every 1000 molecules are converted to acetate ions
Weak base:Weak base: a substance that produces OH-
ions in water in
a reversible reaction.
ammonia, for example, is a weak base:
14. 1. strong acid
2. strong base
3. weak acid
4. weak base
NH3 is classified as a:
17. Acids are proton donors and bases are proton acceptors. An acid-
base (neutralization) reaction is a proton transfer reaction.
HCl + NaOH H2O + NaCl
(strong acid) (strong base) (dissociated in water)
A neutralization reaction between a strong acid an a strong base usually
produces water (depending on what the acid and the base are).
18. In a neutralization reaction hydrochloric acid
(HCl) will react with each of the following
reactants to produce water, except:
1. NaOH
2. Ba(OH)2
3. Mg (magnesium metal)
4. LiOH
19. Equilibrium/Ionization Constants
When a weak acid, HA, dissolves in water
the equilibrium constant expression, Keq, for this ionization is:
Water is the solvent and its concentration changes very little when we add HA,
we treat [H2O] as a constant equal to 1000 g/L or 55.5 mol/L. We combine the
two constants to give the acid ionization constant, Ka:
20. pKa = -log Ka
Note the inverse relationship between values of Ka and pKa. The weaker the
acid, the smaller its Ka, but the larger its pKa.
21. What is the pKa of nitrous acid, if it has a
Ka of 4.0 x 10-4
?
1. -3.4
2. 3.4
3. -4.0
4. 4.0
23. A FEW IMPORTANT FACTS
1. An acid and bases can be positively charged, neutral,
or negatively charged (see table)
2. Acids are classified a monoprotic, diprotic, or triprotic
depending on the number of protons each may give up
ie HCl (gives only one away), H2CO3 (can give 2), and
H3PO4 (can give 3).
3. Several molecules/ions can either accept or donate a
H+
(they can function as acid or base) and are called
amphiproticamphiprotic. ie H2PO4
-
24. 4. A Brønsted-Lowry acid always contains a hydrogen atom
to give away, but not all hydrogen containing compounds
are acids, i.e. CH4 contains hydrogens but does not give
any one away!!!
5. There is an inverse relationship between the strength of
an acid and the strength of its conjugate base (see
table).
25. Conjugate acid-base pair:Conjugate acid-base pair: any pair of molecules or ions that can
be interconverted by transfer of one proton (H+
).
For a conjugate acid-base pair
Ka x Kb = 1x10-14
26.
27. Acid-Base Equilibria
But what if the base is not water? How can we determine
whether the equilibrium lies to the left or the right?
28. To predict the position of an acid-base equilibrium :
Identify the stronger acid and the weaker acid.
Identify the stronger base and the weaker base
(the stronger acid gives the weaker conjugate base, and the weaker acid
gives the stronger conjugate base).
The equilibrium position always favors formation of the weaker acid
and weaker base. At equilibrium the major species present are the
weaker acid and the weaker base.
29. Ka = 1.8 x 10-5
Ka = 5.6 x 10-10
Kb = 1.8 x 10-5
Kb = 5.6 x 10-10
For a conjugate acid-base pair
Ka x Kb = 1x10-14
30. 1.
2.
3.
4.
For the following reaction, equilibrium lies to the
_______ and _______ is the stronger acid.
C6H5OH + H2PO4
-
= H3PO4 + C6H5O-
32. The product of [H3O+
] and [OH-
] in any aqueous solution is
equal to 1.0 x 10-14
.
If we add 0.010 mol of HCl to 1.00 liter of pure water, in
this solution [H3O+
] = 0.010 or 1.0 x 10-2
. This means that
the concentration of hydroxide ion is:
wKOHOH ==−+ -14
3 10x1.0]][[
33. pH and pOH
Because hydronium ion concentrations for most solutions
are numbers with negative exponents, we express these
concentrations as pH:
pH = -log [H3O+
]
Acidic solution:Acidic solution: pH < 7.0.
Basic solution:Basic solution: pH > 7.0.
Neutral solution:Neutral solution: pH = 7.0.
34.
35. if we know the pH of an aqueous solution, we can easily
calculate its pOH:
pOH = -log[OH-
]
the ion product of water, Kw, is 1.0 x 10-14
taking the logarithm of this equation gives:
pH + pOH = 14
36.
37. 1. acidic.
2. basic.
3. neutral.
4. radioactive.
If a solution has a [OH-
] of 4.87 x 10-9
M, then the
solution is classified as:
38. Acid-Base Titrations
AAnalytical procedure in which a solution of known concentration reacts
in a known stoichiometry with a substance whose concentration is to be
determined.
HI + KOH → H2O + K+
+ I-
M = ? 0.138 M.
19.4 mL 39.2 mL
M0.279
Liters0.0194
mole5.41x10
MolarityHI
HofmolesOHofmolesKOHofmoles
KOHofmole.41x105
ml1000
liter1
x39.2mLx
liter
moles
138.0
3
3
==
==
=
−
−
39. pH Buffers
A pH buffer solution resists change in pH
when limited amounts of acid or base are
added to it.
Buffers consist of approximately equal molar
amounts of a weak acid and a salt of the
conjugate base.
40. CH3
–COOH H+
+ CH3-COO-
CH3
-COONa → Na+
+ CH3-COO-
BUFFER SYSTEM
http://www.mhhe.com/physsci/chemistry/essentialchemistry/flash/buffer12.swf
Weak acid
Salt of the conjugate base
41. Blood Buffers
The average pH of human blood is 7.4 any change greater
than 0.10 pH unit in either direction can cause illness.
To maintain this pH, the body uses three buffer systems:
carbonate buffer:carbonate buffer: H2CO3 and its conjugate base, HCO3
-
phosphate buffer:phosphate buffer: H2PO4
-
and its conjugate base, HPO4
2-
proteins:proteins: discussed in Chapter 21.
43. pH = pKa
+ log
[CO3
2-
]
= - log (4.8e-11) + log
0.310
= 10.16
[HCO3
-
] 0.443
Substituting these values in the equation gives:
A buffer solution is 0.443 M in KHCO3 and 0.310 M in K2CO3.
If Ka for HCO3
-
is 4.8e-11
, what is the pH of this buffer
solution?