Acid,Bases And Salt(s) (ScienCe)

! SHREE !

JAIN INTERNATIONAL SCHOOL

“SCIENCE “ Project

“ACID” “BASES”

&“SALT”

Acids & BasesAcids:

acids are sour tastingArrhenius acid: Any substance that, when dissolved

in water, increases the concentration of hydronium ion (H3O+)

Bronsted-Lowry acid: A proton donorLewis acid: An electron acceptor

Bases:bases are bitter tasting and slipperyArrhenius base: Any substance that, when dissolved

in water, increases the concentration of hydroxide ion (OH-)

Bronsted-Lowery base: A proton acceptorLewis acid: An electron donor

Lone Hydrogen ions do not exist by themselves in solution. H+ is always bound to a water molecule to form a hydronium ion

Brønsted-Lowry Theory of Acids & BasesConjugate Acid-Base Pairs

General Equation

Brønsted-Lowry Theory of Acids & Bases

Brønsted-Lowry Theory of Acids & Bases

Brønsted-Lowry Theory of Acids & Bases

Reversible reaction

Notice that water in both an Acid & a base = Amphoteric

ELECTROLYTESElectrolytes are species which conducts electricity when

dissolved in water. Acids, Bases, and Salts are all electrolytes.

Salts and strong Acids or Bases form Strong Electrolytes. Salt and strong acids (and bases) are fully dissociated therefore all of the ions present are available to conduct electricity.

HCl(s) + H2O H3O+ + Cl-

Weak Acids and Weak Bases for Weak Electrolytes. Weaks electrolytes are partially dissociated therefore not all species in solution are ions, some of the molecular form is present. Weak electrolytes have less ions avalible to conduct electricity.

NH3 + H2O NH4+ + OH-

Acids & Bases STRONG vs WEAK_ completely ionized _ partially ionized

_ strong electrolyte _ weak electrolyte

_ ionic/very polar bonds _ some covalent bonds

Strong Acids: Strong Bases:

HClO4 LiOH

H2SO4 NaOH

HI KOH

HBr Ca(OH)2

HCl Sr(OH)2

HNO3 Ba(OH)2

Acids & BasesOne ionizable proton:

HCl → H+ + Cl-Two ionizable protons:

H2SO4 → H+ + HSO4-

HSO4- → H+ + SO4

2-

Three ionizable protons:

H3PO4 → H+ + H2PO4–

H2PO4- → H+ + HPO4

2-

HPO42- → H+ + PO4

-3

Combined:H2SO4 → 2H+ + SO4

2-

Combined: H3PO4 → 3H+ + PO4

3-

Acids & BasesFor the following identify the acid and the base as strong or

weak .

a. Al(OH)3 + HCl

b. Ba(OH)2 + HC2H3O2

c. KOH + H2SO4

d. NH3 + H2O

Weak base Strong acid

Weak acid

Strong acid

Strong base

Strong base

Weak base Weak acid

Acids & BasesFor the following predict the product. To check your answer left click

on the mouse. Draw a mechanism detailing the proton movement.

a. Al(OH)3 + HCl

b. Ba(OH)2 + HC2H3O2

c. KOH + H2SO4

d. NH3 + H2O

3AlCl3 + 3 H2O

2Ba(C2 H3O2)2 + 2 H2O

2K2SO4 2 H2O

NH4+ + O H-

Acids & BasesFor the following Identify the conjugate acid and the conjugate base. The

conjugate refers to the acid or base produced in an acid/base reaction. The acid reactant produces its conjugate base (CB).

a. Al(OH)3 + 3 HCl AlCl3 + 3 H2O

b. Ba(OH)2 + 2 HC2H3O2 Ba(C2H3O2)2 + 2 H2O

c. 2 KOH + H2SO4 K2SO4 + 2 H2O

d. NH3 + H2O NH4+ + OH-

CB CA

CB CA

CB CA

CA CB

Conjugate Acid-Base Pairs

Conjugate Acid-Base Pairs

TITRATIONTitration of a strong acid with a strong base

ENDPOINT = POINT OF NEUTRALIZATION = EQUIVALENCE POINT

At the end point for the titration of a strong acid with a strong base, the moles of acid (H+) equals the moles of base (OH-) to produce the neutral species water (H2O). If the mole ratio in the balanced chemical equation is 1:1 then the following equation can be used.

MOLES OF ACID = MOLES OF BASE

nacid = nbase

Since M=n/V

MAVA = MBVB

TITRATIONMAVA = MBVB

1. Suppose 75.00 mL of hydrochloric acid was required to neutralize 22.50 mLof 0.52 M NaOH. What is the molarity of the acid?

HCl + NaOH H2O + NaCl

Ma Va = Mb Vb rearranges to Ma = Mb Vb / Va

so Ma = (0.52 M) (22.50 mL) / (75.00 mL)

= 0.16 M

Now you try:2. If 37.12 mL of 0.843 M HNO3 neutralized 40.50

mL of KOH, what is the molarity of the base?Mb = 0.773 mol/L

TITRATIONTitration of a strong acid with a strong base

ENDPOINT = POINT OF NEUTRALIZATION = EQUIVALENCE POINT

At the end point for the titration of a strong acid with a strong base, the moles of acid (H+) equals the moles of base (OH-) to produce the neutral species water (H2O). If the mole ratio in the balanced chemical equation is NOT 1:1 then you must rely on the mole relationship and handle the problem like any other stoichiometry problem.

MOLES OF ACID = MOLES OF BASE

nacid = nbase

TITRATION1. If 37.12 mL of 0.543 M LiOH neutralized

40.50 mL of H2SO4, what is the molarity of the acid?

2 LiOH + H2SO4 Li2SO4 + 2 H2O

First calculate the moles of base:0.03712 L LiOH (0.543 mol/1 L) = 0.0202 mol LiOHNext calculate the moles of acid:0.0202 mol LiOH (1 mol H2SO4 / 2 mol LiOH)=

0.0101 mol H2SO4

Last calculate the Molarity: Ma = n/V = 0.010 mol H2SO4 / 0.4050 L = 0.248

M

2. If 20.42 mL of Ba(OH)2 solution was used to titrate29.26 mL of 0.430 M HCl, what is the molarity of the barium hydroxide solution?

Mb = 0.308 mol/L

Molarity and Titration

Molarity and TitrationA student finds that 23.54 mL of a 0.122 M

NaOH solution is required to titrate a 30.00-mL sample of hydr acid solution. What is the molarity of the acid?

A student finds that 37.80 mL of a 0.4052 M NaHCO3 solution is required to titrate a 20.00-mL sample of sulfuric acid solution. What is the molarity of the acid?

The reaction equation is:H2SO4 + 2 NaHCO3 → Na2SO4 + 2 H2O + 2 CO2

WATER EQUILIBRIUM

WATER EQUILIBRIUMKw = [H+] [OH-] = 1.0 x 10-14

Equilibrium constant for water

Water or water solutions in which [H+] = [OH-] = 10-7 M are neutral solutions.

A solution in which [H+] > [OH-] is acidic

A solution in which [H+] < [OH-] is basic

A measure of the hydronium ion (PH)The scale for measuring the hydronium ion

concentration [H3O+] in any solution must be able to cover a large range. A logarithmic scale covers factors of 10. The “p” in pH stands for log.

A solution with a pH of 1 has [H3O+] of 0.1 mol/L or 10-1

A solution with a pH of 3 has [H3O+] of 0.001 mol/L or 10-3

A solution with a pH of 7 has [H3O+] of 0.0000001 mol/L or 10-7

pH = - log [H3O+]

The pH scaleThe pH scale ranges from 1 to 10-14

mol/L or from 1 to 14. pH = - log [H3O+]

1 2 3 4 5 6 7 8 9 10 11 12 13 14

acid neutral base

Manipulating pHAlgebraic manipulation of:

pH = - log [H3O+]

allows for:[H3O+] = 10-pH

If pH is a measure of the hydronium ion concentration then the same equations could be used to describe the hydroxide (base) concentration.

[OH-] = 10-pOH pOH = - log [OH-]

thus:pH + pOH = 14 ; the entire pH range!

Ankush KhatriSuyash Chopda

GauravNanwani

Ashish Agrawal

PRESEMTED BY

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