Equilibrium(nb) 2 Flashcards
Relationship between equilibrium constant and gibs free energy
The value of K doesn’t depend upon the rate of reaction is directly proportional to the wiring of G.
Mathematical expression for thermodynamical view of equilibrium constant.
K= e^dG/RT
Optimum Conditions for Haber’s process
- Temperature= 750 K
- Pressure = 200 atm
- Catalyst = Fe
- Promoter = Mo
Electrolyte
Substances that contain electricity in their acquisitions and on as electrolytes. Example inorganic acids, bases, salts
Non electrolyte.
Substances that do not conduct electricity are known as non-electrolytes.
example glucose.
Strong electrolytes
Substances which should associate almost a completely into ions in aqua solutions are called good conductors of electricity.
Eg: - NaOH, HCl
Weak Electrolytes
Substances which are dissociated to a small extent in aqueous solution.
Eg: - CH3COOH
Dissociation
When an ionic compound is dissolved in water, the ions are already present in the solid compound or separates out.
Eg: - NaCl
Ionization
When a neutral molecule which does not contain ions then dissolves in water splits to produce ions in the solution.
Eg: - HCl ( Polar Covalent compound)
The extent to which ionization occurs depends on the
- Strength of the bond.
- Extent of solution of ions produced.
Ionic equilibrium
It is the equilibrium B/w the ions and the undissociated electrolyte.
But is an acid and base based on the classical concept?
Acids are substances that turn blue letters to red lightness and releases dihydrogen on reacting with some metal.
Eg: - HCl
Bases are substances that turn red litmus to blue, better taste to soup to touch.
Eg: - NaOH
What are acid and bases based on arhenius concept?
Acids are substances that dissociates in water to give hydration ions while bases are substances which dissociate in water to give hydroxide ions.
H plus ions are very reactive and cannot exist freely in acquisitions so it binds to oxygen atom of a solvent molecule to give trigonal hydronium ion.
What is an acid or base based on brownstedt lorry concept.
An acid is a substance which donates a hydrogen ion while a base is a substance of which accepts hydrogen ion.
Define conjugate acid base pair
The acid base pair that differs only by one proton is called conjugate acid base pair.
limitations of Brownstead Lowry’s concept
Substances like BF3 and AlCl3 do not have any hydrogen so it cannot give Proton but still act as acids.
What are acid and bases based on Lewis’s concept of acid and bases.
And acid is substantial which accepts a lone pair of electron while a base is a substance which can donate a lone pair of Electron.
What is the strong acid
Substances which almost completely dissociates into their constituencies in an aqueous solution.
What is a Strong Base?
substances which completely dissociate into ions in an aqueous medium giving hydroxyl ions.
pH scale
It is defined as the negative logarithm to the base 10 of the activity of hydrogen ion.
- at 25 degrees the pH of water is 7.
Ionization constants of weak acids and bases
Ka/b = C@^2/ 1-@
Relation between Ka and Kb
pKa + pKb = pKw
define polybasic acids
Assets having more than one ionizable proton per molecule are known as polybasic acids.
Why is Ka1>Ka2
It is more difficult to remove a positively charged proton from a negative charged ion due to electrostatic forces. Greater the charge on the negative ion, more difficult to remove the Proton hence it is less acidic.
Strength of HA bond
When the strength of HA bond decreases, the energy required to break the bond decreases so ha becomes a strong acid.
Polarity of HA bond
Then Ache bond becomes more polar, the ultra negativity difference between H and a atom increases. Bond breaks easily so strength of the acid is stronger.
define common ion effect.
If to the solution of weak electrolytes which ionizes to a small extent a strong electrolyte having a common ion is added which ionizes almost completely. The ionization of weak electrolyte is further suppressed this is known as common ion effect.
Buffer solutions
The solution which resist change in ph on dilution or with the addition of small amount of acid or alkali are called a buffer solutions.
Solubility product constant
Solubility product of an electrolyte at a specific temperature is defined as the product of the molar concentration of its ions in a saturated solution each concentration raised to the power equal to the number of ions produced on dissociation of one molecule of the electrolyte.
Application of solubility product
- In the calculation of solubility of aspiringly soluble salt.
- In predicting ionic or precipitation reactions.
- In the precipitation of soluble salt
- in qualitative analysis, the complete scheme of qualitative analysis is based on the concept of solubility product and common ion effect.
Difference between ionic product and solubility product
- Ionic product is applicable to all types of solutions May be saturated or unsaturated. Solubility product is applicable only to a saturated solution in which there is equilibrium between the undissolved salt and ions present in the solution.
- Solubility product of a salt at a constant temperature is constant whereas ionic product depends upon the concentration of ions in the solution.
