Acids including formic acid and acetic acid is partly ionised from inside the solution and just have lowest K
2. Acids such as HCI, HNOstep three are almost completely? onised and hence they have high Ka value i.e., Ka for HCI at 25°C is 2 x 10 6 .
cuatro. Acids with Ka value greater than ten are considered as strong acids and less than one considered as weak acids.
- HClO4, HCI, H2SO4 – are strong acids
- NH2 – , O 2- , H – – are strong bases
- HNO2, HF, CH3COOH are weak acids
Question 5. pH of a neutral solution is equal to 7. Prove it. in neutral solutions, the concentration of [H3O + ] as well as [OH – ] are equal to 1 x 10 -7 M at 25°C.
2. The pH of a neutral solution can be calculated by substituting this [H3O + ] concentration in the expression pH = – log10 [H3O + ] = – log10 [1 x 10 -7 ] = – ( – 7)log \(\frac < 1>< 2>\) = + 7 (l) = 7
Answer: 1
Question 7. When the dilution increases by 100 times, the dissociation increases by 10 times. Justify this statement. Answer: (i). Let us consideran acid with Ka value 4 x 10 https://datingranking.net/escort-directory/mckinney/ 4 . We are calculating the degree of dissociation of that acid at two different concentration 1 x 10 -2 M and 1 x 10 -4 M using Ostwalds dilution law
(iv) i.elizabeth., if dilution increases by 100 moments (focus decrease from 1 x 10 -2 Yards to just one x 10 -4 Yards), the dissociation increases by the 10 times.
- Barrier is actually a simple solution using its a mixture of weak acidic and its conjugate foot (or) a deep failing foot and its own conjugate acid.
- This shield services resists radical alterations in the pH on inclusion out of a little quantities of acids (or) angles hence element is called shield action.
- Acidic buffer solution, Solution containing acetic acid and sodium acetate. Basic buffer solution, Solution containing NH4O and NH4Cl.
- The fresh buffering element regarding a simple solution are going to be measured when it comes away from buffer capabilities.
- Buffer list ?, while the a quantitative way of measuring the new buffer strength.
- It’s recognized as exactly how many gram equivalents away from acidic or legs placed into 1 litre of your own barrier substitute for changes the pH of the unity.
- ? = \(\frac < dB>< d(pH)>\). dB = number of gram equivalents of acid / base added to one litre of buffer solution. d(pH) = The change in the pH after the addition of acid / base.
Concern 10. How try solubility device is familiar with pick new precipitation out of ions? If the unit out-of molar intensity of the new constituent ions i.elizabeth., ionic device is higher than the solubility tool then your material becomes precipitated.
2. When the ionic Product > Ksp precipitation will occur and the solution is super saturated. ionic Product < Ksp no precipitation and the solution is unsaturated. ionic Product = Ksp equilibrium exist and the solution ?s saturated.
step three. Through this method, the fresh new solubility equipment discovers good for pick whether an ionic compound gets precipitated whenever services that contain brand new constituent ions was mixed.
Matter 11. Solubility will be calculated regarding molar solubility.i.age., the maximum quantity of moles of the solute which are often demolished in one litre of the solution.
3. From the above stoichiometrically balanced equation, it is clear that I mole of Xm Yn(s) dissociated to furnish ‘m’ moles of x and ‘n’ moles of Y. If’s’ is the molar solubility of Xm Ynthen Answer: [X n+ ] = ms and [Y m- ] = ns Ksp = [X n+ ] m [Y m- ] n Ksp = (ms) m (ns) n Ksp = (m) m (n) n (s) m+n