Conjugate base for Bronsted acids H₂O and HF are _______.

If the solubility product of lead iodide is 3.2 × 10^-8, its solubility will be _______.

Pick out the incorrect statement regarding Lewis acids and bases

K_w represents _______.

pH of buffer depends upon concentration of _______.

The conjugate base of HCIO is ________.

Assertion: According to Bronsted concept. H₂O is an a neutral substance.
Reason: H₂O molecule can accept as well as donate a proton.
Codes:
a) (A) and (R) are true and (R) is the correct explanation of (A)
b) Both (A) and (R) are true but (R) does not explain (A)
c) (A) is true but (R) is false
d) Both (A) and (R) are false

Assertion: The dissociation of acetic acid decreases on addition of sodium acetate.
Reason: It is due to common ion effect.
Codes:
a) (A) and (R) are true and (R) is the correct explanation of (A)
b) Both (A) and (R) are true but (R) does not explain (A)
c) (A) is true but (R) is false
d) Both (A) and (R) are false

When aqueous ammonia is added to CuSO₄ solution, the solution turns deep blue due to the formation of tetra ammine copper (II) complex,\({ [Cu({ H }_{ 2 }O)_4] }_{ (aq) }^{ 2+ }+ 4{ NH }_{ 3 }(aq)\rightleftharpoons { [Cu{ ({ NH }_{ 3 }) }_{ 4 }] }_{ (aq) }^{ 2+ }\) among H₂O and NH₃ Which is stronger Lewis base.

Calculate the ionisation constant for the conjugate base of HF. Ionisation constant of HF at 298 K is 6.8 x 10^-4

Derive an expression for the hydrolysis constant and degree of hydrolysis of salt of strong acid and weak base.

For an aqueous solution of NH₄CI, prove that [H⁺] = \(\sqrt { { K }_{ n }.C } \)

K_sp of AgCl is \(1.8\times10^{-10}\). Calculate molar solubility in 1 M AgNO₃

Calculate the pH of solution with HO⁺ concentrations in mol dm^-3.
(i) 10^-4
(ii) 10^-7
(iii) 6.8 x 10^-3
(iv) 3.2 x 10^-5
(v) 0.035
(vi) 0.25
(vii) 5.4 x 10^-9
(viii) 7.1 x 10^-7

Derive the hydrolysis constant for the hydrolysis of salt of strong base and weak acid. Deduce its pH.