Given below are half cell reactions:

$$MnO_4^ - + 8{H^ + } + 5{e^ - } \to M{n^{2 + }} + 4{H_2}O$$,

$$E_{M{n^{2 + }}/MnO_4^ - }^o = - 1.510\,V$$

$${1 \over 2}{O_2} + 2{H^ + } + 2{e^ - } \to {H_2}O$$

$$E_{{O_2}/{H_2}O}^o = + 1.223\,V$$

Will the permanganate ion, $$MnO_4^ - $$ liberate O₂ from water in the presence of an acid?

What mass of 95% pure CaCO₃ will be required to neutralise 50 mL of 0.5 M HCl solution according to the following reaction?

CaCO_3(s) + 2HCl_(aq) $$\to$$ CaCl_2(aq) + Co_2(g) + 2H₂O_(l)

[Calculate upto second place of decimal point]

The pH of the solution containing 50 mL each of 0.10 M sodium acetate and 0.01 M acetic acid is [Given pK_a of CH₃COOH = 4.57]

Match List-I with List-II.

Choose the correct answer from the options given below