(a)Classify following oxides as neutral, acidic, basic or amphoteric:

CO,

(b)Write suitable chemical equations to show their nature.

(1) CO = Neutral

(2) ${B}_{2}{O}_{3}$ = Acidic
Being acidic, it reacts with bases to form salts. It reacts with NaOH to form sodium
metaborate.

${B}_{2}{O}_{3}+2NaOH\to 2NaB{O}_{2}+{H}_{2}O$

(3) $Si{O}_{2}$ = Acidic
Being acidic, it reacts with bases to form salts. It reacts with NaOH to form sodium silicate.

$Si{O}_{2}+2NaOH\to 2N{a}_{2}Si{O}_{3}+{H}_{2}O$

(4) $C{O}_{2}$ = Acidic
Being acidic, it reacts with bases to form salts. It reacts with NaOH to form sodium
carbonate.

$C{O}_{2}+2NaOH\to N{a}_{2}C{O}_{3}+{H}_{2}O$

(5) $A{I}_{2}{O}_{3}$ = Amphoteric
Amphoteric substances react with both acids and bases. Al2O3 reacts with both NaOH
and ${H}_{2}S{O}_{4}$.

$A{I}_{2}{O}_{3}+2NaOH\to NaAI{O}_{2}\phantom{\rule{0ex}{0ex}}A{I}_{2}{O}_{3}+3{H}_{2}S{O}_{4}\to A{I}_{2}{\left(SO}_{}$4)3+3H2O

(6) $Pb{O}_{2}$ = Amphoteric
Amphoteric substances react with both acids and bases. $Pb{O}_{2}$ reacts with both NaOH and
${H}_{2}S{O}_{4}$.

$Pb{O}_{2}+2NaOH\to N{a}_{2}Pb{O}_{3}+{H}_{2}O\phantom{\rule{0ex}{0ex}}2Pb{O}_{2}+2{H}_{2}S{O}_{4}\to 2PbS{O}_{4}+2{H}_{2}O+{O}_{2}$

(7) $T{I}_{2}{O}_{3}$ = Basic Being basic, it reacts with acids to form salts. It reacts with HCl to form thallium chloride.

$T{I}_{2}{O}_{3}+6HCI\to 2TIC{I}_{3}+3{H}_{2}O$