6. Explain the action of carbon dioxide on following
solutions when
(a) carbon dioxide is passed in
limited amount
(b) carbon dioxide is passed in
excess amount.
(i) Sodium hydroxide solution
(ii) Limewater (calcium hydroxide
solution)
Answers
Answer:
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Answer:
(A) When the limited supply of Co2 is passed through lime water- it reacts and forms calcium carbonate which is insoluble in water and thereby the solution becomes turbid or forms a milky white precipitate.
(B) formation of water soluble calcium bicarbonate
When CO
2
is passed through lime water, it turns milky due to the formation of calcium carbonate which is sinsoluble in water.
limewater
Ca(OH)
2
+CO
2
⟶
milkiness
CaCO
3
+H
2
O
However, when excess of CO
2
is passed through this solution, the milkiness disappears. This is due to the formation of calcium bicarbonate which is colorless and soluble in water.
milkiness
CaCO
3
+H
2
O+
excess
CO
2
⟶
water soluble
Ca(HCO
3
)
2
(C) 2 NaOH (s) + CO2 (g) →Na2CO3 (aq) + H2O (l) This means that solid reagent grade sodium hydroxide is not pure enough to weigh and use directly. ... This reaction also takes place in the aqueous phase, where sodium hydroxide in solution reacts with CO2 from the air to form sodium carbonate.
(D) Carbon dioxide reacts with limewater (a solution of calcium hydroxide, Ca(OH) 2), to form a white precipitate (appears milky) of calcium carbonate, CaCO 3. Adding more carbon dioxide results in the precipitate dissolving to form a colourless solution of calcium hydrogencarbonate.