1.What volume of 0.10M HCl should be needed to titrate .136 g Na2CO3 according t

Question

1.What volume of 0.10M HCl should be needed to titrate .136 g Na2CO3 according to the reaction equation: Na2CO3(aq) + 2HCl(aq) ? 2NaCl(aq) + H2O(l) + CO2(g)

2.Atmospheric carbon dioxide dissolves in raindrops resulting in a solution of carbonic acid that makes rain slightly acidic. Since carbonic acid is a diprotic acid, write the chemical equations that describe its stepwise ionization in water. Include physical states in your answer, e.g., start with H2CO3(aq). Use a double arrow in your answer.
The first step is:

The second step is:

Explanation / Answer

1- Na2CO3(aq) + 2HCl(aq) ----->2NaCl(aq) + H2O(l) + CO2(g)

moles of Na2CO3 = 0.136 /105.99=1.283x10^-3mole

mole of HCl=2x1.283x10^-3= 2.566x10^-3mole

volume of HCl = 2.566x10^-3/ 0.01= 0.2566l=256.6ml

2- The first step is: H2CO3(aq) + H2O(l) <==> HCO3-(aq) + H3O+ (aq)

The second step is: HCO3-(aq) + H2O(l) <==>CO3^-2(aq) + H3O+ (aq)

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