How much carbon dioxide has to be bubbled into aqueous sodium hydroxide to obtain a solution containing 3.5 mol of sodium hydrogen carbonate?
CO2 + NaOH ==> NaHCO3
You want 3.5 mol NaHCO3 so you must bubble 3.5 mol CO2 (and the question doesn't ask but you must also have at least 3.5 mol NaOH present)
To determine the amount of carbon dioxide needed to obtain a solution containing 3.5 mol of sodium hydrogen carbonate, we should first understand the balanced chemical equation for the reaction between carbon dioxide and sodium hydroxide.
The balanced chemical equation for the reaction is:
CO2 + 2 NaOH -> Na2CO3 + H2O
From the equation, we can see that one mole of carbon dioxide reacts with two moles of sodium hydroxide to produce one mole of sodium hydrogen carbonate.
So, if we want to obtain 3.5 moles of sodium hydrogen carbonate, we need to calculate the number of moles of carbon dioxide required by using the stoichiometry of the reaction.
Here's how to calculate it:
1. Start with the given amount of sodium hydrogen carbonate:
3.5 mol NaHCO3
2. Use the stoichiometry of the balanced equation to find the moles of carbon dioxide:
From the equation, we can see that 1 mole of carbon dioxide reacts with 1 mole of sodium hydrogen carbonate.
Therefore, the number of moles of carbon dioxide will be equal to the number of moles of sodium hydrogen carbonate.
Moles of CO2 = 3.5 mol NaHCO3
So, to obtain a solution containing 3.5 mol of sodium hydrogen carbonate, approximately 3.5 moles of carbon dioxide need to be bubbled into aqueous sodium hydroxide.