Question

how many moles of sodium bicarbonate are needed to neutralize 0.8 ml of sulfuric acid stop at least tell the ans​

Answer 1

Explanation:

Q- How many moles of sodium bicarbonate is needed to neutralize 0.8 ml of sulphuric acid?

Ans- To know this you would need to know the concentration of the sulfuric acid unless you really mean 0.8 mL of 100% pure sulfuric acid and, in this case, you would need to know the density. The density of 100% concentrated sulfuric acid can be looked up and is 1.8391 g/mL. So, with 0.8 mL you would have:

0.8 mL * 1.8391 g/mL = 1.471 g

Now, convert this to moles

1.471 g / 98 g/mol H2SO4 = 0.0150 moles

The neutralization reaction is

2NaHCO3 + H2SO4 → Na2SO4 + 2H2CO3

2H2CO3 → 2H2O + 2CO2

Overall, the reaction is

2NaHCO3 + H2SO4 → Na2SO4 + 2H2O + 2CO2

The stoichiometry says you need two moles of NaHCO3 for every mole of sulfuric acid. So, you will need

0.0150 mole H2SO4 * 2 NaHCO3/1H2SO4 = 0.03 mole NaHCO3

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