The 0.03 moles of sodium bicarbonate are needed to neutralize 0.8ml of sulfuric acid at STP.
Calculation,
Let's consider 0.8ml = 100% pure
Density of 100% pure sulfuric acid = mass/volume = 1.839 g/ml
Mass of 0.8ml sulfuric acid = 1.839 g/ml × 0.8ml = 1.47 g
Moles of sulfuric acid = given mass/ molar mass = 1.47/98 = 0.015 moles
Chemical equation is written as,
[tex]2NaHCO_{3} + H_{2}SO_{4}[/tex]→[tex]Na_{2}SO_{4} +2H_{2}O+ 2CO_{2}[/tex]
The mole ratio is 2:1
it means two moles of sodium bicarbonate are needed to neutralize 1 mole of sulfuric acid.
So, 0.015 moles of sulfuric acid need 0.015 × 2 moles of sodium bicarbonate.
So, 0.03 moles of sodium bicarbonate are needed to neutralize 0.015 moles of sulfuric acid at STP.
What is neutralization reaction?
The reaction in which acid and base combine to form complete salt and water is called neutralization reaction.
Learn about neutralization reaction,
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