How many grams of sodium hydroxide would be needed to completely neutralize 2.8g of sulfuric acid? 2NaOH+H2SO4- Na2SO4+ 2H2O The dash is an arrow
Approx....
You have already given the stoichiometric equation...
Both mass and charge are BALANCED ABSOLUTELY, as indeed they must be if we purport to represent a chemical reaction.
And we require TWO equiv of sodium hydroxide....i.e. a mass of...
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To completely neutralize 2.8 grams of sulfuric acid (H2SO4), you need an equal number of moles of sodium hydroxide (NaOH). The molar mass of sulfuric acid (H2SO4) is 98.08 g/mol. Using the balanced chemical equation:
2NaOH + H2SO4 → Na2SO4 + 2H2O
It shows that 1 mole of sulfuric acid (H2SO4) reacts with 2 moles of sodium hydroxide (NaOH). Therefore, to find the number of moles of sodium hydroxide needed, divide the mass of sulfuric acid by its molar mass, then multiply by 2:
( \text{Number of moles of } \text{H}_2\text{SO}_4 = \frac{2.8 \text{ g}}{98.08 \text{ g/mol}} = 0.0285 \text{ mol} )
Since the ratio between sulfuric acid and sodium hydroxide is 1:2, you'll need double the number of moles of sodium hydroxide:
( \text{Number of moles of } \text{NaOH} = 2 \times 0.0285 \text{ mol} = 0.057 \text{ mol} )
The molar mass of sodium hydroxide (NaOH) is 40.00 g/mol. To find the mass of sodium hydroxide needed, multiply the number of moles by its molar mass:
( \text{Mass of } \text{NaOH} = 0.057 \text{ mol} \times 40.00 \text{ g/mol} = 2.28 \text{ g} )
So, you would need 2.28 grams of sodium hydroxide to completely neutralize 2.8 grams of sulfuric acid.
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When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
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