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

Answer 1

Approx....#2*g#

You have already given the stoichiometric equation...

#underbrace(2NaOH(aq)+H_2SO_4(aq))_(80*g+98*g) rarr underbrace(Na_2SO_4(aq) + 2H_2O(l))_(178*g)#

Both mass and charge are BALANCED ABSOLUTELY, as indeed they must be if we purport to represent a chemical reaction.

And so #n_"sulfuric acid"=(2.8*g)/(98.08*g*mol^-1)=0.0286*mol#.

And we require TWO equiv of sodium hydroxide....i.e. a mass of...

#2xx0.0286*molxx40.0*g*mol^-1=??*g#
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Answer 2

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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Answer from HIX Tutor

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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