Question

Calculate the number of liters of 0.500 M H2SO4 (aq) that are needed to neutralize 1.63 g of NaOH. Clear steps please

Answer 1

This is a stoichiometry problem, where we need to convert from 1.63g of NaOH to liters of 0.500 M H₂SO₄.

1st step: Finding and balancing the chemical equation:

This is an acid-base reaction, where the base (NaOH) reacts with the acid (H₂SO₄₎ to form water an a salt:

NaOH + H₂SO₄ ----> H₂O + Na₂SO₄

Balancing the equation:

2NaOH + H₂SO₄ ----> 2H₂O + Na₂SO₄

2nd step: using the molar mass of NaOH (40g/mol), convert from grams of NaOH to moles of NaOH

3rd step: using the balanced equation, convert from moles of NaOH to moles of H₂SO₄ (from the balanced equation, 1 mol of H₂SO₄ reacts with 2 moles of NaOH)

4th step: Using the concentration of H₂SO₄ (0.5M = 0.5 mol/L), convert from moles to liters

Now let's setup the numbers:

We start with 1.63g of NaOH, divide by 40.00g, divide by 2, and finally divide by 0,5:

	1st: Molar mass of NaOH:	Stoichiometry	Concentration of H2SO4	Answer:
1.63 g NaOH	1 mol NaOH	1 mol H2SO4	1 L H2SO4 solution	0.041 L H2SO4
	40.00 g NaOH	2 mol NaOH	0.500 mol H2SO4

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