H2SO4 + Na2CO3 --> Na2SO4 + H2O + CO2 In a titration where H2SO4 is added from a buret to an aqueous solution of 0.850 g Na2CO3, 46.75 mL of H2SO4 are needed to reach the permanent endpoint of the titration.

A) Find the number of moles of Na2CO3 in the reaction.

B) Find the number of moles of H2SO4 in the reaction.

C) Find the mass/mass % of H2SO4 based on the above information about reaching the endpoint of the titration.

The molar mass of Na2CO3 is 105.99 g/mol. The molar mass of H2SO4 is 98.08 g/mol. The density of H2SO4 is 0.985 g/mL.

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Explanation:

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nacl or sodium chloride is an ionic compound. this is because an ionic compound pertains to a compound that consists of positively and negatively charged ions. in this case, na (sodium) has a tendency to lose one electron when it reacts with with other atoms, so the resulting sodium ion contains 11 protons and 10 electrons, thus making it positively charged (na+), when chlorine reacts, it usually gains one electron to form an ion called chloride, thus making it negatively charged ( since the ions are oppositely charged, they attract.