What mass of sodium carbonate is required for complete reaction with 8.35 g of nitric acid to produce sodium nitrate, carbon dioxide, and water?
A) 28.1 g
B) 14.04 g
C) 4.96 g
D) 7.02 g
E) 400.0 g

Question

Quizplus · Accepted Answer

The balanced equation for the reaction is:

2HNO3 + Na2CO3 → 2NaNO3 + CO2 + H2O

From the equation, we can see that 2 moles of nitric acid react with 1 mole of sodium carbonate to produce 2 moles of sodium nitrate, 1 mole of carbon dioxide, and 1 mole of water.

First, we need to determine the number of moles of nitric acid:

n(HNO3) = m/M = 8.35 g / 63.01 g/mol = 0.132 moles

From the balanced equation, we can see that 1 mole of sodium carbonate reacts with 2 moles of nitric acid. Therefore, the number of moles of sodium carbonate required is:

n(Na2CO3) = 0.132 moles / 2 = 0.066 moles

Finally, we can calculate the mass of sodium carbonate required:

m(Na2CO3) = n(M) = 0.066 moles x 105.99 g/mol = 7.02 g

Therefore, the answer is D) 7.02 g.

What Mass of Sodium Carbonate Is Required for Complete Reaction