Question

What volume (in mL) of a 0.150 MHNO3 solution is required to completely react with 39.6 mL of a 0.118 MNa2CO3 solution according to the following balanced chemical equation?

Na2CO3(aq)+2HNO3(aq)→2NaNO3(aq)+CO2(g)+H2O(l)

Express your answer with the appropriate units.

Answer 1

Explanation:

A mole ratio is ​the ratio between the amounts in moles of any two compounds involved in a chemical reaction. The mole ratio can be determined by examining the coefficients in front of formulas in a balanced chemical equation.

Step 1: write the balanced chemical equation.

Na₂CO₃(aq) + 2HNO₃ (aq) -----> 2Na(NO₃) (aq) + H₂O (l)

Step 2: calculate the moles of Na₂CO₃

we know, moles = molarity × volume(in L)

so, moles of Na₂CO₃ = 0.118 mol/L × ( 39.6 mL × 1 L/1000mL) = 0.0046728 mol

[note: 1L = 1000 mL and 1 M = mol/L ]

Step 3: Calculate the moles of HNO₃

Na₂CO₃(aq) + 2HNO₃ (aq) -----> 2Na(NO₃) (aq) + H₂O (l)

According to the reaction:
1 mol of Na₂CO₃ completely reacts with 2 mol of HNO₃

So, 0.0046728 mol of Na₂CO₃ will completely react with = (2 mol of HNO₃ / 1 mol of Na₂CO₃) × 0.0046728 mol of Na₂CO₃ = 0.0093456 mol of HNO₃

Step 4: Calculate the volume of HNO₃

We know, molarity = moles / volume

Given, Molarity = 0.150 M and we got moles = 0.0093456 mol

Hence, Volume = mole / molarity = 0.0093456 mol / 0.150 mol L^-1 = 0.062304 L

Required volume in mL = 0.062304 L × (1000 mL / 1L ) = 62.304 mL