In: Chemistry
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.
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