How many moles of Na2CO3 would be needed to react with 750 mL of 0.250 M H2SO4 solution?
3.00
To determine the number of moles of Na2CO3 needed to react with the H2SO4 solution, we can use the stoichiometry of the balanced chemical equation between Na2CO3 and H2SO4. The balanced chemical equation is:
Na2CO3 + H2SO4 → Na2SO4 + H2O + CO2
From the balanced equation, we can see that one mole of Na2CO3 reacts with one mole of H2SO4.
Step 1: Convert the given volume of H2SO4 solution to moles:
To do this, we need to use the following formula:
Moles = Concentration (in M) × Volume (in liters)
Given:
Concentration of H2SO4 solution = 0.250 M
Volume of H2SO4 solution = 750 mL = 0.750 L
Moles of H2SO4 = 0.250 M × 0.750 L = 0.1875 moles
Step 2: Determine the number of moles of Na2CO3 using stoichiometry:
From the balanced equation, we know that 1 mole of Na2CO3 reacts with 1 mole of H2SO4.
Moles of Na2CO3 = 0.1875 moles
Therefore, 0.1875 moles of Na2CO3 would be needed to react with 750 mL of 0.250 M H2SO4 solution.
To determine the number of moles of Na2CO3 needed to react with the H2SO4 solution, we can use the balanced chemical equation between Na2CO3 and H2SO4.
The balanced chemical equation between Na2CO3 and H2SO4 is:
Na2CO3 + H2SO4 -> Na2SO4 + H2O + CO2
From the balanced equation, we can see that the molar ratio between Na2CO3 and H2SO4 is 1:1. This means that one mole of Na2CO3 will react with one mole of H2SO4.
First, let's calculate the number of moles of H2SO4 in the given solution:
Moles of H2SO4 = Volume of solution (in liters) * Concentration of H2SO4
Given:
Volume of solution = 750 mL = 0.75 L
Concentration of H2SO4 = 0.250 M
Moles of H2SO4 = 0.75 L * 0.250 mol/L = 0.1875 mol
Since the molar ratio between Na2CO3 and H2SO4 is 1:1, we can conclude that we need 0.1875 moles of Na2CO3 to react with the given amount of H2SO4 solution (0.250 M, 750 mL).
Na2CO3 + H2SO4 ==> H2O + CO2 + Na2CO3
moles H2SO4 = M x L = ??
moles Na2CO3 = same as H2SO4. Look at the coefficients in the equation.