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How many milliliters of 0.200 m NH3 solution will exactly react with 18.0 ml of 0.130 m H2SO4 solution? 2nh3(aq) + H2SO4(aq) = (nh4)2so4(aq)
Accepted Answer
Here's how to solve this problem:
1. Balanced Equation: You've already provided the balanced equation, which is crucial for stoichiometry calculations:
2NH3(aq) + H2SO4(aq) → (NH4)2SO4(aq)
2. Moles of H2SO4: Calculate the moles of H2SO4 using the given molarity and volume:
Moles of H2SO4 = (0.130 mol/L)
(18.0 mL)
(1 L / 1000 mL) = 0.00234 mol
3. Moles of NH3: Use the stoichiometric ratio from the balanced equation to find the moles of NH3 needed to react completely with the H2SO4:
Moles of NH3 = (0.00234 mol H2SO4)
(2 mol NH3 / 1 mol H2SO4) = 0.00468 mol
4. Volume of NH3: Finally, calculate the volume of the 0.200 M NH3 solution needed:
Volume of NH3 = (0.00468 mol NH3) / (0.200 mol/L) = 0.0234 L
Convert to milliliters: 0.0234 L
(1000 mL / 1 L) = 23.4 mL
Therefore, 23.4 mL of 0.200 M NH3 solution will exactly react with 18.0 mL of 0.130 M H2SO4 solution.
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