given that 15.00cm3 of H2SO4 was required to completely neutralise 25.00cm3 of 0.125 mole per dm3 of NaOH. calculate the molar concentration of the acid solution
NaOH: .025L * 0.125M = 0.003125 moles
H2SO4 + 2NaOH = Na2SO4 + 2H2O
so, you will need half as many moles of H2SO4
H2SO4: 0.0015625 moles / 0.015L = 0.104 mole/L
or, 0.1M solution
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To calculate the molar concentration of the acid solution, we need to use the balanced chemical equation for the neutralization reaction between H2SO4 (sulfuric acid) and NaOH (sodium hydroxide):
H2SO4 + 2NaOH -> Na2SO4 + 2H2O
From the equation, we can see that one mole of H2SO4 react with two moles of NaOH.
Given:
- Volume of NaOH solution = 25.00 cm³ = 25.00/1000 dm³ = 0.025 dm³
- Molarity (molar concentration) of NaOH solution = 0.125 mol/dm³
We can use the volume of NaOH solution and its molarity to determine the number of moles of NaOH:
Number of moles = Volume × Molarity
Number of moles of NaOH = 0.025 dm³ × 0.125 mol/dm³
Number of moles of NaOH = 0.003125 mol
According to the balanced equation, the ratio between NaOH and H2SO4 is 2:1. So, the number of moles of H2SO4 must be half of the number of moles of NaOH:
Number of moles of H2SO4 = 0.003125 mol / 2
Number of moles of H2SO4 = 0.0015625 mol
Lastly, we need to calculate the molar concentration of the H2SO4 solution using the given volume:
Molarity (molar concentration) of the H2SO4 solution = Number of moles / Volume of solution
Molarity of the H2SO4 solution = 0.0015625 mol / 15.00 cm³
Molarity of the H2SO4 solution = 0.0015625 mol / (15.00/1000) dm³
Molarity of the H2SO4 solution ≈ 0.1042 mol/dm³
Therefore, the molar concentration of the acid solution is approximately 0.1042 mol/dm³.