Write the balanced neutralization reaction that occurs between H 2 SO 4 and KOH in aqueous solution. Phases are optional. neutralization reaction: Suppose 0.650 L of 0.490 M H 2 SO 4 is mixed with 0.600 L of 0.280 M KOH . What concentration of sulfuric acid remains after neutralization? concentration:

0.19 M is the concentration of H₂SO₄ that remains after neutralization

Explanation:

In a neutralization reaction we produce water and a salt, formed by the cation and anion from the correspond base and correspond acid.

Acid: H₂SO₄

Base: KOH

We determine the reaction: H₂SO₄  +  2KOH →  K₂SO₄  +  2H₂O

1 mol of sulfuric reacts with 2 moles of hydroxide to produce 1 mol of sulfate and 2 moles of water.

We determine the moles of each reactant ( M . volume)

0.650L . 0.490mol/L = 0.32 moles of acid

0.600L . 0.280mol/L = 0.17 moles of base

In this question: "What concentration of sulfuric acid remains after neutralization" it is shown that the excess reactant is the H₂SO₄

We verify that, 2 moles of base can react with 1 mol of acid

So, 0.17 moles of base must react with (0.17 .1) / 2 = 0.085 moles

Moles of acid that remains, after the reaction is complete: 0.32 - 0.085 =

0.235 moles.

To determine the concentration, our total volume is (base vol + acid vol)

0.650L + 0.600L = 1.250L → M (mol/L) = 0.235 mol / 1.250L = 0.19 M

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