0.850 L of 0.490 M #H_2SO_4# is mixed with 0.800 L of 0.280 M #KOH#. What concentration of #H_2SO_4# remains after neutralization?
The concentration of
This is really a two-part question:
This is a volume-moles stoichiometry problem.
The steps are:
a. Write the balanced equation.
a. Write the balanced equation:
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To find the concentration of H₂SO₄ remaining after neutralization, calculate the moles of H₂SO₄ and KOH, then determine which reactant is limiting. The limiting reactant will be fully consumed, and the excess reactant will determine the concentration of the remaining acid. The balanced chemical equation for the reaction is:
H₂SO₄ + 2KOH → K₂SO₄ + 2H₂O
The moles of H₂SO₄ and KOH are: moles H₂SO₄ = (volume H₂SO₄) × (molarity H₂SO₄) moles KOH = (volume KOH) × (molarity KOH)
Next, determine the limiting reactant by comparing the moles of H₂SO₄ and KOH.
Once you find the limiting reactant, use stoichiometry to determine the moles of H₂SO₄ that reacted.
Finally, use the remaining volume of H₂SO₄ and the moles of H₂SO₄ remaining to calculate the concentration of H₂SO₄.
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When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
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