In a titration of 35.00 mL of 0.737 M H2SO4, mL of a 0.827 M KOH solution is required for neutralization. A) 35.0
B) 1.12
C) 25.8
D) 62.4
E) 39.3

In a titration of 35.00 mL of 0.737 M H₂SO₄, 62.4 mL of a 0.827 M KOH solution is required for neutralization.

Explanation:

The balanced reaction is

H₂SO₄  +  2 KOH  ⇒  2 H₂O  +  K₂SO₄

By stoichiometry of the reaction (that is, the relationship between the amount of reagents and products in a chemical reaction)  1 mole of H₂SO₄ is neutralized with 2 moles of KOH.

The molarity M being the number of moles of solute that are dissolved in a given volume, expressed as:

in units of

then the number of moles can be calculated as:

number of moles= molarity* volume

You have acid H₂SO₄

Then:

number of moles= 0.737 M* 0.035 L

number of moles= 0.0258

So you must neutralize 0.0258 moles of H₂SO₄. Now you can apply the following rule of three: if by stoichiometry 1 mole of H₂SO₄ are neutralized with 2 moles of KOH, 0.0258 moles of H₂SO₄ are neutralized with how many moles of KOH?

moles of KOH= 0.0516

Then 0.0516 moles of KOH are needed. So you know:

Replacing in the definition of molarity:

Solving:

volume=0.0624 L= 62.4 mL

In a titration of 35.00 mL of 0.737 M H₂SO₄, 62.4 mL of a 0.827 M KOH solution is required for neutralization.

explanation: it gains negative electrons, therefore becoming negatively charged. as charge cannot be created, nor destroyed, only transferred, this leaves the wool positive. now that they have opposite charges, the two items attract.

2b2t

explanation:

2b2t