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Nana76 [90]
3 years ago
9

What is the molarity of a NaOH solution if 28.2 mL of a 0.355 M H2SO4 solution is required to neutralize a 25.0-mL sample of the

NaOH solution?
Chemistry
1 answer:
Verdich [7]3 years ago
8 0

Answer:

[NaOH} = 0.4 M

Explanation:

In a reaction of neutralization, we determine the equivalence point of the titration. In this case, we have a strong base and a strong acid.

(H₂SO₄, is considered strong, but the first deprotonation is weak)

2NaOH  +  H₂SO₄  →  Na₂SO₄  + 2H₂O

As we have 2 protons in the acid, we need 2 OH⁻ from the base to form 2 molecules of water.

In the equivalence point we know mmoles of base = mmoles of acid

Let's finish the excersise with the formula

25 mL . M NaOH = 28.2 mL  .  0.355M

M NaOH = (28.2 mL  .  0.355M) / 25 mL → 0.400

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In order to be able to solve this problem, you will need to know the value of water's specific heat, which is listed as

c=4.18Jg∘C

Now, let's assume that you don't know the equation that allows you to plug in your values and find how much heat would be needed to heat that much water by that many degrees Celsius.

Take a look at the specific heat of water. As you know, a substance's specific heat tells you how much heat is needed in order to increase the temperature of 1 g of that substance by 1∘C.

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What if you wanted to increase the temperature of 1 g of water by 2∘C ?

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And there you have it. The equation that describes all this will thus be

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In your case, you will have

q=100.0g⋅4.18Jg∘C⋅(50.0−25.0)∘C

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