A15.00-ml sample of a naoh solution of unknown concentration requires 17.88 ml of a 0.1053 m h2so4 solution to reach the equivalence point in a titration. what is the concentration of the naoh solution?

Explanation:

1) Data:

Base: NaOH

Vb = 15.00 ml = 15.00 / 1,000 liter

Mb = ?

Acid: H₂SO₄

Va = 17.88 ml = 17.88 / 1,000 liter

Ma = 0.1053

2) Chemical reaction:

The titration is an acid-base (neutralization) reaction to yield a salt and water:

3) Balanced chemical equation:

Placing coefficient 2 in front of NaOH and H₂O balances the equation

4) Stoichiometric mole ratio:

The coefficients of the balanced chemical equation show that 1 mole of H₂SO₄ react with 2 moles of NaOH. Hence, the mole ratio is:

5) Calculations:

a) Molarity formula: M = n / V (in liter)

   ⇒ n = M × V

b) Nunber of moles of acid:

c) Number of moles of base, nb:

d) At equivalence point number of moles of acid = number of moles of base

The concentration of NaOH solution is 0.25 M

Explanation:

Molarity of a solution is defined as the number of moles of solute dissolved per Liter of the solution.

According to the neutralization law,

where,

= molarity of solution = 0.1053 M

= volume of solution = 17.88 ml

= molarity of solution = 0.46 M

= volume of solution = 15.0 ml

= valency of = 2

= valency of = 1

Therefore, the concentration of  NaOH solution is 0.25 M

*tilts head* sounds more like a statement

the right answer is c i just did the question.