Assuming the density of a 5%acetic acid solution is
1.0g/ml, determine the volume of the aceticacid solution necessary
to neutralize 25.0ml of 0.10m naoh.

3.0 mL

Explanation:

Let's consider the neutralization between acetic acid and NaOH.

CH₃COOH + NaOH → CH₃COONa + H₂O

The moles of NaOH are:

25.0 × 10⁻³ L × 0.10 mol/L = 2.5 × 10⁻³ mol

The molar ratio of CH₃COOH to NaOH is 1:1. The moles of CH₃COOH are 2.5 × 10⁻³ mol.

The molar mass of CH₃COOH is 60.05 g/mol. The mass of CH₃COOH is:

2.5 × 10⁻³ mol × (60.05 g/mol) = 0.15 g

The mass percent of acetic acid is 5%. The mass of the solution of acetic acid is:

0.15 g CH₃COOH × (100 g solution/ 5 g CH₃COOH) = 3.0 g solution

The density of the acetic acid solution is 1.0 g/mL. The volume of the solution is:

3.0 g × (1 mL/1.0 g) = 3.0 mL

the electron configuration that you gave me has 16 electrons ergo it has 16 protons ergo it is the element sulfur.