A solution of H2SO4(aq)H2SO4(aq) with a molal concentration of 2.55 m2.55 m has a density of 1.151 g/mL.1.151 g/mL. What is the molar concentration of this solution?

Molar concentration = 2.35 M (Approx)

Explanation:

Given:

Density of solution = 1.151 g/ml

2.55 molal = 2.55 moles of solute/ kg

Find:

Molar concentration

Computation:

Molar mass of H2SO4 = 2(1.0079) + (32.066) + 4(15.999)

Molar mass of H2SO4 =  98.0778

Molar mass of H2SO4 = 98 g/mol (Approx)

Mass of solution = 2.55(98)g + 1000 g

Mass of solution = 1249.9 gm

Volume of solution = 1249.9 / 1.151 = 1086 ml

Volume of solution = 1.086 L

Molar concentration= 2.55 / 1.086

Molar concentration = 2.35 M (Approx)

[H₂SO₄] = 2.35M

Explanation:

Our solute is the sulfuric acid → H₂SO₄

To determine the molar concentration we need the volume of solution.

Mass of solute: moles . molar mass

2.55 mol . 98 g/ 1 mol = 249.9 grams

Mass of solvent: 1 kg (we know this, because data refers about molality, moles of solute in 1kg of solvent)

Mass of solution = solute + solvent → 1000 g + 249.9 g = 1249.9 g

We apply density: Density = Mass / volume

1.151 g/mL = 1249.9 g / mL

mL = 1249.9 g/ 1.151 g/mL = 1086 mL

Molarity → mol/L → 2.55 moles/1.086L = 2.35 M

since the atomic number is the number of protons in the nucleus, as we move to the left on the periodic table, the electrostatic pull between the nucleus and the valence electron shell decreases. as we move down a group (vertical column), the valence shell energy level gets further and further from the nucleus.