Question

find the normality of 0.5 m H2SO4 solution​

Answer 1

Explanation

normality=molarity×n factor

n factor for h2so4 is 2

normality=0.5×2=1

Answer 2

Answer:

The normality of 0.5 m H₂SO₄ solution​ is 1.0N .

Explanation:

The standard definition of normality is that it is determined by the amount of solute (measured in grammes or moles) present in a solution per litre of solution.

The formula of normality is N = Molarity × Basicity .

The molarity of a substance refers to how much of it is present in a given volume of solution (M). Molarity is the measure of how many moles of a solute are present per litre of a solution. Molarity is also referred to as a solution's molar concentration.

The quantity of hydronium ions that a substance can create in an aqueous solution determines the basicity of an acid .

Basicity of $\mathrm{H}_2 \mathrm{SO}_4$ is $2$ as it given $2$ H⁺ ions .

The molarity of  $\mathrm{H}_2 \mathrm{SO}_4$ is $0.5$ .

Put the values in the normality formula

$Normality = 0.5 \times 2=1.0N$

Therefore the normality of 0.5 m $\mathrm{H}_2 \mathrm{SO}_4$ solution​ is 1.0N .

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