Question

What is the molarity of Na⁺ ion in a solution prepared by dissolving 0.550 gram of Na₂So₄ in a volume of 100ml of water?

Answer 1

Answer:

Explanation:

.142

Answer 2

Answer:

The molarity of Na⁺ ion in a solution in which 0.550g of Na₂SO₄ is dissolved in a volume of 100ml of water is equal to 0.077M.

Explanation:

We have given, the mass of Na₂SO₄ = $0.550g$

Given, the volume of water (H₂O) = 100ml = 0.1 L

The chemical reaction:-

Na₂SO₄  $\longrightarrow$  2Na⁺  +   SO₄²⁻

The molar mass of Na₂SO₄ = 142g/mol

Number of moles of Na₂SO₄ $= 0.550/142$ = 0.0039 moles

From the balanced chemical equation we can say that, number of moles  Na⁺ ions twice the number of moles of Na₂SO₄.

Therefore, number of moles sodium ions = 2× 0.0039 = 0.0077 moles

Molarity of sodium ion solution,

Molarity $=\frac{0.0077}{0.1} =0.077M$

Therefore, the molarity of sodium ions in the given solution is equal to $0.077M$.

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