Sodium sulfate dissolves as follows: na2so4(s) → 2na+(aq) + so42- (aq). how many moles of na2so4 are required to make 1.0 l of solution in which the na concentration is 0.10 m?

The number of moles of is 0.05 moles.

Explanation:

To calculate the molarity of solution, we use the equation:

We are given:

Molarity of solution = 0.10 mol/L

Volume of solution = 1 L

Putting values in above equation, we get:

The chemical reaction for the ionization of sodium sulfate follows the equation:

By Stoichiometry of the reaction:

2 moles of sodium ions are produced by 1 mole of sodium sulfate

So, 0.10 moles of sodium ions will be produced by = of sodium sulfate.

Hence, the number of moles of is 0.05 moles.

Number of moles of are required to make 1.0 L of solution is 0.05 mole.

Explanation:

Given:

Na concentration=0.10 M.

To find

The number of moles of  which required to make 1.0 L of solution.

To find the mole value,using the molarity formula:

Molarity

As we have to find the moles of the solute but we know the molarity so,

Molarity of sodium is 0.10 M.

Therefore,

Simplified we get,

Moles of sodium is 0.10 M.

As we know that, 2 moles of sodium ions are formed by 1 mole of sodium sulfate

Divide the moles of sodium by 2,

Learn more about molarity, refer:

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