A5.05% (by mass) of aqueaus solution of sodium sulfate
isallowed to react with an excess of barium chloride. what volume
ofthe sodium sulfate solution (density= 1.03g/ml) is required
toproduce 2.73 g of barium

Answer : The volume  of the sodium sulfate solution required is, 0.0319 L

Explanation :

As we are given that 5.05 % (by mass) of aqueous solution of sodium sulfate that means, 5.05 grams of sodium sulfate present in 100 grams of solution.

Mass of sodium sulfate = 5.05 g

Mass of solution = 100 g

Density of solution = 1.06 g/mL

First we have to calculate the volume of solution.

Now we have  to calculate the molarity of sodium sulfate solution.

Formula used :

Molar mass of sodium sulfate = 142.04 g/mol

Now put all the given values in this formula, we get:

Now we have to calculate the moles of barium sulfate.

Molar mass of barium sulfate = 233.38 g/mol

Now we have to calculate the moles of sodium sulfate.

The balanced chemical reaction will be:

From the balanced chemical reaction, we conclude that

As, 1 mole of produced from 1 mole of

So , 0.0117 mole of produced from 0.0117 mole of

Now we have to calculate the volume of sodium sulfate.

Thus, the volume  of the sodium sulfate solution required is, 0.0319 L

answer: find it ur self

explanation:

yes, water is wet, just as it makes other things wet, it is wet itself, kinda like ice, when ice is in water, the ice makes water cold, and ice is cold, therefore with that example, water is wet