Aqueous sulfuric acid h2so4 will react with solid sodium hydroxide naoh to produce aqueous sodium sulfate na2so4 and liquid water h2o . suppose 89.3 g of sulfuric acid is mixed with 96. g of sodium hydroxide. calculate the minimum mass of sulfuric acid that could be left over by the chemical reaction. be sure your answer has the correct number of significant digits.

will be left.

Explanation:

Given:

Aqueous sulfuric acid will react with solid sodium hydroxide NaOH to produce aqueous sodium sulfate and liquid water .

Now, balance the molecules of the left part of the equation with the right part of the equation.  

Now, from the above-balanced equation, it is clear that  1-mole sulphuric acid equated with two moles of sodium hydroxide to balance the above equation.

Now,

The weight of sulphuric acid is 89.3 g and the weight of sodium hydroxide is 96 g.

Therefore, convert 89.3 g of and 96.0 g of into moles by using the formula,

Known Quantity:

Hence,

Therefore,

If 0.91 moles react of then the number of moles required of for the reaction will be twice as 0.91 moles.  

Moles required of is 1.82.

Thus,

The remaining moles of NaOH will be (2.40 - 1.82) that is 0.58.

Now,

The weight of 0.580 moles NaOH will be calculated by the below expression:

For more information, please refer to the link:

link