Ask Question
14 July, 17:31

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.

+3
Answers (1)
  1. 14 July, 19:14
    0
    1) Balanced chemical equation

    H2SO4 + 2NaOH - - - > Na2 SO4 + 2H2O

    => 1 mol H2SO4 : 2 moles NaOH

    2) Convert 89.3 g of H2SO4 and 96.0 g of NaOH to moles

    Molar mass of H2SO4 = 98.1 g/mol

    Molar mass of NaOH = 40.0 g/mol

    moles = mass in grams / molar mass

    moles H2SO4 = 89.3 g / 98.1 g/mol = 0.910 mol

    moles NaOH = 96.0 g / 40.0 g/mol = 2.40 mol

    3) Theoretical molar ratio = 2 moles NaOH / 1 mol H2SO4

    So, all the 0.91 mol of H2SO4 will be consumed along with 1.820 (2*0.91) moles of NaOH, and 0.580 moles (2.40 - 1.82) of NaOH will be left over by the chemical reaction.

    4) Convert 0.580 moles NaOH to mass

    0.580 moles * 40.0 g/mol = 23.2 g of NaOH will be left over
Know the Answer?
Not Sure About the Answer?
Get an answer to your question ✅ “Aqueous sulfuric acid h2so4 will react with solid sodium hydroxide naoh to produce aqueous sodium sulfate na2so4 and liquid water h2o. ...” in 📙 Chemistry if there is no answer or all answers are wrong, use a search bar and try to find the answer among similar questions.
Search for Other Answers