Problem page aqueous hydrobromic acid will react with solid sodium hydroxide to produce aqueous sodium bromide and liquid water . suppose 80. g of hydrobromic acid is mixed with 55.0 g of sodium hydroxide. calculate the minimum mass of hydrobromic acid that could be left over by the chemical reaction. be sure your answer has the correct number of significant digits.

To produce 0.9888 moles of NaBr and 0.9888 moles of H2O, there will remain 0.3862 moles of NaOH. All the HBr will be consumed, no HBr will be left over by the chemical reaction

Explanation:

Step 1: Data given

Mass of hydrobromic acid = 80.00 grams

Mass of sodium hydroxide = 55.00 grams

Molar mass HBr = 80.91 g/mol

Molar mass NaOH = 40 g/mol

Step 2: The balanced equation

HBr(aq) + NaOH(s) → NaBr(aq) + H₂O(l)

Step 3: Calculate moles of HBr

Moles HBr = Mass HBr / molar mass HBr

Moles HBr = 80.00 grams / 80.91 g/mol

Moles HBr = 0.9888 moles

Step 4: Calculate moles NaOH

Moles NaOH = 55.00 grams / 40.00 g/mol

Moles NaOH = 1.375 moles

Step 5: Calculate limiting reactant

For 1 mol of HBr we need 1 mol of NaOH to produce 1 mol of NaBr and 1 mol of H2O

The limiting reactant is HBr. It will completely be consumed. (0.9888 moles). NaOH is in excess. There will react 0.9888 moles. There will remain 1.375 - 0.9888 = 0.3862 moles

This means to produce 0.9888 moles of NaBr and 0.9888 moles of H2O, there will remain 0.3862 moles of NaOH. All the HBr will be consumed, no HBr will be left over by the chemical reaction

a. a primary source combines several different accounts of an event. b. a primary source generally benefits from having been written after an event.

explanation: