Stella is measuring the heat of neutralization when aqueous solutions of HCl and

Question

Stella is measuring the heat of neutralization when aqueous solutions of HCl and NaOH are combined in a coffee cup calorimeter. She combines 45.5 mL of aqueous 1.00 M HCl and 36.58 mL of aqueous 1.00 M NaOH in a coffee cup calorimeter (mass of the coffee cups + the stir bar = 48.67 g). What is the mass of the solution after mixing, in g, assuming the solution has the same density as pure water (d =1.00g/mL)? Express your answer to two digits after the decimal. Do not use units (i.e. g) in your answer.

Explanation / Answer

Moles of HCl = 0.0455 L x 1 M = 0.0455 moles

Moles of NaOH = 0.03658 x 1 M = 0.03658 moles

moles of NaCl formed = 0.03658 moles

Mass of NaCl left = 0.03658 moles x 58.5 g/mol = 2.257 g

Moles of water = 0.03658 moles

Mass of water = 0.694 g

Moles of HCl left = 0.0455 moles - 0.03858 moles = 0.00692 moles

mass of HCl left = 0.00692 moles x 36.5 g/mol = 0.25258 g

Total mass left = 0.25258 g + 2.257 g + 0.694 g = 3.20 g

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