Mass Relationships in Chemical Reactions

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Emre Çobanoğlu IB1 HL C

Mass Relationships in Chemical Reactions

Aim

The aim of this experiment is to show that a reaction doesn’t have always 100% yield by reacting NaHCO3 and HCl and determining the amount of the products to calculate actual yield.

Introduction

A chemical reaction will be quantitative if one of the reactants is completely consumed. In this experiment sodium bicarbonate and hydrochloric acid start a reaction. The formula of this reaction is below.

NaHCO3 + HCl → NaCl + H2O + CO2

Observations

In this experiment, sodium bicarbonate is put in an evaporating dish and some amount of HCl is added in the dish and the reaction started. Bubbles are formed and CO2 gas is produced and the reaction started to make sound. There was also water vapor formed. White NaHCO3 started to turn into a colorless liquid after adding HCl. As the reaction takes place water is started to form. NaCl was dissolved in water, so salty water is heated to obtain NaCl. As the liquid is heated it turned into a yellowish color for a few seconds. Then it started bubbling and water vapor is formed.

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Raw Data:

Mass of Evaporating Dish + Lid: 62.14 +-0.1 g

Processed Data:

Trial #1

64.14 – 62.14 = 2 g NaHCO3

72.16 – 62.14 = 10.02 g NaCl + H2O

63.28 – 62.14 = 1.14 g NaCl

Trial # 2

65.14 – 62.14 = 3 g NaHCO3

72.95 – 62.14 = 10.81 g NaCl + H2O

63.91 – 62.14 = 2.07 g NaCl

Calculations

Na: 14.01 g/mol, H: 1.01 g/mol, Cl: 35.45 g/mol, O: 16 g/mol, C: 12.01 g/mol

NaCl= 49.46 g/mol

H2O= 18.02 g/mol

NaHCO3: 75.03 g/mol

Mole number of NaHCO3 = ...

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