# Sulfamic Acid Titration

Introduction: ? Neutralization reactions involve the reaction of an acid and a base to produce a salt (ionic compound) and water. Acid + Base ( Salt + Water ? In this lab, sulfamic acid (a weak acid which contains one acidic hydrogen) will be used: H2NSO2OH(aq) + NaOH(aq) ( NaOSO2NH2(aq) + H2O(l) (Net Equation: H+(aq) + OH-(aq) ( H2O(l)) ? Titration is a process of neutralization Titration is commonly used to determine the concentration of an acid or base in a solution. ? This process involves a solution of known concentration (the titrant or standard solution) delivered from a buret into the unknown solution (analyte) until the substance being analyzed is just consumed.
The moles of H+ = moles of OH- at this point (called the equivalence point). ? Information about the analyte (i. e. mass) can be calculated at the equivalence point. The volume of titrant is recorded and the moles of titrant can then be calculated using n = C(V, where n = # of moles, C = concentration in mol/L and V = volume in L. ? The end point in a titration is often signaled by the color change of an indicator and occurs just slightly past the equivalence point. ? An indicator is a substance (weak acid) that has distinctively different colors in acidic and basic media. *Not all indicators change color at the same pH, so the choice of indicator for a particular titration depends on the strength of the acid and base.
An indicator is chosen whose end point range lies on the steep part of the titration curve. ? The progress of an acid-base titration is often monitored by plotting the pH of the solution being analyzed as a function of the amount of titrant added (called a titration curve). Types of Titrations: 1. Strong Acid / Strong Base pH at equivalence point = 7 2. Weak Acid / Strong Base pH at equivalence point >7 3. Strong Acid / Weak Base pH at equivalence point

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