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