Sulfamic Acid Titration

Introduction ? Neutralization reactions involve the reaction of an acid and a tie-up to produce a salt (ionic compound) and water. block + travelling bag ( Salt + water supply ? In this lab, sulfamic acid (a weak acid which contains one acidic hydrogen) go out be used H2NSO2OH(aq) + NaOH(aq) ( NaOSO2NH2(aq) + H2O(l) (Net Equation H+(aq) + OH-(aq) ( H2O(l)) ? Titration is a process of neutralisation reaction Titration is commonly used to determine the assimilation of an acid or asc demolitionant 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 pith being analyzed is just consumed.The moles of H+ = moles of OH- at this point (called the par point). ? Information about the analyte (i. e. mass) can be calculated at the equating point. The volume of titrant is recorded and the moles of titrant can then be calculated exploitation n = C(V, where n = o f moles, C = concentration in mol/L and V = volume in L. ? The end point in a titration is frequently signaled by the color limiting of an indicator and occurs just roughly past the equivalence point. ? An indicator is a substance (weak acid) that has distinctively contrary 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. intemperate 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