Acid base titration discussion

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Everything needed or explained is within the document I provided, if you need more information, just let me know. I will try to respond as quick as possible and if I do not, mainly because of my job, you can guess or assume the answer. Than you in advanceLab: Titration Objectives • Understand the titration process • Use titration in a laboratory process to determine the acidity level of a solution • Demonstrate proper laboratory titration techniques when working with acids and bases Introduction The acid/base titration process relies on the use of a known concentration of a base (or an acid) to determine the unknown concentration of an acid (or base). Titration is based upon the neutralization reaction that occurs between acids and bases. Neutralization occurs when the equivalence point of the titration has been achieved. To determine when the neutralization takes place, a chemical, known as a neutralization indicator, is added to the solution. The neutralization indicator changes color when the desired pH is achieved. The acid-base indicator changes color at the end point of the titration – the point at which the pH level of the solution is determined. At the equivalence point, the number of H+ ions donated by the acid is equivalent to the number of H+ ions accepted by the base. © KC Distance Learning You can also use the titration process to calculate the quantity of moles of acid in a solution. Use the following equation to perform the calculation: molesacid = a = reaction coefficient of the acid Mb = molarity of the basic solution a x Mb x Vb b Vb = volume of base used in titration – converted to Liters b = reaction coefficient of the base Balance the reaction in order to determine the reaction coefficients of the acid and base. Once balanced, calculate the number of moles of acid in the solution. In this experiment, you will accurately determine the concentration of a solution of sodium hydroxide (NaOH) using a 0.500-M potassium hydrogen phthalate (KHP) standard solution. Add the acid-base indicator phenolphthalein, in its (colorless) acidic form, to a precisely measured volume sample of KHP. Slowly add the base, NaOH, to the sample of KHP. Once all the KHP has reacted with the base, the first excess drop of NaOH will cause the indicator to convert to its basic (pink) form. Then you can calculate the exact concentration of the NaOH solution. © KC Distance Learning Pre-lab Questions 1. How does the end point of a titration differ from the equivalence point? 2. How does a base differ from an acid? 3. Describe the term molarity as it relates to an acid or base.