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Hints and Practice Calculations for the 1033 practical exam

# Hints and Practice Calculations for the 1033 practical exam...

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Page 1 Titration experiments are divided into two parts A. The standardization of a base with KHP B. Determination of the concentration of an unknown acid using the Standardized Base. The number of equivalents can be determined by using the following molarity formulas: 1. KHP(s) KHP KHP MM i m 2. NaOH(aq) 1000 B V B M j 3. HA(aq) 1000 A V A M i Part A Standardization of the Base I Using the Molarity Formula Eq of Acid = Eq of Base KHP KHP MM i m = 1000 B V B M j m KHP = mass of KHP (g) V B = volume of base (mL) to reach endpoint MM KHP = molar mass of KHP i = number of H + ion(s) M B = molarity of base j = number of OH ion(s) II. Using DA 1 mole NaOH 1 mole KHP m KHP g KHP 1 1000 mL ?? moles NaOH = 1 mole KHP 204.22 g KHP V B mL NaOH(aq) 1 L = 1 L NaOH(aq) Part B Determination of the molarity of an unknown acid I Using the Molarity Formula Eq of Acid = Eq of Base A A V M i = B B V M j Or A n A V A M = B n B V B M Where n A = j and n B = i II. Using DA moles HA j mole HA M B mole NaOH 1 L NaOH V B mL NaOH(aq) 1 1000 mL HA M A molesHA 1 L

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