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 im 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 im = 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
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Unformatted text preview: 1 L HA(aq) = i moleNaOH 1 L NaOH(aq) 1000 mL NaOH V A mL HA(aq) 1 L HA = 1 L HA(aq) Page 2 Practice Problem Set: Part A: Standardization of a Base USE THE FOLLOWING DATA TO CALCULATE THE MOLARITY OF THE SODIUM HYDROXIDE SOLUTION. SHOW YOUR CALCULATIONS CLEARLY. THE MOLAR MASS OF KHP = 204.22 g/mol The following data represent the average from two best runs. Average Mass KHP (g) 0.7621 Initial Buret Reading (mL) 0.00 Final Buret Reading (mL) 14.95 Volume of NaOH used ____________ Average Molarity of NaOH ____________ Part B: Determination of the molarity of an Unknown Acid. The standard solution form Part A is used to determine the molarity of an unknown acid. A 15.00 mL sample of Unknown acid is titrated with the standard base where V i = 0.25 mL and V f = 30.15 mL, what is the concentration of the unknown acid if its structure is? 1. HA 2. H 2 A 3. H 3 A...
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This note was uploaded on 04/19/2011 for the course CHEM 1033 taught by Professor Price during the Fall '10 term at Temple.

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

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