Standardization Data 1. Write a balanced molecular equation (with phases, of cou

Question

Standardization Data 1. Write a balanced molecular equation (with phases, of course) for the reaction between the KHP and the titrant: 2. Write the net ionic equation for this reaction (note that HC_ H_4 O_4 ^- is a weak acid). Be sure to include phases: 3 Calculate the for each trial. You must use dimensional analysis to get any credit - no other methods or short cuts will be accepted, so show all unit conversions Trial 1: ___ Trial 2: ____ Trial 3: Trial 3: ____ If one of the trials differs significantly from the others, consult your instructor. 4. Calculate the average molarity of the base: Average: ____ USE THIS AVERAGE MOLARITY OF THE BASE FOR THE DATA ANALYSIS ON PAGES 3 & 4 5. Using dimensional analysis, calculate how many mg of KHP would react with 20.15 mL of your base:

Explanation / Answer

1. Balanced equation for KHP with titrant

KHC8H4O4 + NaOH --> KNaC8H4O4 + H2O

2. Balanced ionic equation,

HC8H4O4- + OH- --> C8H4O4^2- + H2O

3. molarity of base (Trial 1)

= 0.4975 g/204.22 g/mol x 0.01166 L

= 0.21 M

molarity of base (Trial 2)

= 0.5025 g/204.22 g/mol x 0.01101 L

= 0.22 M

molarity of base (Trial 3)

= 0.4992 g/204.22 g/mol x 0.01177 L

= 0.21 M

4. Average molarity of base = 0.021 M

5. mg of KHP reacting = 0.021 M x 21.15 ml x 204.22 g/mol = 86.41 mg

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