PRE-LABORATORY ASSIGNMENT: AN ACID-BASE TITRATION Name _________________________

Question

PRE-LABORATORY ASSIGNMENT: AN ACID-BASE TITRATION

Name ____________________________________

1. What is the stoichiometric ratio of NaOH to KHP using the equation below:

NaOH(aq) + KHC8H4O4(aq) KNaC8H4O4(aq) + H2O(l)

Base Acid (KHP) Salt   Water

______ Moles of NaOH = _______Moles of H2C2O4

2. If I use 0.025 moles of NaOH to neutralize the KHP,

how many moles of KHP are there?

3. Calculate the molar mass of KHC8H4O4 (KHP).

4. What is the Equivalence Point?

5. What indicator will be used in this experiment?

6. What color is the indicator in an acid solution?

7. If the initial buret reading is 0.50 ml and the final burette reading is at 30.50 mL, what is the volume of NaOH delivered?

Explanation / Answer

1. The stoichiometric ratio of NaOH to KHP is 1:1. This is clearly visible from the available chemical reaction. We first inspect the reaction and find that it is completely balanced for all elements present. Thus for the balanced reaction, one part of NaOH reacts with one part of KHP. Thus their molar requirement is equal.

2. The molar requirement is equal for both aid and base. Thus 0.025 mole NaOH will neutralise .025 moles of KHP.

3. Molar mass of KHP = (K*1)+(H*5)+(O*4)+(C*8) = (39*1)+(1*5)+(16*4)+(12*8) = 39+5+64+96 = 204.

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