a. The number of moles of HX that is added at the equivalence point is 0.0003 moles.
b. The predominant form of B at the equivalence point is [tex]BH^{+}[/tex]
c. A factor which determines the pH at the equivalence point is the acid-base nature of the conjugate base and acid respectively.
d. Methyl red is likely to be the better choice for this titration because it would change color in the acid range.
Given the following data:
- Volume of weak base B = 30.0 mL.
- Molarity of weak base B = 0.10 M.
- Molarity of strong acid HX = 0.10 M.
What is an equivalence point?
An equivalence point can be defined as the point in a titration wherein the amount of reagent (titrant) added sufficiently neutralizes the analyte (titrand) solution. Thus, it is the amount of strong acid that is needed to neutralize a weak base completely
For this chemical reaction, the properly balanced chemical equation is written as follows:
[tex]B(aq)+HX(aq) \rightarrow BH^{+}(aq) + X^{-}(aq)[/tex]
By stoichiometry:
0.10 M solution = 0.10 moles of solute per liter of solution.
Note: 10,000 mL = 1 Liter.
[tex]Number\;of\;moles = \frac{30}{10000} \times 0.10\\\\Number\;of\;moles = 0.003 \times 0.10[/tex]
Number of moles = 0.0003 moles of HX.
b. The predominant form of B at the equivalence point is given by this equilibrium expression:
[tex]B(aq)+HX(aq)\rightleftharpoons BH^{+} + X^{-}[/tex]
Therefore, the predominant form of B at the equivalence point is [tex]BH^{+}[/tex]
c. A factor which determines the pH at the equivalence point is the acid-base nature of the conjugate base and acid respectively.
d. Methyl red is likely to be the better choice for this titration because it would change color in the acid range.
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