Step 1 of 5) We determine whether a given chemical reaction is an oxidation–reduction reaction by keeping track of the oxidation numbers (oxidation states) of the elements involved in the reaction. (Section 4.4) This procedure identifies whether the oxidation number changes for any elements involved in the reaction. For example, consider the net reaction that occurs spontaneously when zinc metal is added to a strong acid (Figure 20.1):The oxidation numbers below the equation show that the oxidation number of Zn changes from 0 to +2, while that of H changes from +1 to 0. Thus, this is an oxidation– reduction reaction. Electrons are transferred from zinc atoms to hydrogen ions; Zn is oxidized and H+ is reduced. In a reaction such as Equation 20.2, a clear transfer of electrons occurs. In some reactions, however, the oxidation numbers change, but we cannot say that any substance literally gains or loses electrons. For example, in the combustion of hydrogen gas.
Assume that 30.0 mL of a 0.10 M solution of a weak base B that accepts one proton is titrated with a 0.10 M solution of the monoprotic strong acid HA.
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Problem 17.40
Assume that 30.0 mL of a 0.10 M solution of a weak base B that accepts one proton is titrated with a 0.10 M solution of the monoprotic strong acid HA. (a) How many moles of HA have been added at the equivalence point? (b) What is the predominant form of B at the equivalence point? (c) Is the pH 7, less than 7, or more than 7 at the equivalence point? (d) Which indicator, phenolphthalein or methyl red, is likely to be the better choice for this titration?
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Assume that 30.0 mL of a 0.10 M solution of a weak base B that accepts one proton is titrated with a 0.10 M solution of the monoprotic strong acid HA.