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What is the correct relationship between the pHs of isomolar solutions of sodium oxide (pH1), sodium sulphide (pH2), sodium selenide (pH3) and sodium telluride (pH4) ?

  1. A
    pH1 > pH2 ≈ pH3 > pH4
  2. B
    pH1 < pH2 < pH3 < pH4
  3. C
    pH1 < pH2 < pH3 ≈ pH4
  4. D
    pH1 > pH2 > pH3 > pH4

Solution & Step-by-step Explanation

The pH of a solution of a salt of a weak acid and a strong base depends on the strength of the weak acid. The weaker the acid, the higher the pH of its salt's solution. Among the given options, the anions are oxide (O2-), sulfide (S2-), selenide (Se2-), and telluride (Te2-). The acid strengths of their conjugate acids (H2O, H2S, H2Se, H2Te) increase in the order H2O < H2S < H2Se < H2Te, meaning the weakest acid is H2O and the strongest is H2Te. Therefore, the pH of the solutions of their sodium salts will be in the order pH1 > pH2 > pH3 > pH4, as the weakest acid (H2O) will have the highest pH and the strongest acid (H2Te) will have the lowest pH.

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What is the correct relationship between the pHs of isomolar solutions of sodium oxide (pH1), sodium sulphide (pH2), sodium selenide (pH3) and sodium telluride (pH4) ?
A
pH1 > pH2 ≈ pH3 > pH4
B
pH1 < pH2 < pH3 < pH4
C
pH1 < pH2 < pH3 ≈ pH4
D
pH1 > pH2 > pH3 > pH4

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