For a 1.0 M solution of H2S at equilibrium, which of the following statements are correct?...
For a 1.0 M solution of H2S at equilibrium, which of the following statements are correct? Ka: H2S = 9.1 x 10-8 HS- = 1.0 x 10-13 1. [H3O+] = [H2S] 2. [OH-] = 1.0 x 10-7 M 3. [HS-] = 9.1 x 10-8 M 4. [S2-] = 1.0 x 10-13 M
Homework Answers
The correct statement is : (4.) [S2-] = 1.0 x 10-13 M
Explanation
Aqueous H2S is weak acid. H2S does not dissociate completely which means hydronium ion concentration, [H3O+] cannot be equal to H2S concentration because only a small part of H2S is converted to H3O+
Since the solution is weakly acidic, therefore [H3O+] > 1.0 x 10-7 M. This means [OH-] < 1.0 x 10-7 M
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Explain the process of how to get the answer. The
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Ch. 18 Values The following values will be useful for problems in this chapter. Acid Substance or Species HF HNO2 CH3COOH HOCI HOBr HOCN HCN H2SO4 KA = 7.2 x 10-4 Ka = 4.5 x 10-4 Ka = 1.8 x 10-5 Ka = 3.5 x 10-8 = 2.5 x 10-9 K4 = 3.5 x 10-4 Ka = 4.0 x 10-10 Kai = very large Kq2 = 1.2...
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