Calculate the pOH of 0.055 M NH3 (Kb = 1.8 x 10-5); assume NH3 is not a strong base and does not 100% ionize into OH", t
Posted: Sat Jul 02, 2022 7:47 pm
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Calculate the pH of 0.44 M HF (K₂ = 6.8 x 10-4); assume HF does not 100% ionize into H3O+, therefore need the reaction of HF in H₂0 and ICE table 0.0173 12.24 0.36 1.76 3.17
A solution at 25 °C that contains 1 x 10-8 M H3O+ is which of the below based on its pH value? basic. acidic. neutral. neither acidic nor basic. both acidic and basic.
Select the correct statement concerning this reaction. CN (aq) + H₂O(1) HCN(aq) + OH¯ (aq) CN acts as a Brønsted base. H₂O acts as a Brønsted base. HCN is a conjugate base. OH is a conjugate acid. All of the above are correct statements.
Select the strong acid ionization reaction. HNO2(aq) + H₂O(1) NO₂ (aq) + H3O*(aq) HF(aq) + H₂O(1) ⇒ F(aq) + H3O+ (aq) HCN(aq) + H₂O(1) CN (aq) + H3O+ (aq) HNO3(aq) + H₂O(1)→ NO3(aq) + H3O*(aq) O HCIO(aq) + H₂O(1) CIO (aq) + H30¹(aq)