Determine if each of the following compounds will create an acidic, basic or neutral solution.
a) Co(HSO₄)₂           b) Sr(HSO₃)₂

• A. a) acidic b) basic
• B. a) basic b) basic
• C. a) acidic b) acidic
• D. a) basic b) acidic

Answer: (A)

Verified step by step guidance

1. Identify the ions present in each compound. For Co(HSO4)2, the ions are Co^2+ and HSO4^-. For Sr(HSO3)2, the ions are Sr^2+ and HSO3^-.
2. Determine the nature of each ion. Co^2+ is a metal cation that does not affect pH significantly. HSO4^- is the hydrogen sulfate ion, which can donate a proton (H^+) and is therefore acidic. Sr^2+ is a metal cation that does not affect pH significantly. HSO3^- is the hydrogen sulfite ion, which can accept a proton and is therefore basic.
3. Analyze the effect of each ion on the solution's pH. In Co(HSO4)2, the presence of HSO4^- suggests the solution will be acidic. In Sr(HSO3)2, the presence of HSO3^- suggests the solution will be basic.
4. Consider the overall effect of the ions in each compound. Since HSO4^- is acidic, Co(HSO4)2 will create an acidic solution. Since HSO3^- is basic, Sr(HSO3)2 will create a basic solution.
5. Conclude the nature of the solutions: Co(HSO4)2 will create an acidic solution, and Sr(HSO3)2 will create a basic solution.