Which of the following is the correct chemical formula for the ionic compound formed between Au^{3+} and HSO_4^{-}?

• A. Au_2(HSO_4)_3
• B. AuHSO_4
• C. Au(HSO_4)_3
• D. Au_3(HSO_4)_2

Answer: (C)

Verified step by step guidance

1. Identify the charges of the ions involved: Au^{3+} has a charge of +3, and HSO_4^{-} has a charge of -1.
2. Determine the ratio of ions needed to balance the total positive and negative charges so that the compound is electrically neutral.
3. Since Au^{3+} has a +3 charge and HSO_4^{-} has a -1 charge, you need three HSO_4^{-} ions to balance one Au^{3+} ion.
4. Write the chemical formula by placing the Au ion first, followed by the HSO_4 ion with a subscript of 3 to indicate three of these ions: Au(HSO_4)_3.
5. Verify that the total positive charge (+3 from Au) equals the total negative charge (3 × -1 from HSO_4), confirming the compound is neutral.