Which of the following is the chemical formula for the conjugate base of perchloric acid (HClO_4)?

• A. ClO_4^+
• B. HClO_3
• C. ClO_3^-
• D. ClO_4^-

Answer: (D)

Verified step by step guidance

1. Identify the acid given in the problem: perchloric acid, which has the chemical formula \(\mathrm{HClO_4}\).
2. Recall that a conjugate base is formed when an acid donates a proton (\(\mathrm{H^+}\)). This means the conjugate base will have one less hydrogen ion than the acid.
3. Remove one proton (\(\mathrm{H^+}\)) from the acid formula \(\mathrm{HClO_4}\), which leaves the species \(\mathrm{ClO_4^-}\).
4. Recognize that the charge on the conjugate base increases by one negative charge because the proton removed was positively charged, so the conjugate base carries a negative charge.
5. Compare the options given and select the species that matches \(\mathrm{ClO_4^-}\), which is the conjugate base of perchloric acid.