Question

1. hcn

section ii: formulas for binary acids and oxyacids
correctly write the chemical formula for the following acids following the rules for binary acids and oxyacids.

1. phosphoric acid
2. hydrobromic acid
3. sulfurous acid
4. perchloric acid
5. hydrofluoric acid
6. acetic acid
7. iodic acid
8. hydrosulfuric acid

Explanation:

To solve for the chemical formulas of these acids, we use the rules for binary acids (composed of hydrogen and a non - metal) and oxyacids (composed of hydrogen, oxygen, and another element):

9. Phosphoric acid

Phosphoric acid is an oxyacid. The polyatomic ion here is the phosphate ion, \(\ce{PO_4^{3 - }}\). Since hydrogen has a \(+ 1\) charge and the phosphate ion has a \(-3\) charge, to balance the charges, we need 3 hydrogen ions for 1 phosphate ion. So the formula is \(\ce{H_3PO_4}\).

10. Hydrobromic acid

Hydrobromic acid is a binary acid. Binary acids have the form \(\ce{HX}\), where \(X\) is the non - metal. For hydrobromic acid, the non - metal is bromine (Br). So the formula is \(\ce{HBr}\).

11. Sulfurous acid

Sulfurous acid is an oxyacid. The polyatomic ion is the sulfite ion, \(\ce{SO_3^{2 - }}\). Hydrogen has a \(+ 1\) charge. To balance the \(-2\) charge of the sulfite ion, we need 2 hydrogen ions. So the formula is \(\ce{H_2SO_3}\).

12. Perchloric acid

Perchloric acid is an oxyacid. The polyatomic ion is the perchlorate ion, \(\ce{ClO_4^{-}}\). Hydrogen has a \(+ 1\) charge. So we need 1 hydrogen ion to balance the \(-1\) charge of the perchlorate ion. The formula is \(\ce{HClO_4}\).

13. Hydrofluoric acid

Hydrofluoric acid is a binary acid. Using the binary acid formula \(\ce{HX}\), where \(X\) is fluorine (F), the formula is \(\ce{HF}\).

14. Acetic acid

The formula for acetic acid is a well - known one, which is \(\ce{CH_3COOH}\) (or \(\ce{C_2H_4O_2}\)).

15. Iodic acid

Iodic acid is an oxyacid. The polyatomic ion is the iodate ion, \(\ce{IO_3^{-}}\). Hydrogen has a \(+ 1\) charge, so we need 1 hydrogen ion to balance the \(-1\) charge of the iodate ion. The formula is \(\ce{HIO_3}\).

16. Hydrosulfuric acid

Hydrosulfuric acid is a binary acid. The non - metal is sulfur (S). Using the binary acid formula \(\ce{HX}\) (in this case, since sulfur has a \(-2\) charge, we need 2 hydrogen ions to balance it), the formula is \(\ce{H_2S}\).

Answer:

s:

1. \(\boldsymbol{\ce{H_3PO_4}}\)
2. \(\boldsymbol{\ce{HBr}}\)
3. \(\boldsymbol{\ce{H_2SO_3}}\)
4. \(\boldsymbol{\ce{HClO_4}}\)
5. \(\boldsymbol{\ce{HF}}\)
6. \(\boldsymbol{\ce{CH_3COOH}}\) (or \(\boldsymbol{\ce{C_2H_4O_2}}\))
7. \(\boldsymbol{\ce{HIO_3}}\)
8. \(\boldsymbol{\ce{H_2S}}\)