IV. Provide the chemical Name of below acid or base. (a) Vinegar

(b) Fruits (orange)

(c) Curd

(d) Lime water

(e) Window cleaner

(f) Soap

V. When ‘X’ is added to ‘Y’ immediately ‘Y” turns to pink. Identify X.

VI. Give examples of a common acid and a common salt. Compare their composition. How do they differ and what do they have in common?

VII. Explain why pickles and jams should not be stored in metal containers.

VIII. Differentiate between weak acid and strong acid.

IX. Explain the reaction involved in the formation of sodium
chloride.

X. Why does a doctor give an antacid to treat indigestion?

A)Acetic acid

a)citric acid

b)lactic acid

c)citric acid

d)NH3

f)oxygen hidro-oxide

Explanation:

Limiting reactant  = O₂

Excess reactant = NO

Theoretical yield of NO₂ = 46 g

Mass of excess reactant = 30 g

Explanation:

O₂ + 2NO → 2NO₂

Mole ratio for the reaction is;

1 : 2 → 2

mass of O₂ = 16 g

mass of NO = 80 g

mass of NO₂ = 25 g

molecular weight  of O₂ = 32 g/mol

molecular weight  of NO = 30 g/mol

molecular weight  of NO₂ = 46 g/mol

molar mass of O₂ = mass ÷ molecular weight = 16 g ÷ 32 g/mol = 0.5 mol

molar mass of NO = mass ÷ molecular weight = 80 g ÷ 30 g/mol = 2.67 mol

Since, 1 mole of O₂ requires 2 moles of NO for the combustion reaction, 0.5 mole shall require 1 mole of NO for the reaction. Thus, O₂ is the limiting reactant and NO is the excess reactant as it has an excess of 2.67 mol - 1 mol = 1.67 mol.

1 mole of O₂ shall yield 2 moles of NO₂

Thus, 0.5 mole of O₂ shall yield 1 mole of NO₂

mass of NO₂ = molecular weight * molar mass = 46 g/mol * 1 mole = 46 g

1 mole of O₂ shall react with 2 moles of NO

Thus, 0.5 mole of O₂ shall yield 1 mole of NO

mass of NO = molecular weight * molar mass = 30 g/mol * 1 mole = 30 g