Considering the reaction stoichiometry, 0.00495 grams of water is produced when 2.75×10⁻⁴ moles of NaOH reacts completely.
Sodium hydroxide (NaOH) and hydrochloric acid (HCl) react to form sodium chloride (NaCl) and water. So, the balanced reaction is:
NaOH + HCl → NaCl + H₂O
By reaction stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of moles of each compound participate in the reaction:
In the periodic table, you can find the molar mass of the elements, also called atomic mass or atomic weight. So, to calculate the molar mass of a compound, you must add the molar mass of the elements of the compound multiplied by the times they appear in the compound.
So, in the case of water:
H₂O= 2× 1 g/mole + 16 g/mole
H₂O= 18 g/mole
Then, if by stoichiometry of the reaction 1 mole of water is produced, the mass of water produced is calculated as:
mass H₂O= 1 mole× 18 g/mole
mass H₂O= 18 g
Then you can apply the following rule of three: if by stoichiometry 1 moles of NaOH produce 18 grams of H₂O, 2.75×10⁻⁴ moles of NaOH will produce how much mass of H₂O?
[tex]mass of H_{2} O=\frac{2.75x10^{-4} moles of NaOHx18 grams of H_{2} O}{1 mole of NaOH}[/tex]
mass of H₂O= 0.00495 grams
In summary, 0.00495 grams of water is produced when 2.75×10⁻⁴ moles of NaOH reacts completely.
Learn more about stoichiometry:
