what would the written chemical reaction be to this problem?
How many grams of hydrochloric acid should we use so we have exactly enough to react with 40g of sodium hydroxide? You'll need to write a chemical reaction, balance it, and then perform your calculation.
HCl + NaOH -> NaCl + H2O
each mole of NaOH reacts with one mole of HCl.
so, how many moles of NaOH in 40g?
How many grams of HCl in that many moles?
To determine the written chemical reaction and balance it, we first need to understand the chemical formula for hydrochloric acid and sodium hydroxide.
The chemical formula for hydrochloric acid is HCl, where H represents a hydrogen atom, and Cl represents a chlorine atom. The chemical formula for sodium hydroxide is NaOH, where Na represents a sodium atom, and OH represents a hydroxide ion.
The balanced chemical equation for the reaction between hydrochloric acid and sodium hydroxide is:
HCl + NaOH -> NaCl + H2O
According to this equation, one molecule of hydrochloric acid (HCl) reacts with one molecule of sodium hydroxide (NaOH) to produce one molecule of sodium chloride (NaCl) and one molecule of water (H2O).
To perform the calculation and determine the grams of hydrochloric acid required to react with 40g of sodium hydroxide, we need to use the concept of stoichiometry.
The molar mass of hydrochloric acid (HCl) is about 36.46 g/mol, and the molar mass of sodium hydroxide (NaOH) is about 40 g/mol.
To calculate the grams of hydrochloric acid required, we can set up a proportion using the molar ratio from the balanced equation:
(40 g NaOH) * (1 mol NaOH / 40 g NaOH) * (1 mol HCl / 1 mol NaOH) * (36.46 g HCl / 1 mol HCl) = x g HCl
By plugging in the values and simplifying the expression, we can find the grams of hydrochloric acid needed to react with 40g of sodium hydroxide.