To determine the final pH of the solution resulting from the reaction between hydrochloric acid (HCl) and sodium hydroxide (NaOH), we need to consider the neutralization reaction between the two.
The balanced equation for the neutralization reaction between HCl and NaOH is:
HCl + NaOH → NaCl + H2O
From the equation, we can see that 1 mole of HCl reacts with 1 mole of NaOH to produce 1 mole of water (H2O) and 1 mole of sodium chloride (NaCl).
To determine the amount of HCl and NaOH that reacts, we can use the concept of stoichiometry and calculate the limiting reactant.
First, let's calculate the number of moles of HCl and NaOH:
moles of HCl = volume (in liters) × concentration (in moles per liter) = 0.022 L × 0.50 mol/L = 0.011 mol
moles of NaOH = volume (in liters) × concentration (in moles per liter) = 0.112 L × 0.20 mol/L = 0.0224 mol
Based on the stoichiometry of the reaction, we can see that 1 mole of HCl reacts with 1 mole of NaOH. Therefore, the moles of HCl and NaOH are equal.
Since both the HCl and NaOH completely react, the moles of excess HCl and NaOH are zero. The resulting solution consists only of the products NaCl and H2O.
Now, let's calculate the concentration of the resulting NaCl solution:
volume of resulting NaCl solution = volume of NaOH solution = 0.112 L
concentration of NaCl = moles of NaCl / volume of resulting NaCl solution = 0.0224 mol / 0.112 L = 0.20 mol/L
Since the reaction produces a salt, NaCl, which is a strong electrolyte that dissociates completely in water, the resulting solution will be neutral. Therefore, the final pH of the solution will be 7.00.
So, the correct answer is 7.00.