The reaction of HCl with NaOH is represented by the equation HCl(aq) + NaOH(aq) → NaCl(aq) + H₂O(l)
What volume of 0.614 M HCl is required to titrate 18.8 mL of 0.619 M NaOH?

Question

The reaction of HCl with NaOH is represented by the equation HCl(aq)+ NaOH(aq)→ NaCl(aq)+ H₂O(l) What volume of 0.614 M HCl is required to titrate 18.8 mL of 0.619 M NaOH?

Quizplus · Accepted Answer

First, we need to use stoichiometry to find the amount of HCl needed to neutralize the NaOH. From the balanced equation, we can see that 1 mole of HCl reacts with 1 mole of NaOH to produce 1 mole of NaCl and 1 mole of water:

HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l)

We can use the following formula to calculate the moles of NaOH that were used:

moles NaOH = Molarity × Volume (in liters)
          = 0.619 M × 0.0188 L
          = 0.01163 mol

Since the reaction is 1:1, we know that the moles of HCl required is also 0.01163 mol.

Now we can use the molarity and the moles of HCl to calculate the volume needed:

moles HCl = Molarity × Volume (in liters)
Volume (in liters) = moles HCl ÷ Molarity
Volume (in liters) = 0.01163 mol ÷ 0.614 M
Volume (in liters) = 0.01894 L = 19.0 mL

Therefore, the correct answer is C) 19.0 mL.

The Reaction of HCl with NaOH Is Represented by the Equation