25 mL of 0.2 M NaOH solution will neutralize 10 mL of 0.5 M HCl solution.

Question

Quizplus · Accepted Answer

This is a stoichiometry problem involving acid-base neutralization. The balanced chemical equation for the reaction is:

NaOH + HCl -> NaCl + H2O

From the equation, we can see that 1 mole of NaOH reacts with 1 mole of HCl to produce 1 mole of NaCl and 1 mole of water. Therefore, the number of moles of HCl in 10 mL of 0.5 M HCl solution is:

moles of HCl = volume (in L) x molarity = 0.01 L x 0.5 mol/L = 0.005 mol

To neutralize this amount of HCl, we need an equal number of moles of NaOH. The amount of NaOH required can be calculated using the equation:

moles of NaOH = moles of HCl

Since the concentration of NaOH solution is given as 0.2 M, the number of moles of NaOH in 25 mL of solution is:

moles of NaOH = volume (in L) x molarity = 0.025 L x 0.2 mol/L = 0.005 mol

This is the same as the number of moles of HCl, so the NaOH solution is sufficient to neutralize the HCl solution. Therefore, the statement is true and the answer is A.

25 ML of 0