Question

What volume of 0.0748 M perchloric acid can be neutralized with 115 mL of 0.244 M sodium hydroxide?

Answer 1

To find the volume of perchloric acid that can be neutralized with the given volume and concentration of sodium hydroxide, we need to use stoichiometry. The volume of 0.0748 M perchloric acid that can be neutralized is 375 mL.

Step-by-step explanation:

To find the volume of perchloric acid that can be neutralized by the sodium hydroxide, we need to use the concept of stoichiometry. The balanced equation for the reaction between perchloric acid (HClO4) and sodium hydroxide (NaOH) is:

HClO4(aq) + NaOH(aq) → NaClO4(aq) + H2O(l)

From the balanced equation, we can see that the ratio of HClO4 to NaOH is 1:1. This means that for every 1 mole of NaOH, 1 mole of HClO4 is required. We can use this information to calculate the volume of HClO4:

Number of moles of NaOH = concentration of NaOH x volume of NaOH

Number of moles of NaOH = 0.244 M x 0.115 L = 0.02806 moles of NaOH

Since the ratio of NaOH to HClO4 is 1:1, the number of moles of HClO4 required is also 0.02806 moles. To find the volume of HClO4, we can use the equation:

Volume of HClO4 = number of moles of HClO4 / concentration of HClO4

Volume of HClO4 = 0.02806 moles / 0.0748 M = 0.375 L = 375 mL

Answer 2

0.375 L

Step-by-step explanation:

We know that at neutralization, the number of mol of acid must equal the number of equivalents of base.

This is a reaction 1:1 acid to base:

HClO₄ + NaOH ⇒ NaClO₄ + H₂O

We re given the moles of the base indirectly since we know the volume and molarity. From there we can calculate the volume of HClO₄.

Moles NaOH = 0.115 L x 0.244 M = 0.115 L x 0.244 mol/L =0.028 mol

Thus we require 0.028 mol of HClO₄ in the pechloric acid solution:

Molarity = # moles / V ⇒ V = # moles / M

V = 0.028 mol / 0.0748 mol/L = 0.375 L

Note that this problem can be solved in just one step since

M(HClO₄) x V(HClO₄) = M(NaOH) x V(NaOH) ⇒

V(HClO₄) = M(NaOH) x V(NaOH) / M(HClO₄)