Question

What is the molarity of a NaOH solution if 15.0 mL is exactly neutralized

by 7.5 mL of a 0.02 M HC2H3O2 solution?
Show all work using titrations formula.

Answer 1

see below for explanation

Step-by-step explanation:

1. you need to set up and balance the equation

NaOH + HC2H3O2 --> NaC2H3O2 + H2O

2. Write the value they gave you underneath the equation to figure out what we are solving for, which is the molarity of NaOH

NaOH (Base) + HC2H3O2 (Acid)--> NaC2H3O2 + H2O

15.0 ml | 7.5ml

? M | 0.02M

3. Use the MaVa=MbVb ·
`(mol a)/(mol b)`

- This formula is saying the M of an acid times the volume of the acid = the M of the base times the volume of the base times the mol of the acid/ mol of the base ratio. ***You should always compute the volume in Liters.

- Convert your values (x is the molarity of the base, the unknown value) Our acid values are first because that is how the equation is set up

0.0075 · 0.02 = 0.0150 · x · 1/1

4. Simplify

0.00015 = 0.0150x

5. Solve

Molarity of the base = 0.01