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.

see below for explanation

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 ·

- 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

the density(ratio between mass and volume as m/v) decreases from top to bottom in periodic table group as the size increases and nuclear charge decreases. but in periods density increases from left to right as atom size decreases and nuclear charge increases.

the temperature of the gas, in k, not celsius.