Question

# Show your work and explain how you would find out how many liters of 0.500 M...

Show your work and explain how you would find out how many liters of 0.500 M H3PO4 it would take to react with 8.00 L of 0.100 M NaOH.

Given molarity of H3PO4 is 0.5M, volume=? and NaOH Molarity=0.1 M and volume=8 L.

Now find the moles of NaOH=Molarity x volume=0.1 moles/Lx8 L=0.8 moles.

The balanced equation between H3PO4 and NaOH is

H3PO4+3NaOH------>Na3PO4+3H2O

Therefore mole ratio between H3PO4 and NaOH is 1:3.

So moles of H3PO4=1/3(moles of NaOH)=1/3(0.8 moles)=0.266 moles H3PO4.

Given Molarity of H3PO4=0.5 M, so volume=moles/Molarity

Volume=0.266 moles/0.5 moles/L=0.533 L

So volume of H3PO4 is 0.533 L.

(Or) We can find out in another way

First convert Molarity into normality.

So normality of H3PO4=Molarity X3(since it has 3H's)=0.5x3=1.5 N, and for NaOH Molarity=normality (since it has 1 OH )

Therefore for NaOH 0.1 N and 8 L volume

From dilution law, N1V1=N2V2

1.5 NxV1=0.1 Nx8 L

V1=0.8/1.5=0.533 L.

So volume of H3PO4 is 0.533 L.

#### Earn Coins

Coins can be redeemed for fabulous gifts.