Question

Ir. contain howaining 5.0 m2 unlabeled to 5. You have two unlabeled test tubes, one containing 5.0 mL of 1.0 M HCl and the other containing 5.0 mL of 1.0 M of H2SO4. If you had only 6.0 mL of 1.0 M NaOH, describe how you could determine, without doubt, which test tube contained which acid? (You may use any equipment normally found in the lab.) withou. So pment

Answer 1

Acid + Base —> Salt + water

If the moles of acid(H+) and base(OH-) will be equal Complete neutralisation will occur.

If base (OH-) becomes more Solution will be basic.

If acid (H+) becomes more solution becomes acidic.

Milimoles of NaOH = 6.0 ml × 1.0M = 6 milimoles

Milimoles of HCl = 5.0 ml × 1.0M = 5 milimoles

Milimoles of H2SO4 = 5.0 ml × 1.0M = 5 milimoles

But H2SO4 is dibasic acid so milimoles of H+ in H2SO4 = 2×5 milimoles = 10 milimoles.

So from this we can see that :

HCl + NaOH —> BASIC

And H2SO4 + NaOH —> ACIDIC

on Mixing whole NaOH with any one of the Unlabeled test tubes and check out with litmus .

If the solution is basic unknown sample is HCl

If the solution is acidic unknown sample is H2SO4