Asked by Naomie

WOULD THE VOLUME OF A 0.10M NAOH SOLUTION NEEDED TO TITRATE25.0ML OF A 0.10M HNO2 ( A WEAK ACID)SOLUTION BE DIFFERENT FROMTHAT NEEDED TO TITRATE 25.0ML OF A 0.10M HCL (A STRONGACID)SOLUTION?

Answers

Answered by bonjo
that depends on the number of moles of the acids that need to be neutralized by the base and the concentration of the base.


1. HNO2 + NaOH --> NaNO2 + H2O

i.e. 1 mole base react with 1 mole acid

the mole for the HNO2 is cv = 0.1Mx0.025L = 0.0025mol = mole of NaOH

therefore, v(NaOH) = n/c = 0.0025/0.1 = 0.025L (25mL)

2. HCl + NaOH --> NaCl + H2O

so again the 1:1 reaction, and the mole for the HCl is cv = 0.1x0.025L = 0.0025mole = mole of NaOH

v(NaOH) = n/c = 0.0025/0.1 = 25mL

so the volume of NaOH required to neutralize the HNO2 and HCl is 25mL. i.e. same volume.

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