Magnesium ribbons of same size are taken in test tubes A and B. Hydrochloric acid is added
to test tube A. while acetic acid is added to test tube B. The concentrations of both the acids
are the same. In which test tube will the fizzing occur more vigorously? why? (AS)
Answers
Step-by-step explanation:
please follow me please.........
Answer :
As we know all acids have the common property of disassociating hydrogen when mixed with a liquid solution . In test tube A we have taken HCL or hydrochloric acid which has a stronger pH value and hence stronger hydrogen releasing properties in it . In test tube B acetic acid is taken which is a very weak acid when in comparison with hydrochloric acid . Magnesium ribbons when added to any acid will give off a vigorously fizzing gas . This is nothing but hydrogen gas . When magnesium ribbon is put in test tube A which contains HCL ( hydrochloric acid ) a very strong fizzing reaction occurs due to HCL being a very strong acid . But though acetic acid when in contact with magnesium ribbon does produce hydrogen gas fizzing , it is not as vigorous as the reaction of magnesium ribbon with hydrochloric acid because hydrochloric acid is much more stronger than acetic acid .
Hope you find my answer useful!!