Question

Equal length of magnesium ribbon are taken in two test tubes 'A' and 'B'. H2SO4 is added to test tube 'A' and H2CO3 in the test tube B' in equal amounts. Out of the acids taken above, which one will have (i) lower pH value and why? (ii) lower H ion concentration respectively? (iii) In which test tube will the fizzing occur more vigorously and why?​

Answer 1

Answer:

a) H

2

SO

4

test tube i.e A will show more rigorous reactions

b) Since acidic strength of H

2

SO

4

is more than H

2

CO

3

c) Mg+H

2

SO

4

→MgSO

4

+H

2

(g)

Mg+H

2

CO

3

→MgCO

3

+H

2

(g)

The liberated gas is H

2

and it burns with popping sound.

d) Mg+H

2

SO

4

→MgSO

4

+H

2

(g)

Mg+H

2

CO

3

→MgCO

3

+H

2

(g)

e)

i) Since H

2

SO

4

is more acidic, it will have lower pH value.

ii) Test tube B will have lower H

+

concentration as H

2

CO

3

is a weak acid.