equal length of magnesium ribbon are taken in two test tubes A and B.
H2SO4 is added to test tube 'A' and H2CO3 is added in test tube 'B' in equal amounts:
a. Identify the test tube showing vigorous reaction.
b. Give reason to support your answer.
C. Name the gas liberated in both the test tubes. How will you prove its liberation?
1. Write chemical equations for both the reactions.
Out of two acids taken above, which one will have lower pH value and lower H+ ion concentration
respectively?
Answers
Answer:
see the answer down here
Explanation:
A) test tube A will show a vigorous reaction
B) since H2SO4 is a strong acid it liberates more hydrogen gas on reacting with magnesium whereas H2CO3 being a weak acid liberates less of hydrogen gas on reaction .
C) the gas liberated is hydrogen we can test its presence by bringing a burning matchstick near it and will hear a pop sound .
1) reaction of magnesium with sulphuric acid :
Mg + H2So4 === MgSo4 + H2
reaction of magnesium with carbonic acid:
Mg + H2Co3 ==== Mg(Co3)2 + H2
out of the following sulphuric acid will have a lower pH value and carbonic acid will have lower H+ ion concentration
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