An important part of acid/base chemistry is neutralization, or when an acid or a base is completely used up during a reaction. Assume the reaction below goes to completion. + NaOH(aq) H₂CO3(aq) Nat is a alkali ion acid base conjugate base conjugate acid →→→>> Na+ HCO3( (aq) OH is the H₂CO3 is the , HCO3 is the + H₂O and H₂O is the There is a 1:1 stochiometric ratio between NaOH and H₂CO3. Therefore, if we have 5 moles of NaOH, we need 5 moles of H₂CO3 for neutralization.
An important part of acid/base chemistry is neutralization, or when an acid or a base is completely used up during a reaction. Assume the reaction below goes to completion. + NaOH(aq) H₂CO3(aq) Nat is a alkali ion acid base conjugate base conjugate acid →→→>> Na+ HCO3( (aq) OH is the H₂CO3 is the , HCO3 is the + H₂O and H₂O is the There is a 1:1 stochiometric ratio between NaOH and H₂CO3. Therefore, if we have 5 moles of NaOH, we need 5 moles of H₂CO3 for neutralization.
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Chapter1: Chemical Foundations
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Question
Both are the same question, the image with the chemical equation in it is for context.
The second part is asking about whether the acid will be in: excess, limiting reagent, or equal moles to base.
The therefore part is referring to whether it will be neutralized or not.
Can someone help with this second part?
Thank you
Transcribed Image Text:An important part of acid/base chemistry is neutralization, or
when an acid or a base is completely used up during a
reaction.
Assume the reaction below goes to completion.
+ NaOH(aq)
H₂CO3(aq)
Nat is a alkali ion
acid
base
conjugate base
conjugate acid
There is a
→→→→
1:1
V
V
Na+ HCO3
(aq)
OH is the
H₂CO3 is the
HCO3 is the
+ H₂0
and H₂O is the
stochiometric ratio
between NaOH and H₂CO3. Therefore, if we have 5 moles of
NaOH, we need 5
moles of
H₂CO3 for neutralization.
![There is a 1:1
between NaOH and H₂CO3. Therefore, if we have 5 moles of
NaOH, we need 5
moles of
H₂CO3 for neutralization.
If we have 5 mL of 1 M NaOH and add 2.5 mL of 2 M H₂CO3,
the acid is in excess
and is therefore
not neutralized
If we have 10 mL of 0.1 M NaOH and add 16 mL of 0.05 M
H₂CO3, the acid is equal moles to the base
therefore neutralized
✓[Select
If we have 2 mL of 5 M NaOH and add 5 mL of 3 M H₂CO3,
the acid is [Select]
and is therefore
neutralized
not neutralized
Overall
Reaction:
Molecular
Weight (g/mol):
Na2CO3(aq)
105.99
stochiometric ratio
+ HCl (aq)
36.46
-
and is
NaHCO3(aq) + NaCl(aq)
84.001
58.44
ㅏ
G](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F84577f47-6855-4e4f-91d0-241ebc051b86%2F5fec35ca-8e0a-4dfe-834b-bd36c7fb6d15%2Fk6x93ys_processed.jpeg&w=3840&q=75)
Transcribed Image Text:There is a 1:1
between NaOH and H₂CO3. Therefore, if we have 5 moles of
NaOH, we need 5
moles of
H₂CO3 for neutralization.
If we have 5 mL of 1 M NaOH and add 2.5 mL of 2 M H₂CO3,
the acid is in excess
and is therefore
not neutralized
If we have 10 mL of 0.1 M NaOH and add 16 mL of 0.05 M
H₂CO3, the acid is equal moles to the base
therefore neutralized
✓[Select
If we have 2 mL of 5 M NaOH and add 5 mL of 3 M H₂CO3,
the acid is [Select]
and is therefore
neutralized
not neutralized
Overall
Reaction:
Molecular
Weight (g/mol):
Na2CO3(aq)
105.99
stochiometric ratio
+ HCl (aq)
36.46
-
and is
NaHCO3(aq) + NaCl(aq)
84.001
58.44
ㅏ
G
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