Question

As shown by the equations: H2O + HCO3− table_14.JPG H3O+ + CO32− H2O + HCO3− table_14.JPG...

As shown by the equations: H2O + HCO3− table_14.JPG H3O+ + CO32− H2O + HCO3− table_14.JPG H2CO3 + OH−

a)water is a base

b)water is an acid

c)water is amphoteric

d)water is neutral

Homework Answers

Answer #1

H2O    +      HCO3−   .............>    H3O+      +       CO32−

Water accepts the proton from HCo3- so it act as a base

H2O +    HCO3− .............>    H2CO3 + OH−

Water donates the proton to HCo3- so it act as a acid

A compound which act as both proton donor and acceptor is called amphotric. So water is amphotiric

answer C is correct

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Identify the conjugate acid-base pair in the equation: H3O+(aq)+CO32−(aq)⇌H2O(l)+HCO3−(aq) Identify the conjugate acid-base pair in the...
Identify the conjugate acid-base pair in the equation: H3O+(aq)+CO32−(aq)⇌H2O(l)+HCO3−(aq) Identify the conjugate acid-base pair in the equation: H2O(l)+HBr(aq)⇌H3O+(aq)+Br−(aq)
1. Net ionic equation before the equivalence point: CO32-(aq) + H+ (aq) <--> HCO3-(aq) K= 1.8...
1. Net ionic equation before the equivalence point: CO32-(aq) + H+ (aq) <--> HCO3-(aq) K= 1.8 x 1010 What is the relationship between this reaction (above) and this reaction (below)? HCO3-(aq) + H2O(l) <--> H3O+(aq) + CO32-(aq) K= 5.6 x 10-11 2. Net ionic equation after the equivalence point: HCO3-(aq) + H+(aq) <--> H2CO3(aq) K= 2.3 x 106 What is the relationship between this reaction (above) and this reaction (below)? H2CO3(aq) + H2O (l) <--> H3O+(aq) + HCO3-(aq) K= 2.6...
Calculate the concentration of [H2CO3], [HCO3(-)], [CO3 (2-)], [H3O(+)], and [OH(-)] in a 0.140M solution of...
Calculate the concentration of [H2CO3], [HCO3(-)], [CO3 (2-)], [H3O(+)], and [OH(-)] in a 0.140M solution of H2CO3. In paranthesis, are the charges of the ions.
What is the percent ionization of carbonic in 0.1441 M carbonic acid solution, H2CO3? H2CO3(aq) +...
What is the percent ionization of carbonic in 0.1441 M carbonic acid solution, H2CO3? H2CO3(aq) + H2O(l) « HCO3−(aq) + H3O+(aq) Ka1 = 4.3000e-7 HCO3−(aq) + H2O(l) « CO32−(aq) + H3O+(aq) Ka2 = 5.6000e-11
Consider the following equation: CO2 + H2O -<-> H2CO3<-> H3O+ + HCO3- Explain how this equation...
Consider the following equation: CO2 + H2O -<-> H2CO3<-> H3O+ + HCO3- Explain how this equation helps buffer blood. What organ systems are working to maintain a normal blood pH? What is meant by metabolic and respiratory acidosis and alkalosis?
A water has a pH of 8.00 and the concentration of HCO3- is 193.00 mg/L. What...
A water has a pH of 8.00 and the concentration of HCO3- is 193.00 mg/L. What is the alkalinity of the water in unit of mg/L as CaCO3? (Note: The pKa for H2CO3/HCO3- is 6.3. The pKa for HCO3-/CO32- is 10.33. The pKa for the dissociation of water to H+ and OH- is 14.0. The temperature is 25oC
Hard/ Soft water: Why is CaCO3 present in hot water, but not in cold? My prfoessor...
Hard/ Soft water: Why is CaCO3 present in hot water, but not in cold? My prfoessor talked about he has his water softerner only for hot water, but the cold water is not passed through a water softner. Can you please explain showing step by step equilibrium reactions and where the equilibrium is favored. Here are a few equations that might help your thought process. I guess I would just like an explaination as to why hot vs cold and...
The alkalinity of a water consists of 12 mg/L of CO32- and 100 mg/L HCO3-. Calculate...
The alkalinity of a water consists of 12 mg/L of CO32- and 100 mg/L HCO3-. Calculate the alkalinity in mg/L as CaCO3 by Ignoring [OH-] and [H+].
1.) You will work with 0.10 M acetic acid and 17 M acetic acid in this...
1.) You will work with 0.10 M acetic acid and 17 M acetic acid in this experiment. What is the relationship between concentration and ionization? Explain the reason for this relationship 2.) Explain hydrolysis, i.e, what types of molecules undergo hydrolysis (be specific) and show equations for reactions of acid, base, and salt hydrolysis not used as examples in the introduction to this experiment 3.) In Part C: Hydrolysis of Salts, you will calibrate the pH probe prior to testing...
a.) Phosphoric acid is a triprotic acid: H3PO4(aq) +H2O(l) ↔ H3O+(aq) + H2PO4-(aq) Ka1 = 7.5...
a.) Phosphoric acid is a triprotic acid: H3PO4(aq) +H2O(l) ↔ H3O+(aq) + H2PO4-(aq) Ka1 = 7.5 x 10-3 H2PO4-(aq) +H2O(l) ↔ H3O+(aq) + HPO42-(aq) Ka2 = 6.2 x 10-8 HPO42-(aq) +H2O(l) ↔ H3O+(aq) + PO43-(aq) Ka3 = 4.8 x 10-13 Determine whether sodium monohydrogen phosphate (Na2HPO4) is neutral, basic, or acidic. First, what is its Ka when it acts as an acid? b.) Second, what is its Kb when it acts as a base? c.) Finally, indicate whether the HPO42-...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT