Compare the ph of 0.1 m na2co3 and 0.1 m nahco3. select the statements that explain the difference. na2co3 is a stronger base. nahco3 is a stronger base. na2co3 puts more oh- ion into solution.

na2co3 is a stronger base

na2co3 puts more oh- ion into solution

Explanation:

Step 1: Calculate the pH of 0.1 M Na2CO3

Kb value for Na2CO3 = 2.1 * 10⁻⁴

Set up an ICE table

          CO_{3}^{2-}  + H_{2} O ------HCO_{3}^{-}  + OH^{-} \\[/tex]

I           0.1                    -                             -               -

C         -x                                                +x                   +x

E       (0.1-x)                                            x                      x

Step 2: Calculate pH of 0.1M NaHCO3

NaHCO3 is amphiprotic i,e it acts as an acid and base

For amphiprotic systems:

Conclusion:

pH of 0.1 M Na2CO3 = 11.66

pH of 0.1 M NaHCO3 = 8.33

Higher the pH , more basic the solution. Hence, Na2CO3 is a stronger base than NaHCO3

explanation:

let the different atoms be x and y. each with four protons and same mass will be represented as follows.

mass number is number of protons + number of neutrons.

            and  

since, it is given that one has a negative charge while the other is neutral. therefore, there will be increase in number of protons and the atom will be represented as follows.

according to periodic table, mass number of beryllium is 9 and it has atomic number 4 so, the atoms will be and .  

the protons and neutrons will be located inside the nucleus whereas the electrons will be revolving around the nucleus.  

the answer your looking for is c).