Question

2) a) Write the chemical reaction showing hydrogen carbonate polyatomic ion acting as an acid in water.

b) Write the chemical reaction showing hydrogen carbonate polyatomic ion acting as a base in water.


3) Acidic solutions have pH
than 7, while basic solutions have pH.
Neutral solutions have pH.


4) In a certain aqueous solution, the concentration of [H*] = 1.0 x 10-4 mol/L.

a) Calculation the pH of this solution. Show your work.

b) Is this solution acidic, neutral, or basic?


5) In another solution, the concentration of (H*1 = 1.0 × 10° mol/L.

a) Calculation the pH of this solution. Show your work.

b) Is this solution acidic, neutral, or basic?

c) Can a basic solution have any H* ions in it?

Answer 1

a) When hydrogen carbonate (HCO3-) acts as an acid in water, it donates a proton (H+) to water. The chemical equation can be written as: HCO3- + H2O → H2CO3 + OH-. b) When hydrogen carbonate (HCO3-) acts as a base in water, it accepts a proton (H+) from water. The chemical equation can be written as: HCO3- + H2O →
`CO3^(2-)` + H3O+. 3) Acidic solutions have a pH less than 7, while basic solutions have a pH greater than 7. Neutral solutions have a pH of 7.

Step-by-step explanation:

a) When hydrogen carbonate (HCO3-) acts as an acid in water, it donates a proton (H+) to water. The chemical equation can be written as: HCO3- + H2O → H2CO3 + OH-

b) When hydrogen carbonate (HCO3-) acts as a base in water, it accepts a proton (H+) from water. The chemical equation can be written as: HCO3- + H2O →
`CO3^(2-)` + H3O+

3) Acidic solutions have a pH less than 7, while basic solutions have a pH greater than 7. Neutral solutions have a pH of 7.

4) a) The pH of the solution can be calculated using the formula pH = -log[H+]. Given [H+] = 1.0 x 10-4 mol/L, the pH can be calculated as -log(1.0 x
`10^(-4)`) = 4.

b) Since the pH of the solution is less than 7, it is acidic.

5) a) The pH of the solution can be calculated using the formula pH = -log[H+]. Given [H+] = 1.0 x
`10^0` mol/L, the pH can be calculated as -log(1.0 x
`10^0`) = 0.

b) Since the pH of the solution is equal to 7, it is neutral.

c) No, a basic solution cannot have any H+ ions in it. Basic solutions have a lower concentration of H+ ions compared to neutral solutions.

Answer 2

2a) The chemical reaction showing hydrogen carbonate polyatomic ion (HCO3-) acting as an acid in water is:

HCO3- + H2O → H3O+ + CO32-

In this reaction, the hydrogen carbonate ion donates a hydrogen ion (H+) to water, forming hydronium ion (H3O+) and carbonate ion (CO32-).

2b) The chemical reaction showing hydrogen carbonate polyatomic ion (HCO3-) acting as a base in water is:

HCO3- + H2O ↔ H2CO3 + OH-

In this reaction, the hydrogen carbonate ion accepts a hydrogen ion (H+) from water, forming carbonic acid (H2CO3) and hydroxide ion (OH-).

3) Acidic solutions have a pH less than 7, while basic solutions have a pH greater than 7. Neutral solutions have a pH of 7.

4a) The pH of a solution can be calculated using the formula:

pH = -log[H+]

Given [H+] = 1.0 x 10^-4 mol/L, we have:

pH = -log(1.0 x 10^-4) = 4

Therefore, the pH of the solution is 4.

4b) Since the pH of the solution is less than 7, it is acidic.

5a) The pH of a solution can be calculated using the formula:

pH = -log[H+]

Given [H+] = 1.0 x 10^0 mol/L, we have:

pH = -log(1.0 x 10^0) = 0

Therefore, the pH of the solution is 0.

5b) Since the pH of the solution is 0, it is highly acidic.

5c) No, a basic solution cannot have any H+ ions in it. Basic solutions have a higher concentration of hydroxide ions (OH-) than hydrogen ions (H+).