To answer this question, we first need to understand that the pH of a solution is determined by the concentration of hydrogen ions [H+] in the solution.

Sulphuric acid (H2SO4) is a strong acid and it completely ionizes in water to produce 2 moles of H+ ions per mole of H2SO4. Therefore, a 0.05 M H2SO4 solution will have a [H+] of 0.05 M * 2 = 0.1 M.

When this solution is diluted to 1L, the concentration of H+ ions remains the same because the number of moles of H+ ions does not change, only the volume of the solution changes. Therefore, the [H+] of the diluted solution is also 0.1 M.

Now, we need to find a solution from the given options that has the same [H+] as the diluted H2SO4 solution.

(A) 10^-2 M sodium hydroxide (NaOH) solution: NaOH is a strong base and it ionizes in water to produce OH- ions. The concentration of H+ ions in a basic solution can be calculated using the ion product of water (Kw = [H+][OH-] = 10^-14 at 25°C). If [OH-] = 10^-2 M, then [H+] = Kw / [OH-] = 10^-14 / 10^-2 = 10^-12 M. This is not equal to 0.1 M.

(B) 10^-2 M calcium hydroxide (Ca(OH)2) solution: Ca(OH)2 is a strong base and it ionizes in water to produce 2 moles of OH- ions per mole of Ca(OH)2. Therefore, [OH-] = 10^-2 M * 2 = 2*10^-2 M. Using the same calculation as above, [H+] = 10^-14 / (2*10^-2) = 5*10^-13 M. This is not equal to 0.1 M.

(C) 0.06 M hydrochloric acid (HCl) solution: HCl is a strong acid and it ionizes in water to produce 1 mole of H+ ions per mole of HCl. Therefore, [H+] = 0.06 M. This is not equal to 0.1 M.

(D) 0.01 M nitric acid (HNO3) solution: HNO3 is a strong acid and it ionizes in water to produce 1 mole of H+ ions per mole of HNO3. Therefore, [H+] = 0.01 M. This is not equal to 0.1 M.

Therefore, none of the given solutions has the same pH value as 100 mL of 0.05 M sulphuric acid diluted to 1L.

Question

To answer this question, we first need to understand that the pH of a solution is determined by the concentration of hydrogen ions [H+] in the solution.

Sulphuric acid (H2SO4) is a strong acid and it completely ionizes in water to produce 2 moles of H+ ions per mole of H2SO4. Therefore, a 0.05 M H2SO4 solution will have a [H+] of 0.05 M * 2 = 0.1 M.

When this solution is diluted to 1L, the concentration of H+ ions remains the same because the number of moles of H+ ions does not change, only the volume of the solution changes. Therefore, the [H+] of the diluted solution is also 0.1 M.

Now, we need to find a solution from the given options that has the same [H+] as the diluted H2SO4 solution.

(A) 10^-2 M sodium hydroxide (NaOH) solution: NaOH is a strong base and it ionizes in water to produce OH- ions. The concentration of H+ ions in a basic solution can be calculated using the ion product of water (Kw = [H+][OH-] = 10^-14 at 25°C). If [OH-] = 10^-2 M, then [H+] = Kw / [OH-] = 10^-14 / 10^-2 = 10^-12 M. This is not equal to 0.1 M.

(B) 10^-2 M calcium hydroxide (Ca(OH)2) solution: Ca(OH)2 is a strong base and it ionizes in water to produce 2 moles of OH- ions per mole of Ca(OH)2. Therefore, [OH-] = 10^-2 M * 2 = 2*10^-2 M. Using the same calculation as above, [H+] = 10^-14 / (2*10^-2) = 5*10^-13 M. This is not equal to 0.1 M.

(C) 0.06 M hydrochloric acid (HCl) solution: HCl is a strong acid and it ionizes in water to produce 1 mole of H+ ions per mole of HCl. Therefore, [H+] = 0.06 M. This is not equal to 0.1 M.

(D) 0.01 M nitric acid (HNO3) solution: HNO3 is a strong acid and it ionizes in water to produce 1 mole of H+ ions per mole of HNO3. Therefore, [H+] = 0.01 M. This is not equal to 0.1 M.

Therefore, none of the given solutions has the same pH value as 100 mL of 0.05 M sulphuric acid diluted to 1L.

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