Question

Calculate the ph of a solution that is 1.10×10−3 m in hcl and 1.20×10−2 m in hclo2.

Answer 1

To calculate the pH of the given solution, we need to find the hydronium ion concentration and use the pH formula. The pH is approximately 1.88.

Step-by-step explanation:

In order to calculate the pH of a solution, we need to determine the hydronium ion concentration, [H3O+].

1. For the HCl solution with a concentration of 1.10×10−3 M, the hydronium ion concentration is equal to the HCl concentration. So, [H3O+] = 1.10×10−3 M.
2. For the HClO2 solution with a concentration of 1.20×10−2 M, the hydronium ion concentration is also equal to the HClO2 concentration. So, [H3O+] = 1.20×10−2 M.
3. Add the hydronium ion concentrations from both solutions together to get the total hydronium ion concentration: [H3O+] = 1.10×10−3 M + 1.20×10−2 M = 1.31×10−2 M.
4. Finally, calculate the pH using the formula pH = -log[H3O+]: pH = -log(1.31×10−2) = 1.88.

Therefore, the pH of the solution is approximately 1.88.

Answer 2

To calculate the pH of the solution, we need to consider the dissociation of HCl and HClO₂. HCl dissociates completely, so its concentration of H₃O+ ions is equal to its concentration. HClO₂ is a weak acid, so we need to use the equilibrium expression.

Step-by-step explanation:

To calculate the pH of the solution, we need to consider the dissociation of HCl and HClO₂. HCl dissociates completely, so its concentration of H₃O+ ions is equal to its concentration. HClO₂ is a weak acid, so we need to use the equilibrium expression.

Given [HCl] = 1.10 × 10⁻³ M and [HClO₂] = 1.20 × 10⁻² M, we can find the concentrations of H₃O+ ions. The pH is calculated as the negative logarithm (base 10) of the H₃O+ concentration.

pH = -log[H₂O+]