Find the pH of each mixture of acids. b. 0.150 M in HNO₂ and 0.085 M in HNO₃ c. 0.185 M in HCHO₂ and 0.225 M in HC₂H₃O₂ d. 0.050 M in acetic acid and 0.050 M in hydrocyanic acid

Verified step by step guidance

1. Step 1: Identify the acids in each mixture and determine their strengths. HNO_3 is a strong acid, while HNO_2, HCHO_2, HC_2H_3O_2, and hydrocyanic acid (HCN) are weak acids.
2. Step 2: For each mixture, calculate the contribution of the strong acid to the pH. Since strong acids dissociate completely, the concentration of H^+ ions from the strong acid is equal to its initial concentration.
3. Step 3: For the weak acids, use the acid dissociation constant (K_a) to calculate the concentration of H^+ ions. Set up an equilibrium expression for each weak acid: K_a = [H^+][A^-]/[HA].
4. Step 4: For each mixture, add the concentration of H^+ ions from the strong acid to the concentration of H^+ ions from the weak acids to find the total [H^+].
5. Step 5: Calculate the pH of each mixture using the formula pH = -log[H^+].