Determine the pH of each two-component solution. a. 0.050 M KOH and 0.015 M Ba(OH)₂ b. 0.265 M NH₄NO₃ and 0.102 M HCN c. 0.075 M RbOH and 0.100 M NaHCO₃ e. 0.115 M NaClO and 0.0500 M KI

Verified step by step guidance

1. Step 1: Identify the nature of each component in the solution. For example, KOH and Ba(OH)_2 are strong bases, NH_4NO_3 is a salt of a weak base (NH_3) and a strong acid (HNO_3), HCN is a weak acid, RbOH is a strong base, NaHCO_3 is a weak base, NaClO is a salt of a weak acid (HClO) and a strong base (NaOH), and KI is a neutral salt.
2. Step 2: For solutions containing strong bases (like KOH and Ba(OH)_2), calculate the total hydroxide ion concentration by adding the contributions from each base. Remember that Ba(OH)_2 dissociates to give two OH^- ions per formula unit.
3. Step 3: For solutions containing weak acids and their salts (like NH_4NO_3 and HCN), use the Henderson-Hasselbalch equation to find the pH. Calculate the pKa of HCN and use the concentrations of NH_4^+ and HCN to find the pH.
4. Step 4: For solutions containing a strong base and a weak base (like RbOH and NaHCO_3), determine the dominant species affecting the pH. Since RbOH is a strong base, it will dominate the pH calculation. Calculate the pH based on the concentration of OH^- from RbOH.
5. Step 5: For solutions containing salts of weak acids (like NaClO and KI), consider the hydrolysis of the anion from the weak acid (ClO^-). Use the Kb of ClO^- to calculate the pH, considering that KI does not affect the pH as it is a neutral salt.