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- The ionization constant, Ka, for dichloroacetic acid, HC2HO2Cl2 , is 5.0 × 10‑2. What is the pH of a 0.15 molar solution of this acid?Estimate the pH of 0.05 M NaCN(aq) at 25°C. Ka(HCN) = 3.4 × 10−9. Write your answer with two decimal placesCalculate the pH of a solution of 0.0005 M sodium actate (NaAc) at 25 °C.
- Determine the pH of a 1.497 M solution of potassium cyanide (KCN) in water. Ka for HCN is 6.17 × 10–10. Enter your response in pH units to the nearest 0.01.The hydroxide ion concentration of an aqueous solution of 0.532 M phenol (a weak acid), C,H;OH, is [OH] = M.The base protonation constant K, of ammonia (NH,) is 1.8 x 10 . Calculate the pH of a 1.1 M solution of ammonia at 25 °C. Round your answer to 1 decimal place. pH =
- The pH of an aqueous solution of acetic acid (CH3COOH) is 2.0. What is the initial molar concentration of CH3COOH, if its acid ionization constant is Ka = 1.8×10–5?The value of K₂ for nitrous acid is 4.50×10-4. What is the value of K₁, for its conjugate base, NO₂? ||The base protonation constant K of ammonia (NH₂) is 1.8 × 10¯5. Calculate the pH of a 1.2 M solution of ammonia at 25 °C. Round your answer to 1 decimal place. pH = 0 X 血