Hello student
I am here to help youmy answer is 2.21 which is close to 2.17 hence its c option is correct
Thank you
What is the pH of aqueous 0.10 M HNO2? Ka(HNO2) = 4.5 x 10-4 a. 1.67 b. 3.35 c 1.00 d. 4.35 e. 2.17
What is the pH of aqueous 0.10 M HNO2? K (HNO3) = 4.5 * 10-4 O a. 1.67 Ο 6. 3.35 ι Ο υ τ Ο ο Ο υ
Calculate the pH of a 0.383 M aqueous solution of nitrous acid (HNO2, Ka = 4.5×10-4) and the equilibrium concentrations of the weak acid and its conjugate base. pH = [HNO2 ]equilibrium = M [NO2- ]equilibrium = M
What is the pH of a 0.50 M NO2- solution. The Ka of HNO2 is 4.5 x 10-4. a) 7.54 b) 8.52 c) 8.30 d) 7.76 e) 8.04
Nitrous acid, HNO2(aq), has a Ka of 4.5 x 10-4 at 25 °C. What is the pH of a solution that contains 1.0 M KNO2(aq) and 0.50 M HNO2(aq).
Header & FO 5) Using the data in the table for 0.10 M aqueous species at 25°C, which conjugate base below is the weakest base? Explain your answer for full credit! Acid НОАс 1.8 x 10-5 HC7H502 6.3 x 10-5 HNO2 4.5 x 10-4 HF 6.8 x 10-4 6) The K, for HCN is 4.9 10-10. What is the pH of a 0.068 M aqueous solution of potassium cyanide?
13) Using the data in the table for 0.10 M aqueous species at 25°C, which conju base below is the weakest base? Explain your answer for full credit! НОАс Acid 1.8 x 10-5 HC7H502 6.3 x 10-5 HNO2 4.5 x 10-4 6.8 x 10-4 HF 14) The K, for HCN is 4.9 x 10-10. What is the pH of a 0.068 M aqueous solutie potassium cyanide?
Calculate the (H+) and pH of a 2.55 x 10-4 M butanoic acid solution. The Ką of butanoic acid is 1.52 x 10-5. 0.000063246 M pH = 4.1989
What is the pH of a 0.180 M aqueous solution of potassium nitrite, KNO2 at 25 °C? (Ka for HNO2 = 4.5×10-4)
9. What is the pH for 0.20 M HCIO solution? K = 2.5 x 10-7 a) 4.05 b) 3.70 c) 4.80 d) 7.00 e) 7.40 10. What is the pH of a mixture containing 0.30 M HNO, and 0.15 M NaNO, (K, for HNO2 is 4.5 x 104) a) 4.35 b) 3.05 c) 4.65 d) 5.01 e) 4.05 11. Acid strength increases in the series: HCN <HF <HSO.. Which of these species is the strongest base? a) SO42- b) F-...