What is the pH of a 0.35 M solution of NO2-? (Ka of HNO2 = 4.0 x 10-4)
7.32
8.47
5.53
9.86
4.16
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
Calculate the pH of 0.35 M KNO2. What is the molarity of HNO2? The Ka for HNO2 is 7.1 ×10‒4.
d) ka-9.jj×10 Ka 1.45 x 104 P19. (Sec. 15.5) What is the pH of a 0.35 M solution of nitrous acid, HNO2? [Hint: ICE Table & Percent Ionization] & (Ka 4.5 x 104) HNO2(aq)H(aq)+ NO2 (aq)4.5 x 1o a) 4.11 b) 3.29 c) 12.70 d) 1.90 e) 9.10 P20. (Sec. 15.5) What is the pH of a 0.095 M solution of hydrofluoric acid, HF? [Hint: ICE Table & Percent Ionization] & (Ka = 6.8 × 10-4) 4
HNO2 has an acid dissociation constant of Ka = 4.0 x 10-4. What is the pH of a 0.25 M NO2- solution? a. 2.00 b. 4.30 c. 8.40 d. 10.25 e. 14.00
Question 52 of 68 What is the pH of a 0.320 M solution of Ca(NO2)2 (Ka of HNO2 is 4.5 x 10²4)? х +/- x 100
You have nitrous acid, HNO2, Ka=4.0 x 10-4 Calculate the pH of the solution and calculate the concentration of HNO2 and its conjugate base in a 0.025 M HNO2 Solution. Please please show all work!
What is the pH of a 0.043 M solution of nitrous acid, HNO2? Ka = 4.6 x 10-4
What is the pH of a solution prepared to 0.040 M NaNO2. Ka HNO2 = 7.1 x 10-4
Calculate the pH of a 0.400 M HNO2 solution. Report answer to 2 decimal places. Ka = 7.1 x 10-4 HNO2 (aq) + H20 (1) = NO2 (aq) + H30+ (aq) Calculate the pH of a solution consisting of 0.225 M solution of CH3NH2 (methylamine) and 0.200 M CH3NH3 (methylammonium chlorides Report answer to 2 decimal places. CHH) - 4.4 x 10-4 CH3NH2 (aq) + H200 - Chynas (aq) + OH" () 1. Questa
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