Calculate the concentration of nitrite (NO2-) in a solution, which is 0.2M in nitrous acid and 0.0050 M in nitric acid (HNO3)
Comment in case of any doubt.
Calculate the concentration of nitrite (NO2-) in a solution, which is 0.2M in nitrous acid and...
1. A 1.00 liter solution contains 0.46 M nitrous acid and 0.35 M sodium nitrite. If 30.0 mL of water are added to this system, indicate whether the following statements are true or false. (Note the the volume MUST CHANGE upon the addition of water.) _______TrueFalseA. The concentration of HNO2 will remain the same. _______TrueFalseB. The concentration of NO2- will decrease. _______TrueFalseC. The equilibrium concentration of H3O+ will remain the same. _______TrueFalseD. The pH will increase. _______TrueFalseE. The ratio of...
Calculate the percent ionization of nitrous acid in a solution that is 0.222 M in nitrous acid (HNO2) and 0.278 M in potassium nitrite (KNO2). The acid dissociation constant of nitrous acid is 4.50 × 10-4.
A solution of nitrous acid, HNO2 is 6.3x10^-3 M, which is a weak acid with Ka=7.2x10^-4. Calculate: [HNO2] [NO2] pH What is the concentration of a nitrous acid solution with a pH of 2.21
The nitrous acid/sodium nitrite conjugate pair has been chosen to prepare a buffer solution. What should the concentration ratio of NO2-/HNO2 be if the desired pH of this buffer is 4.00? (Ka of HNO2 = 4.27 x 10-4)
A solution contains 0.271 M potassium nitrite and 8.24x10-2 M nitrous acid. The pH of this solution is A solution contains 7.53x10-2 M potassium nitrite and 0.104 M nitrous acid. The pH of this solution is
A 1.00 liter solution contains 0.54 moles nitrous acid and 0.42 moles potassium nitrite . If 0.21 moles of perchloric acid are added to this system, indicate whether the following statements are true or false. (Assume that the volume does not change upon the addition of perchloric acid.) A. The number of moles of HNO2 will remain the same. B. The number of moles of NO2 will increase. C. The equilibrium concentration of Hz0+ will increase. D. The pH will...
Now calculate the [H+] and pH of a 0.00725 M solution of nitrous acid. Nitrous acid (HNO2) is a weak acid that partially dissociates as follows, with a Ka = 0.0004266: HNO2 + H20 + H30+ + NO2 a) Calculate the [h+] and pH of a 1.73 M solution of nitrous acid. [H+]=49) 0.0270 b) pH = 49 1.57 c) Now calculate the [H+] and pH of a 0.00725 M solution of nitrous acid. 49) 0.0016 d) 49 1.7
A solution contains 0.440 M potassium nitrite and 0.102 M nitrous acid. The pH of this solution is .
A 1.00 liter solution contains 0.40 moles nitrous acid and 0.31 moles potassium nitrite. If 0.15 moles of hydrobromic acid are added to this system, indicate whether the following statements are true or false. (Assume that the volume does not change upon the addition of hydrobromic acid.) DA. The number of moles of HNO, will increase. B. The number of moles of NO, will increase C. The equilibrium concentration of H,0" will increase D. The pH will decrease. E. The...
Which is the conjugate base of nitrous acid, HNO2? NO2- NO4+ HNO3 H2NO2