Since no2 in liquid form is considered an acid, it has a ph lower than 7 yet it is still consumable therefor it is a weak acid most likely with a ph of higher than 4
HNO2 ==> H+ + NO2^-Ka = 4x10^-4 = [H+][NO2^-]/[HNO2] 4x10^-4 = (x)(x)/0.100 x^2 = 4x10^-5 x = 6.32x10^-3 = [H+] pH = -log 6.32x10^-3 pH = 2.2
NO2- is a base not an acid. It's conjugate acid is HNO2.
Molar mass NO2 = 46.0 g/mole1.18 g NO2 x 1 mol NO2/46.0 g = 0.0257 moles NO2 (to 3 significant figures)
2x air+lighting=no2
Ca(NO2)2
They do not have any effect
HNO2 ==> H+ + NO2^-Ka = 4x10^-4 = [H+][NO2^-]/[HNO2] 4x10^-4 = (x)(x)/0.100 x^2 = 4x10^-5 x = 6.32x10^-3 = [H+] pH = -log 6.32x10^-3 pH = 2.2
These are oxides which can form acids: NO2, SO2, CO2.
NO2 is the molecular formula for NO2.
NO2+ is.
NO2 is the chemical formula for nitrous oxide.
NaNO2 yields NO2 - + Na+ The salt NaNO2 completely ionizes, producing 0.35M [NO2-] and 0.35 [Na+] ions. NO2- is the conjegate base of the weak acid HNO2. You have to write a balanced equation for the reation at equilibrium. After you have done so, you need to set up an ICE (Initial, change, equilibrium) table, experssing the equilibrium concentrations of all species in terms of initial concentrations and a single unknown x, that represenst the change in concentraion: NO2 - + H2O yields HNO2 + OH- ---- Initial 0.35 0.00 0.00 Change -x +x +x ---- Equil. 0.35-x x x Know we use the equilibrium equation: Kb = [HNO2][OH-]/[NO2 - ] (2.5 x 10-11) = x2/ 0.35 - x (in this case we can omitt the x that is subtracted from the 0.35 concentration because the Kb value is so small and will not affect the value) So, 2.5 x 10-11 = x2/0.35 x = [OH-] = 2.96 x 10-6 Now that we have solved for the OH- concentration, we can solve for the pOH and then use that to solve for the pH. pOH = -log[OH-] pOH = -log[2.96 x 10-6] pOH = 5.53 pH + pOH = 14 pH = 14 - pOH pH= 14 - 5.53 pH= 8.47 ----
NO2- is a base not an acid. It's conjugate acid is HNO2.
Determine the molar mass of NO2 using the subscripts in the formula and the atomic weights in grams from the periodic table. 1 mole NO2 = (1 x 14.0067g N) + (2 x 15.9994g O) = 46.0055g NO2 Calculate the moles NO2 by dividing the given mass by the molar mass. 25.5g NO2 x (1mol NO2/46.0055g NO2) = 0.554mol NO2
No. NO2 Is Nitrogen Dioxide.
NO2 is a conjugate base.
nitrogen dioxide = NO2