It is able to (completely) donate its protons (H+) to water when in dilute solution (protolysis). This is what, according to Bronsted-Lowry, makes it a (strong) acid.
HNO3 + H2O --> H3O+ + NO3-
This is nitric acid in water solution.
nitric acid.
Hydrogen nitrite acid
ka=[H+][NO2_]/[HNO2]
Ka= [H+][NO2-] [HNO2]
NO2-(aq) + H2O HNO2(aq) + OH -(aq)
HNO2 (aq) is nitrous acid in solution.
Nitrous acid HNO2 cannot be isolated as a pure compound. In the gas phase molecules of HNO2 are covalently bonded. In water it is a weak acid forming the nitrite ion however it readily disproportionates:- 3HNO2 -> H3O+ + NO3- + NO
Hydrogen nitrite acid
ka=[H+][NO2_]/[HNO2]
Ka= [H+][NO2-] [HNO2]
ka=[H+][NO2_]/[HNO2]
Equilibrium:NO2- (aq) + H2O HNO2 (aq) + OH- (aq)
NO2-(aq) + H2O HNO2(aq) + OH -(aq)
HNO2 (aq) is nitrous acid in solution.
HNO2 is nitrous acid. It is not to be confused with nitric acid, which is HNO3
NO2 is the polyatomic ionic compound nitrite Since it is bonded with hydrogen, this compound is an acid The correct name for HNO2, is therefore nitrous acid
Nitrous acid HNO2 cannot be isolated as a pure compound. In the gas phase molecules of HNO2 are covalently bonded. In water it is a weak acid forming the nitrite ion however it readily disproportionates:- 3HNO2 -> H3O+ + NO3- + NO
The compound NO is called "nitric oxide". Combined with oxygen and water, it forms HNO2, or nitrous acid.
The two will react to form salt and water HCOOH (aq)+ KOH(aq) --> HCOOK(aq) + H2O(l) In ionic form, HCOOH + K+ + OH- --> HCOO- + K+ + H2O HCOOH is weak acid so it should not be written in ionic form. K+ ions cancel out leaving HCOOH + OH- --> HCOO- + H2O (net ionic equation)