Write an equation that explains the conductivity of NH3
NH3 + HOH ==> NH4^+ + OH^-
NH3 is a base, it accepts a proton from water (HOH), and forms the two ions shown. Those ions conduct electricity through the solution.
If you use the lmax during the calibration plot (Beer's plot) and then change to some other wavelength for the measurement of the sample, how will this affect x?
The equation that explains the conductivity of NH3 (ammonia) is:
NH3 + H2O ⇌ NH4+ + OH-
In this equation, ammonia (NH3) reacts with water (H2O) to form ammonium ions (NH4+) and hydroxide ions (OH-). These ions are responsible for the conductivity of the solution. Ammonium ions are positively charged and can move towards the negative electrode (cathode), while hydroxide ions are negatively charged and can move towards the positive electrode (anode). The movement of these ions allows the flow of electric current, indicating the solution's conductivity.
The equation that explains the conductivity of NH3 (ammonia) is:
NH3 + H2O <--> NH4+ + OH-
Ammonia (NH3) can dissolve in water (H2O) to form ammonium ions (NH4+) and hydroxide ions (OH-). The presence of these ions allows the solution to conduct electricity.
To understand this equation, let's break it down:
- NH3: This represents the ammonia molecule.
- H2O: This represents water, or H2O molecules.
- NH4+: This represents the ammonium ion, which is formed when ammonia accepts a proton (H+) from the water molecule.
- OH-: This represents the hydroxide ion, which is formed when water donates a hydroxyl group (OH-) to the ammonia molecule.
When ammonia (NH3) dissolves in water (H2O), it is able to form ammonium ions (NH4+) and hydroxide ions (OH-). These ions can move around freely in the solution, allowing the solution to conduct electricity.
Therefore, the equation NH3 + H2O <--> NH4+ + OH- explains the conductivity of NH3.