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A) Write a net ionic equation for the reaction that occurs when sodium sulfite (aq) and excess nitric acid (aq) are combined. Note: Sulfites follow the same solubility trends as sulfates.
B) Write a net ionic equation for the reaction that occurs when iron(II) sulfide (s) and excess hydriodic acid (aq) are combined.
Include in your explanation from which C and in what form the H would have to leave: [H+, H(with one electron), H(with two electrons)].
Lethality of Carbon Monoxide, Sulfur Dioxide and TNT Air monitoring provides the following contaminant concentrations at the approximate center of a fire scene in which acres of automobile tires are burning:
The water level in a graduated cylinder initially at 225 rises to 278 after a piece of lead is submerged. What is the mass in grams of the lead?
Where does the extra electron come from when determining the formal charge of NH2? N has 5 valence electrons and H each have one which lead to two bonds and one lone pair and one lone electron which equals a formal charge
A 0.250 mol sample of argon gas has a volume of 9.00 L at a pressure of 875 mm Hg. What is the temperature (in celsius) of the gas?
200 drops of 0.025 M NaF solution and 100 drops of 0.025 M Ba(NO3)2 solution are mixed. a.) write the equation for the formation of solid BaF2.
How many molecules (not moles) of NH3 are produced from 1.52×10?4g of H2?
At a certain temperature and pressure 4.2 L of N2 reacts with 6.3 L of O2. If all the N2 and O2 are consumed, what volume of N2O3, at the same temperature and pressure, will be produced?
What is the mole fraction of solute and the molal concentration for an aqueous solution
Which of the following correctly lists the following isomeric alkanes in order of increasing boiling point? n-hexane, 2,3-dimethylbutane, 2-methylpentane
What is the pH of the solution resulting from the addition of 25.0 mL of .01M NaOH solution to 40.0 mL of .01M acetic acid
Calculate the expansion work done against a constant external pressure of 0.999 atm and at a constant temperature of 24°C. Assume that the initial volume of dry ice is negligible and that CO2 behaves like an ideal gas.
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