A pollutant in smog is nitrogen dioxide, NO₂. The gas has a reddish brown color and is responsible for the red-brown color associated with this type of air pollution. Nitrogen dioxide is also a contributor to acid rain because when rain passes through air contaminated with NO2, it dissolves and undergoes the following reaction: 3NO2(g) + H₂O → NO(g) + 2H*(aq) + 2NO3(aq). In this reaction, which element is reduced and which is oxidized? OH is both reduced and oxidized. OO is oxidized and H is reduced. O is oxidized and N is reduced. ON is both reduced and oxidized. ON is oxidized and H is reduced. ON is oxidized and O is reduced.

The pH of an aqueous solution of 1.08×10-2 M carbonic acid, H2CO3 (aq), is

The following chemical reaction takes place in aqueous solution: AgF(aq)+KCl(aq) →AgCl(s)+KF(aq) Write the net ionic equation for this reaction. ☐

In sediments and waterlogged soil, dissolved O2 concentrations are so low that the microorganisms living there must rely on other sources of oxygen for respiration. Some bacteria can extract the oxygen in sulfate ions, reducing the sulfur in them to hydrogen sulfide gas and giving the sediments or soil a distinctive rotten-egg odor.Write the net ionic equation for the reaction under acidic conditions (H3O+) that releases O2 from sulfate and forms hydrogen sulfide gas. Use water as the reactant in the half-reaction that describes the formation of oxygen.

1. a) Write the formula for the conjugate base of HPO4^-2  b) Write the formula for the conjugate acid of NH3

What is the pH of 3.5 × 10−4 M HNO3 (aq)?

The pH of an aqueous solution of 8.39×10-2 M ammonium nitrate, NH4NO3 (aq), is

What volume, in liters, of hydrogen gas measured at STP can be produced from 50.0 mL of 6.0 M hydrobromic acid and an excess of zinc metal, according to the following reaction?

Given Zn(s) and AL(s), what observations would you make when combining AL(s) with ZnSO4(aq), and combining Zn(s) with Al(SO4)3(aq)?

Coral structures found in the Great Barrier Reef are composed of calcium carbonate, CaCO3, and are under threat of dissolution due to ocean acidification. Consider the following equilibrium reaction equation. CaCO3(s) + CO2(aq) + H2O(l) ⇌ Ca2+(aq) + 2HCO3–(aq) Write the expression for the equilibrium constant, Kc for this reaction. Predict whether the pH of the ocean will increase or decrease as a result of a decrease in the partial pressure of carbon dioxide in the atmosphere (circle your answer).       Calculate the molar solubility (s) of calcium carbonate in water at 25 °C when    Ksp = 4.5 ´ 10–9.