Given the following substances, listed in order of increasing acid strength, HOCl(aq) < HC2H3O2(aq) < HC2O4-(aq) < HOCN(aq) < HNO2(aq) < HCl(aq) Which species listed below is the strongest base?

For the reaction, 2SO2(g) + O2(g) 2SO3(g), at 900.0 K the equilibrium constant, Kc, has a value of 13.0. Calculate the value of Kp at the same temperature.

A mixture is made by adding 50.0 mL of 0.20 M NaOH(aq) to 50.0 mL of water. At 25.0 °C, what is its pH?

The pH of a solution is measured to be 10.40. What are the values of [H3O+] and [OH−] for this solution?

The conjugate base of H2SO4 is

The reaction, 2NO(g) + O2(g) → 2NO2(g), was found to be first order in each of the two reactants and second order overall. The rate law is, therefore:

A solution is made by dissolving 0.840 moles of sodium hydroxide in 300.0 g of water. If the van’t Hoff factor, i, for this particular concentration is 1.70, what is the expected freezing point of this solution? Kf = 1.86 °C m−1.

Given the two reactions shown with their equilibrium constants, PCl3(g) + Cl2(g) PCl5(g)K12 NO(g) + Cl2(g) 2 NOCl(g)K2What is the equilibrium constant for the reaction, PCl5(g) + 2 NO(g) PCl3(g) + 2 NOCl(g)

The reaction, NO2Cl(g) + Cl(g) → NO2(g) + Cl2(g), was found to be first order in each of the two reactants and second order overall. The rate law is, therefore:

For the reaction, 2SO2(g) + O2(g) 2SO3(g), at 450.0 K the equilibrium constant, Kc, has a value of 4.62. A system was charged to give these initial concentrations: [SO3] = 0.500 M, [O2] = 0.00855 M, [SO2] = 0.254 M. In which direction will it go?Hint: Find the value for Q and then compare that value to the given value for Kc