Blog

Calculate the concentration of H+(aq) in a solution in which [OH-] is 0.010 M.

A solution contains three anions with the following concentrations: 0.20 M CrO42–, 0.10 M CO32–, and 0.010 M Cl–. If a dilute AgNO3 solution is slowly added to the solution, what is the first compound to precipitate: Ag2CrO4 (Ksp = 1.2 × 10–12), Ag2CO3 (Ksp = 8.1 × 10–12), or AgCl (Ksp = 1.8 × 10–10)?

For a saturated solution of Co(OH)2, what happens when a strong acid is added?

The first-order decomposition of N2O5 was studied at a particular temperature and found to have a rate constant of 6.2 x 10-4s-1. What is the half-life for the decomposition under these conditions?

Identify the Brønsted-Lowry base in the following reaction, (CH3)3N(aq) + H2O(l) → (CH3)3NH+(aq) + OH-(aq).

Which statement is true for the following reaction, NH3(aq) + H2O(l) → NH4+(aq) + OH-(aq)?

Arrhenius defines an acid as

Consider the following hypothetical aqueous reaction: A(aq) → B(aq). A flask is charged with 0.065 mol of A in a total volume of 100.0 mL. The following data are collected. Calculate the average rate of appearance for B in units of M/s between 20 and 40 minutes. Time (min) 0 10 20 30 40 Moles of A 0.065 0.051 0.042 0.036 0.031

The decomposition reaction of N2O5 in carbon tetrachloride is 2 N2O5 → 4 NO2 + O2. The rate law is first order in N2O5. At 64 °C the rate constant is 4.82 × 10–3 s–1. What is the rate of reaction when [N2O5] = 0.0240 M?

A reaction involves 2 different reactants and both reactants are first order. How does the rate change if the concentration of both reactants is doubled?