Given the following reaction:

Consider the following equilibrium reaction:

H₂CO₃ (aq)  ⇌  H⁺ (aq) + HCO₃^– (aq);     K = 5.0 x 10^–7

 If the initial concentrations of the species are:

[H₂CO₃] = 0.010 M;   [H⁺] = 1.2 x 10^–5 M;   [HCO₃^–] = 4.0 x 10^–3 M

Which one of the statements below describes the relationship between Q and K and then the correct direction of chemical change?

Of the following equilibria, only ________ will shift to the right in response to a decrease in volume.

The magnitude of the equilibrium constant, K, for a given reaction depends on:

At elevated temperatures, molecular hydrogen and molecular bromine react to partially form hydrogen bromide:

For the equilibrium reaction below K = 0.112.

SO₂ (g) + ½O₂ (g) ⇌ SO₃ (g)

In the acid-base titration part of this experiment you will be provided with an unknown acid or base. How do you determine if the unknown is an acid or a base?

In the acid-base titration part of this experiment you will be adding a standardised acid or base from a burette to the solution you are measuring the pH of using a pH meter. At the start of the titration you add the solution from the burette in 2.0 mL portions. How do you tell that you should add smaller (0.5 mL) portions for a part of the titration?

What is the pH of a buffer solution containing 1.29 mol/L ammonium chloride and 0.86 mol/L ammonia? 

pK_a (NH₄⁺) = 9.24

Which of the following best describes the pH values at points A, B, and C on this titration curve?