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Equilibrium and acid/base chemistry (Modules 5 and 6) quiz

12questions. Pick an answer and you'll see why right away.

  1. A reaction at equilibrium has Q = K. What happens next?

  2. For N2(g) + 3H2(g) goes to 2NH3(g), increasing pressure at constant temperature will:

  3. Which is the correct Bronsted-Lowry definition?

  4. A 0.10 mol/L solution of a strong monoprotic acid has pH:

  5. The conjugate base of HCO3- (hydrogen carbonate) is:

  6. Buffer solutions resist pH change because they contain:

  7. In a titration of a strong acid with a strong base, the equivalence point pH is:

  8. Indicators change colour over a pH range because:

  9. A reaction with K = 1 x 10^10 is best described as:

  10. Adding a catalyst to an equilibrium system:

  11. Increasing temperature for an exothermic forward reaction will:

  12. Which statement BEST opens a Module 6 extended response on buffers in blood?