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Equilibrium Chapter Exam

Exam Instructions:

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Question 1 1. Titrations are used to analyze properties of an unknown solution. In a titration, the equivalence point is the point at which _____ have been added together to create a neutral solution. 

Question 2 2. The equilibrium constant is a value that relates the ratio of the concentrations of _____ once the reaction has reached chemical equilibrium.

Question 3 3.

The reaction below is exothermic. Which of the following will occur if the temperature increases?

A(g) + B(g) ---- C(g) + D(g)

Question 4 4. The _____ is useful in determining the direction in which the reaction is moving toward or away from chemical equilibrium.

Question 5 5. Which of the following is true about buffers?

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Question 6 6. In which of the following scenarios will a precipitate form?

Question 7 7.

What is the equilibrium constant for the reaction when 0.1908 moles of CO2 react with 0.0908 moles of H2 to produce 0.0092 moles of CO and 0.0092 moles of H2O?

CO2 + H2 -- > CO + H2O

Question 8 8.

In the reaction below, which of the following occurs after the pressure is increased?

A(g) + B(g) ---- 2C(g) + D(g)

Question 9 9. Which of the following compounds is the least soluble given the Ksp values?

Question 10 10.

Calculate the concentration of calcium in a solution of calcium fluoride (CaF2) in pure water:

Ksp = 1.46 x 10^-10

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Question 11 11.

Consider the following reaction:

2 NH3(g)   N2(g) + 3 H2(g)    Kc = 0.0076

If 3.00 moles NH3 react to produce 2.00 moles of N2, and 5.00 moles of H2, in a 5.00 L container, what is the equilibrium concentration for each species present in the equilibrium mixture?

Question 12 12. The common ion effect states that the addition of an ion common to two solutes causes _____.

Question 13 13. Which of the following affects the equilibrium of a chemical reaction?

Question 14 14. What is the concentration of tin (Sn) in a solution of tin(II) hydroxide (Sn(OH)2) in pure water? Ksp = 5.45 x 10^-27?

Question 15 15. The concentration of H ions in a solution can be used to calculate its:

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Question 16 16. A certain amount of Sodium hydroxide (NaOH) is dissolved in water. If the product of Na+ and OH- is equal to the Ksp for NaOH, what does this tell us about the solution?

Question 17 17. When are there more ions in the solution than in equilibrium?

Question 18 18. When a solution of a given volume has a maximum amount of a solid dissolved in it, it is said to be _____.

Question 19 19.

In the reaction below, what will happen if you decrease the concentration of A?

A + B ---- C + D

Question 20 20. The ability of a solid to be dissolved in a given volume of a solvent at a given temperature is known as _____.

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Question 21 21. What is the pH of a 1.34 M solution of hydrofluoric acid (HF) with a Ka of 3.55 × 10^-4?

Question 22 22. In chemistry, what does Le Chatelier's principle explains about an equilibrium?

Question 23 23. Which of the following is true about chemical equilibrium?

Equilibrium Chapter Exam Instructions

Choose your answers to the questions and click 'Next' to see the next question. You can skip questions if you would like and come back to them later with the "Go To First Skipped Question" button. When you have completed the practice exam, a green submit button will appear. Click it to see your results. You will lose your work if you close or refresh this page. Good luck!

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