Solutions and Chemical Reactions

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This is a 6 point assignment

Objectives: After completing this unit, students should be able to:

1. Write equations to show ion formation from electrolytes when they ionize or dissociate.
2. Define and identify substances as strong, weak and non electrolytes.
3. Use solubility rules to predict the water solubility of salts.
4. Knowing the solubility rules, predict whether a precipitation reaction will occur.
5. Write balanced molecular, complete ionic and/or net ionic equations.
6. Differentiate between the terms acid and base, strong acid and weak acid.
7. Identify the common strong acids and bases.
8. Define and identify end point, Stoichiometric point and indicator.
9. Calculate molarity, solution volume, or number of moles of solute, given any two of these quantities.
10. Calculate the concentration of ions present for the solutions of strong electrolytes.
11. Solve problems involving dilution of solutions.
12. Calculate the mass of a substance produced or used in precipitation or neutralization reaction.
13. Given the chemical formula of any atom, ion, or compound listed in the “Formula and Nomenclature” handout, give the name and vice versa.
14. Identify a chemical reaction as dissociation, combination, decomposition, combustion, neutralization, single replacement, double displacement. (See the Chemical Reaction Handout.)
15. Given the reactants and the reaction type (dissociation, combination, decomposition, combustion or neutralization, single replacement, double displacement), predict the products and then balance the equation. (See the Chemical Reaction Handout.)

Reading and Homework Exercises

Table of Contents from: OpenStax Chemistry 2e: Chapter 3 (section 3.3), section 11.2, Chapter 4 (Selected sections, see specific reading recommendations for each link),

Objective 1 Practice – Questions 1 and 2 address ion formation from electrolytes when they ionize or dissociate.  You might find the following reading in OpenStax helpful:

• 4.1 Writing and Balancing Chemical Equations
• 4.2 Classifying Chemical Reactions

Question 1:

Question 2:

Objective 2,3 and 6 Practice – Questions 3-5 give you practice in identifying strong and weak acids, strong and weak bases, and strong, weak, and non electrolytes

Question 3:

Question 4:

Question 5: (Hint: use solubility rules to determine whether salts are strong or weak electrolytes)

Objective 4 and 5 Practice – Questions 6-11  give you practice in predicting the products of precipitation reactions and with molecular, ionic, and net ionic equations

Question 6:

Question 7:

Questions 8 and 9:

Aqueous solutions of iron (III) nitrate and sodium carbonate are mixed and allowed to react.  The reactants are

Fe(NO₃)_{3 (aq)} + Na₂CO_{3 (aq)} →

Question 8:

Question 9:

Questions 10 and 11:

Aqueous solutions of calcium nitrate and sodium iodide are mixed and allowed to react.  The reactants are

Ca(NO₃)_2 (aq) + NaI _(aq) →

Question 10:

Question 11:

Objective 4 and 5 Practice – Questions 12-15  give you practice in predicting the products of acid-base neutralization reactions and with molecular, ionic, and net ionic equations

Questions 12 and 13:

Aqueous solutions of nitrous acid (a weak acid) and potassium hydroxide are mixed and allowed to react.  The reactants are

HNO_2(aq) + KOH _(aq) →

Question 12:

Question 13:

Questions 14 and 15:

Aqueous solutions of nitric acid (a strong acid) and calcium hydroxide are mixed and allowed to react.  The reactants are

HNO_3(aq) + Ca(OH)_{2 (aq)} →

Question 14:

Question 15:

Objective 15 practice for single replacement reactions – Questions 16 and 17 utilize the activity series of metals to predict the products of single replacement reactions.

Question 16:

Mg + AgI→

Question 17:

Cu + Al₂O₃→

Objective 9 Practice – Questions 18-20 provide practice on molarity calculations.  You might find the following reading in OpenStax helpful:

3.3 Molarity

Question 18:

Question 19:

Question 20:

Objective 11 Practice – Questions 21 and 22 provide practice on dilution calculations. 

Question 21:

Question 22:

Objective 10 Practice – Questions 23 and 24 add the concept of concentration of individual ions to the molarity and dilution calculations done earlier. 

Question 23:

Question 24:

Objective 12 Practice – Questions 25 and 26 provide practice with solution stoichiometry problems. You might find the following reading in OpenStax helpful:

• 4.3 Reaction Stoichiometry

Question 25:

Aqueous solutions of silver nitrate and sodium carbonate are mixed and allowed to react.  The reaction is:

2 AgNO_3 (aq) + Na₂CO_{3 (aq)} → Ag₂CO_3 (s) + 2 NaNO_3 (aq)

If 40.0 mL of 0.0235 M silver nitrate solution is added to enough sodium carbonate solution to react with all of the silver nitrate, calculate the mass of precipitate produced.

Question 26:

The neutralization reaction between nitric acid and calcium hydroxide is:

2 HNO₃ + Ca(OH)₂ → Ca(NO₃)₂ + 2 H₂O

Answer the following question: