Honors Unit 4 Homework Packet

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1 1 Honors Homework Packet Reactions in Aqueous Solutions Part I: Aqueous Solns. Part II: Acid/Base Chemistry Part III: Redox Reactions Name:

2 2 Molarity of Solutions (pg. 2 & 3) Directions: Solve each of the following problems. Show your work and include units!! 1. Calculate the molarity of the following solutions. a. 12 g of lithium hydroxide (LiOH) in 1.0 L of solution b. 198 g of barium bromide (BaBr2) in 2.0 L of solution c. 54 g of calcium sulfide (CaS) in 3.0 L of solution 2. Calculate the volume of each solution, in liters. a. a 1.0 M solution containing 85 g of silver nitrate (AgNO3) b. a 0.5 M solution containing 250 g of manganese (II) chloride (MnCl2) GO ON TO THE NEXT PAGE

3 3 3. How many grams of potassium chloride (KCl) are required to make 2.0 L of a 3.0 M solution? 4. How many grams of magnesium chloride (MgCl2) are needed to make 6.0 L of a 3.0 M solution? 5. What mass of barium chloride (BaCl2) is needed to make 0.5 L of a 4.0 M solution? 6. What is the molarity of a solution in which 1.6 g of sodium hydroxide (NaOH) are dissolved in 125 ml of solution? 7. What is the molarity of a solution in which 5.0 g of sodium carbonate (Na2CO3) are dissolved in 200 ml of solution?

4 4 Strong Electrolytes: Equation Writing Practice Directions: For each of the electrolytes listed below, write the ionization or disassociation equation. Part I. Ionic Compounds 1. KCl(aq) 2. Cu(NO2)2 (aq) 3. Zn3(PO4)2 (aq) 4. Fe(ClO3)3 (aq) Part II. Strong Acids 1, HCl (aq) 2. HBr(aq) 3. HI (aq) 4. HClO4 (aq) 5. HNO3 (aq) Part III. Strong Bases 1. NaOH (aq) 2. KOH (aq) 3. Ba(OH)2 4. Ca(OH)2

5 5 Net Ionic Equations: Equation Writing Write the full ionic equation and net ionic equations for the following reactions. If the equation is not balanced, you MUST balance it first! 1. Pb(NO3)2 (aq) + 2 KCl (aq) PbCl2 (s) + 2 KNO3 (aq) Complete Ionic: Net Ionic: 2. NaOH (aq) + CuCl2 (aq) NaCl (aq) + Cu(OH)2 (s) Complete Ionic: Net Ionic: 3. NiClO3 (aq) + K3PO4 (aq) Ni3PO4 (s) + KClO3(aq) Complete Ionic: Net Ionic: 4. K2SO4 (aq) + Ba(NO3)2 (aq) BaSO4 (s) + KNO3 (aq) Complete Ionic: Net Ionic:

6 6 Predicting Precipitates & Net Ionic Equations Directions: Predict the products for each reaction. Next, write a complete balanced equation. Finally, write the full ionic equation and net ionic equation. 1. magnesium nitrate + potassium phosphate 2. sodium chromate + iron (II) nitrate 3. barium acetate + ammonium sulfate 4. sodium hydroxide + iron (III) nitrate 5. sodium iodide + lead (II) nitrate

7 7 Bronsted-Lowry Acids and Bases Part A. Directions: For the following reactions, label each reactant as either an acid or base according to the Bronsted-Lowry definitions. Next, label each product as either a conjugate acid or a conjugate base. 1. NH3(aq) + HC2H3O2(aq) NH4 + (aq) + C2H3O2 - (aq) 2. H2O(l) + HC2H3O2(aq) H3O + (aq) + C2H3O2 - (aq) 3. NH3(aq) + H2O(l) NH4 + (aq) + OH - (aq) 4. HC2H3O2(aq) + H2PO4 - (aq) C2H3O2 - (aq) + H3PO4(aq) Part B. Directions: For the following reactants, complete the reaction by donating a proton from the acid to the base. Then, label all the reactants and products as in Part A. 4. HCl (aq) + NH3 (l) 5. HF (aq) + H2O (l) 6. HS - (aq) + OH - (aq) Part C. Write the formulas as indicated below. Conjugate Acids: Write the formula for the conjugate acid of: (a) F - (c) HSO4 - (b) NH3 (d) CrO4 2 - Conjugate Bases: Write the formula for the conjugate base of: (a) HClO3 (c) H2O (b) H2SO3 (d) HCO3 -

8 8 ph Calculations Utilize the ph box and the ph equations we talked about in class to perform the following calculations. 1. Find [H3O + ] for a solution with an [OH - ] of M. 2. What is the ph of a solution that has an [H + ] of 6.6 x 10-4 M? 3. What is the poh of a solution that has a ph of 4.50? Is this solution acidic or basic? 4. A solution of HNO3 has a ph of 4.5. Calculate the [H3O + ], [OH - ] and poh. ph = poh = [H + ] = [OH - ] = Is this solution acidic or basic? 5. What is the [H3O + ], [OH - ] and poh in a solution that has a ph of 10.0? ph = poh = [H + ] = [OH - ] = Is this solution acidic or basic?

9 9 Titration Problems Directions: First write the balanced neutralization reaction occurring between the acid and base. Then, solve the problems. Report your answers to the correct number of sig. figs. and with the correct units. 1. If it takes ml of M NaOH to neutralize ml of HCl, what is the molarity of the acid? 2. If it takes ml of M HNO3 to neutralize 345 ml of LiOH, what is the concentration of the base? 3. If it takes ml of 0.50 M KOH to neutralize ml of H2SO4, what is the concentration of the acid? 4. A student titrates an unknown solution of Ca(OH)2 in the laboratory with a standard solution of 1.5 M HCl. and obtains the following data. STANDARD SOLUTION (1.5 M HCl) UNKNOWN SOLUTION (Ca(OH)2) Starting buret reading: ml 0.00 ml Ending buret reading: ml ml Calculate the molarity of the unknown solution.

10 10 Oxidation Number & Oxidation/Reduction (pg. 10 & 11) For each of the following substances, determine the oxidation states of each element in the formula. EXAMPLE: 1) sodium nitrate NaNO3 Na= +1 O= -2 therefore N = +5 2) ammonia (NH3) 3) zinc oxide (ZnO) 4) water (H2O) 5) calcium hydroxide (Ca(OH)2) 6) carbon dioxide (CO2) 7) nitrogen (N2) 8) sodium sulfate(na2so4) 9) aluminum hydroxide (Al(OH)3) 10) magnesium phosphate (Mg3(PO4)2) In each of the following reactions, determine what was oxidized and what was reduced. 11) Ca + H 2 O CaO + H 2 Element oxidized: 12) 2 H 2 + O 2 2 H 2 O Element oxidized: GO ON TO THE NEXT PAGE Dr. Mihelcic 10

11 11 In each of the following reactions, determine which element was oxidized and which was reduced. 1) Na + FeCl2 NaCl + Fe Element oxidized: 2) Mn 2+ + SbO4 1- Sb 3+ + MnO4 1- Element oxidized: 3) Cr2O Sn 2+ Cr 3+ + Sn 4+ Element oxidized: 4) Ag(s) + NO 3 (s) Ag + (s) + NO Element oxidized: 5) Cu 2+ + Ce 3+ CeO2 + Cu Element oxidized: 6) P + Cu 2+ Cu + H2PO4 - Element oxidized: Dr. Mihelcic 11

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