(use SF, units; show all work)
#. a: Acetic acid (HC2H3O2) is a weak electrolyte. What substances are present in HC2H3O2 (aq)?
b: Chloric acid (HClO3) is a strong electrolyte. What substances are present in HClO3 (aq)?
#. Identify each of the following substances as a strong electrolyte, weak electrolyte, or nonelectrolyte:
a. C6H12O6 (glucose) b: HF
c. HI d. H2O2
e. LiNO3
#. Give the Arrhenius and Bronsted definitions of acids and bases.
Why are the Bronsted definitions more useful?
#. a: Write the molecular and net ionic versions of the reaction of aluminum bromide and
mercury (II) nitrate. You must include the states!
b: Which substance in the above reaction is a precipitate? What are the spectator ions?
#. a: Write the molecular and net ionic versions of the reaction of hydroiodic acid and
calcium hydroxide. You must include the states!
b: Which substance in the above reaction is a precipitate? What are the spectator ions?
#. Identify each of the following species as a Bronsted acid, Bronsted base, or both:
a. F1- b. HAsO42-
c. HCO31- d. HNO
#. Is it possible to have a reaction in which oxidation occurs and reduction does not? Explain.
#. Use the metal activity series in your textbook to answer this question. (Page 118 of Chang
7th Ed.) Which of the following single displacement reactions can occur? For any
reactions that can occur determine the products and balance the reaction. For any
reactions that cannot occur write NR.
a. Au + KCl è
b. Mg + CoCl2 è
c. Ba + AlBr3 è
d. Sn + ZnI2 è
#. Use the halogen displacement series in your textbook to answer this question. (Page 118 of
Chang 7th Ed.) Which of the following single displacement reactions can occur? For any
reactions that can occur determine the products and balance the reaction. For any
reactions that cannot occur write NR.
a. Br2 + KCl è
b. F2 + CoCl2 è
c. I2 + AlBr3 è
d. Cl2 + AgI è
#. Give the oxidation number of the underlined atoms in the following molecules and ions:
a. IF
b. BrF5
c. PH3
d. C2H6
e. C4H4
f. LiMnO3
g. Cr2O7 2-
h. KClO4
i. KHCO3
j. O3
k. AsF41+
l. CaRuCl6
11. Give the oxidation number of the underlined atoms in the following molecules and ions:
a. NaBrO2
b. Cs3P
c. Be(IO3)2
d. B2S3
e. K3PO2
f. ZrSe2
g. MoO42-
h. PdN22-
i. PtCl82-
j. SnF4
k. BF3
l. BiF61-
12. Label the following compounds (aq) if they are soluble in water, and (s) if insoluble.
a. K2SO4 b. Hg2Cl2
c. SrS d. NiBr5
e. (NH4)3PO4 f. PbCO3
g. Ru(OH)4 h. AgC2H3O2
13. Using the redox method and showing all work, balance the following reactions.
(Determine the oxidation states, write the half-reactions, label each half reaction
red. or ox., and balance the reaction.)
a: Al3+ + Cr2+ è Al + Cr6+
b: Zn + Mn2S7 è MnS + ZnS
c: B2F4 + AsF5 è BF3 + As2F2
14. For each of the redox reactions in problem #13, determine which substance is the oxidizer/oxidizing agent and which substance is the reducer/reducing agent.
a. oxidizer reducer
b. oxidizer reducer
c. oxidizer reducer
15. Calculate the molarity of each of the following solutions:
a. 19.28 g of hydrazine (N2H4) in 3.50 x 102 mL of aqueous solution
b. 1.28 g of aluminum chloride (AlCl3) in 4.30 x 102 mL of aqueous solution
c. 882 mg of 1-heptyne (C7H10) in 0.692 ml of solution in benzene (C6H6)
16. a. How many grams of rubidium fluoride are there in 350. mL of 0.200 M solution?
b. How many mL of 2.166 M Na2CO3 solution would contain 0.400 mole of
sodium carbonate?
17. How many grams of CoCl2*6 H2O would you need to dissolve in a 250.0 mL volumetric flask
to make a solution that has a concentration of chloride ions of 0.2300M?
(Hint: You can either balance an equation or use internal stoichiometry.)
18. a: Write the balanced equation for neutralizing H3PO4 with Ba(OH)2.
b: How many liters of 0.400 M H3PO4 would you need to neutralize
10.0 mL of 1.200 M Ba(OH)2?
19. Using the same reaction from problem #18, how many grams of precipitate could you make
if you reacted 286.0 mL of 3.000 M H3PO4 with 855.0 mL of 1.400 M Ba(OH)2?
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