2 Question 1 Which of the following are generally considered to be nonelectrolytes? A) Soluble ionic compoundsB) Strong acidsC) Weak acidsD) None of the above
3 Question 2 Which of the following are generally considered to be strong electrolytes? A) Strong acidsB) Soluble ionic compoundsC) Weak acidsD) Both A and B
4 Question 3 Compounds containing the nitrate ions are generally soluble with the exception of silver nitrate.A) TrueB) False
5 Question 4 Compounds containing the ammonium ion are generally soluble. A) TrueB) False
6 Question 5 A precipitate will form when a solution of silver nitrate is mixed with a solution of sodium bromide.A) TrueB) False
7 Question 6 Mixing which of the following pairs of substances in aqueous solution will result in a precipitate being formed?A) sodium nitrate and ammonium bromideB) sodium hydroxide and hydrochloric acidC) calcium chloride and sodium carbonateD) All of the above
8 Question 7 Which of the following types of substances should be represented as separated ions in an ionic equation?A) Insoluble ionic compoundsB) Weak acids and basesC) WaterD) Strong acids or soluble ionic compounds (strong electrolytes)
9 Question 8 Which of the following "rules" for assigning oxidation numbers is incorrect? A) The oxidation number of an elemental substance is determined by its group number.B) The oxidation numbers of the atoms in a polyatomic ion add up to zero.C) In an ionic compound, the oxidation number is equal to the subscript in the compound formula.D) All of the above are incorrect.
10 Question 9 If mol of ethanol liquid (volume around 100 mL) is mixed with L of water, the solution will be M in ethanol.A) TrueB) False
11 Question 10 How many mL of 2.0 M hydrochloric acid would be required to prepare mL of 1.0 M HCl?A) 50.0 mLB) mLC) mLD) Depends on how much of the 2.0 M hydrochloric acid you have available
12 Question 11 When calcium carbonate is placed in water, which of the following best describes what is present in the mixture?A) calcium carbonate molecules onlyB) calcium ions and carbonate ions onlyC) mostly calcium ions and carbonate ions and little undissociated calcium carbonateD) a few calcium ions and carbonate ions and a lot of undissociated calcium carbonateE) hydrated calcium and carbonate ions only
13 Question 12 Ammonium sulfide and mercuric bicarbonate are expected to be A) both soluble.B) soluble and insoluble.C) insoluble and soluble.D) both insoluble.
14 Question 13 Which of the following salts is expected to be soluble? A) Silver chlorideB) Mercuric sulfateC) Silver chlorateD) Barium sulfateE) Lead iodide
15 Question 14 The equation Fe3+(aq) + 3OH-(aq) → Fe(OH)3 represents A) a balanced molecular equation.B) a balanced ionic equation.C) a balanced net ionic equation.D) a dissociation reaction.E) an example of a redox reaction.
16 Question 15 Which of the following is not an acid/conjugated base pair? A) sulfuric acid / sulfate ionB) ammonia / ammonium ionC) water / hydroxide ionD) phosphoric acid / dihydrogen phosphate ionE) dihydrogen phosphate ion / hydrogen phosphate ion
17 Question 16 Which of the following species should be considered a weak Bronsted acid? A) HIB) OH-C) HNO3D) HClO4E) None of the above
18 Question 17 Which of the following species is not amphoteric? A) Al2O3B) H2OC) H2PO4-D) HPO42-E) PO43-
19 Question 18 In which of the following species is the oxidation number of manganese highest? A) MnO2B) Mn2(SO4)3C) K2MnO4D) KMnO4E) MnO3
20 Question 19 Which of the following equations does not represent a redox reaction? A) Cu + 2AgNO3 → 2Ag + Cu(NO3)2B) 2CrO H+ → Cr2O72- + H2OC) 2SO2 + O2 → 2SO3D) 2H2 + O2 → 2H2OE) All are redox
21 Question 20 A sample of oxalic acid (a diprotic acid of the formula H2C2O4) is dissolved in enough water to make 1.00 L of solution. A mL sample of this solution is titrated with a solution of sodium hydroxide of concentration M and requires 20.0 mL of sodium hydroxide to reach the end point. Calculate the mass of the original oxalic acid sample.A) 6.75 gB) gC) 1.35 gD) 13.5 gE) None of the above
22 23. 48mL of a NaOH solution are needed to neutralize 0 23.48mL of a NaOH solution are needed to neutralize g of KHP (MW g/mol). What is the concentration of the base solution?0.1141MM1.14MCan’t tell