Chemistry Final 2B – Flashcards

A weak electrolyte exists predominantly as __________ in solution. a. atoms b. ions c. molecules d. electrons e. an isotope

What are the spectator ions in the reaction between KOH (aq) and HNO3 (aq)? a. K+ and H+ b. H+ and OH- c. K+ and NO3- d. H+ and NO3- e. OH- only

The spectator ions in the reaction between aqueous hydrochloric acid and aqueous ammonia are __________. a. H+ and NH3 b. H+, Cl-, NH3, and NH4+ c. Cl- and NH4+ d. H+, Cl-, and NH4+ e. Cl- only

How many moles of Co2+ are present in 0.200 L of a 0.400 M solution of CoI2? a. 2.00 b. 0.500 c. 0.160 d. 0.0800 e. 0.0400

Calculate the concentration (M) of sodium ions in a solution made by diluting 50.0 mL of a 0.874 M solution of sodium sulfide to a total volume of 250.0 mL. a. 0.175 b. 4.37 c. 0.525 d. 0.350 e. 0.874

The molarity of an aqueous solution containing 75.3 g of glucose (C6H12O6) in 35.5 mL of solution is __________. a. 1.85 b. 2.12 c. 0.197 d. 3.52 e. 11.8

With which of the following will the ammonium ion form an insoluble salt? a. chloride b. sulfate c. carbonate d. sulfate and carbonate e. none of the above

With which of the following will the potassium ion form an insoluble salt? a. chloride b. sulfate c. carbonate d. sulfate and carbonate e. none of the above

The net ionic equation for the dissolution of zinc metal in aqueous hydrobromic acid is __________. a. Zn (s) + 2Br- (aq) ZnBr2 (aq) b. Zn (s) + 2HBr (aq) ZnBr2 (aq) + 2H+ (aq) c. Zn (s) + 2HBr (aq) ZnBr2 (s) + 2H+ (aq) d. Zn (s) + 2H+ (aq) Zn2+ (aq) + H2 (g) e. 2Zn (s) + H+ (aq) 2Zn2+ (aq) + H2 (g)

You are given two clear solutions of the same unknown monoprotic acid, but with different concentrations. Which statement is true? a. There is no chemical method designed to tell the two solutions apart. b. It would take more base solution (per milliliter of the unknown solution) to neutralize the more concentrated solution. c. A smaller volume of the less concentrated solution contains the same number of moles of the acid compared to the more concentrated solution. d. If the same volume of each sample was taken, then more base solution would be required to neutralize the one with lower concentration. e. The product of concentration and volume of the less concentrated solution equals the product of concentration and volume of the more concentrated solution.

A 0.100 M solution of __________ will contain the highest concentration of potassium ions. a. potassium phosphate b. potassium hydrogen carbonate c. potassium hypochlorite d. potassium iodide e. potassium oxide

What volume (mL) of a concentrated solution of sodium hydroxide (6.00 M) must be diluted to 200.0 mL to make a 0.880 M solution of sodium hydroxide? a. 2.64 b. 176 c. 26.4 d. 29.3 e. 50.0

What volume (L) of 0.250 M HNO3 is required to neutralize a solution prepared by dissolving 17.5 g of NaOH in 350 mL of water? a. 50.0 b. 0.44 c. 1.75 d. 0.070 e. 1.75 10-3

The point in a titration at which the indicator changes is called the __________. a. setpoint b. indicator point c. standard point d. endpoint e. volumetric point

__________ is an oxidation reaction. a. Ice melting in a soft drink b. Table salt dissolving in water for cooking vegetables c. Rusting of iron d. The reaction of sodium chloride with lead nitrate to form lead chloride and sodium nitrate e. Neutralization of HCl by NaOH

Pure acetic acid (HC2H3O2) is a liquid and is known as glacial acetic acid. Calculate the molarity of a solution prepared by dissolving 10.00 mL of glacial acetic acid at 25°C in sufficient water to give 500.0 mL of solution. The density of glacial acetic acid at 25°C is 1.05 g/mL. a. 1.26 x 10^3 b. 21.0 c. 0.0210 d. 0.350 e. 3.50 x 10^-4

The value of H° for the reaction below is -790 kJ. The enthalpy change accompanying the reaction of 0.95 g of S is __________ kJ. 2S (s) + 3O2 (g) 2SO3 (g) a. 23 b. -23 c. -12 d. 12 e. -790

Given the following reactions N2 (g) + O2 (g) 2NO (g) H = +180.7 kJ 2NO (g) + O2 (g) 2NO2 (g) H = -113.1 kJ the enthalpy of reaction for 4NO (g) 2NO2 (g) + N2 (g) is __________ kJ. a. 67.6 b. 45.5 c. -293.8 d. -45.5 e. 293.8

The value of H° for the following reaction is 177.8 kJ. The value of H°f for CaO(s) is __________ kJ/mol. CaCO3 (s) CaO (s) + CO2 (g) a. -1600 b. -813.4 c. -635.5 d. 813.4 e. 177.8

The average fuel value of sugars is 17 kJ/g. A 2.0 L pitcher of sweetened Kool-Aid contains 400 g of sugar. What is the fuel value (in kJ) of a 500 mL serving of Kool-Aid? (Assume that the sugar is the only fuel source.) a. 4.2 x 10^4 b. 1.7 x 10^3 c. 1.7 x 10^6 d. 1.7 x 10^2 e. 17

A 5.00-g sample of liquid water at 25.0 C is heated by the addition of 84.0 J of energy. The final temperature of the water is __________ °C. The specific heat capacity of liquid water is a. 95.2 b. 25.2 c. -21.0 d. 29.0 e. 4.02

A gas vessel is attached to an open-end manometer containing a nonvolatile liquid of density 0.791 g/mL as shown below. The difference in heights of the liquid in the two sides of the manometer is 43.4 cm when the atmospheric pressure is 755 mm Hg. Given that the density of mercury is 13.6 g/mL, the pressure of the enclosed gas is __________ atm. a. 1.03 b. 0.960 c. 0.993 d. 0.990 e. 0.987

A gas vessel is attached to an open-end manometer filled with a nonvolatile liquid of density 0.993 g/mL as shown below. The difference in heights of the liquid in the two sides of the manometer is 32.3 cm when the atmospheric pressure is 765 mm Hg. Given that the density of mercury is 13.6 g/mL, the pressure of the enclosed gas is __________ atm. a. 1.04 b. 1.01 c. 0.976 d. 0.993 e. 1.08

A sample of N2 gas (2.0 mmol) effused through a pinhole in 5.5 s. It will take __________ s for the same amount of CH4 to effuse under the same conditions. a. 7.3 b. 5.5 c. 3.1 d. 4.2 e. 9.6

Of the following, only __________ is impossible for an ideal gas. a. V1/T1=V2/T2 b. V1T1 = V2T2 c. V1/V2=T1/T2 d. V2=T2/T1(V1) e. V1/V2=T1/T2=0

Of the following gases, __________ has density of 2.104 g/L at 303 K and 1.31 atm. a. He b. Ne c. Ar d. Kr e. Xe

Which of the following is not part of the kinetic-molecular theory? a. Atoms are neither created nor destroyed by ordinary chemical reactions. b. Attractive and repulsive forces between gas molecules are negligible. c. Gases consist of molecules in continuous, random motion. d. Collisions between gas molecules do not result in the loss of energy. e. The volume occupied by all of the gas molecules in a container is negligible compared to the volume of the container.

Of the following gases, __________ will have the greatest rate of effusion at a given temperature. a. NH3 b. CH4 c. Ar d. HBr e. HCl

How much faster does 235UF6 effuse than 238UF6? a. 1.013 times as fast b. 1.009 times as fast c. 1.004 times as fast d. 1.006 times as fast e. 1.018 times as fast

A 1.44-g sample of an unknown pure gas occupies a volume of 0.335 L at a pressure of 1.00 atm and a temperature of 100.0°C. The unknown gas is __________. a. argon b. helium c. krypton d. neon e. xenon