Solutions Questions and Answers

Add a small pinch of crushed calcium carbonate to each of two test tubes. Put about 2 mL (2 squirts) of 1 M acetic acid, HC₂H3O2, into each test tube. Set one test tube in a beaker without stirring, and stir the other by tapping the side of the test tube to swirl its contents for one minute. Compare the rate of reaction in the two test tubes. Did one "dissolve" faster? Using two test tubes, add a very small pinch of yeast to only ONE. Add about 2 mL of hydrogen peroxide to each of the two test tubes. Compare the rate of bubbling due to the decomposition of the hydrogen peroxide. Yeast may catalyze this reaction.

What does the "2M" in 2M NaHCO3 tell us? * A) It describes the concentration of the solution that was made from solid NaHCO3 and water. B) It suggests that there are 0.75 moles of NaHCO3 in 0.50 liters of the solution. C) It expresses the number of moles of NaHCO3 dissolved in every liter of solution. D) Answers A and C are both correct. E) Answers A, B, and C are all correct.

QUESTION: What do the following reactants produce? Why? Al + Br₂ → [Reaction: 2Al + Br₂ 2A1Br ] Aluminum bromide is AlBr because the charge of Al+³ cancels the charge of Br-¹. [Reaction: 2Al + 3Br₂ → 2AIBr3] Aluminum bromide is AlBr, because the charge of Al+3 cancels the charge of 3Br-¹. [Reaction: Al + Br₂ AlBr₂] Aluminum bromide is AlBr₂ because the charge of Al+³ cancels the charge of 2Br-¹. [Reaction: 2Al + 3Br₂2 2AIBr3] Aluminum bromide is AlBr, because the charge of Al+3 cancels the charge of 3Br-².

What distinguishes a saturated solution from a supersaturated solution? A. A saturated solution contains more solute than is theoretically possible at a given temperature. B. A supersaturated solution contains more solute than is theoretically possible at a given temperature. C. A supersaturated solution contains less than the maximum amount of solute that is possible at a given temperature. D. A saturated solution contains more solute than the same volume of supersaturated solution at the same temperature.

What will happen to the ability of a gas to dissolve in a liquid if the temperature increases? F. Solubility of the gas is not affected G. Solubility of the gas increases or decreases H. Solubility of the gas decreases J. Solubility of the gas increases

I. A student calculated the molarity of a solution prepared by dissolving 0.730 mol of table sugar (sucrose, C12H22011) in 1.8x10^3 mL of water as 4.06x10^-4cMC12H22011. Explain the student's calculation error and explain how the studentcshould solve for the correct value of molarity. Show a valid calculation for the molarity. II. The student then takes a 1.00 M stock solution of table sugar (sucrose, C12H22011) and mixes 0.305 L of stock solution with additional distilled water to create a dilute solution with a total volume of 1.25 L. Explain how the student can determine the molarity of the resulting solution. Show a valid calculation for the final molarity.

The rare earth metal terbium is produced from terbium (III) sulfate and calcium metal by the following single replacement reaction: Tb2(SO4)3+2Ca →Ca₂ (SO4)3+2 Tb Given 27.5 g of Tb2(SO4)3, how many grams of terbium could be produced?

Which of the following will speed up the dissolving of a solid solute in water? All of the above. Heat the solution. Stir the solution Grind the solute.

To prepare a lab solution a chemist dissolves solid potassium chloride in a given amount of water until no more will dissolve at that temperature. How could that solution be described? A. The solution is saturated; it is a concentrated solution. B. The solution is unsaturated; it is a dilute solution. C. The solution is supersaturated; it is a concentrated solution. D. The solution is aqueous; it is a dilute solution.

A 41.0-mL barium hydroxide solution of molarity 2.39 M is diluted with water to form 76.70 mL of the solution. Calculate the molarity of the solution. Do not include units in your answer. Round to the tenths place or further.

The concentration of a liquid solution can be expressed in terms of the percentage by volume of the solute. True False

Imagine you have two beakers. Both beakers are filled with the same amount of water. The water in both beakers is the same temperature as well. You add 50 g of Substance A to the first beaker, and 50 g of Substance B to the second beaker. After stirring both beakers, there is a small pile of Substance A at the bottom of the first beaker. None of Substance B is visible in the second beaker. Which of the following statements is true? Substance A is less soluble in water than Substance B. Substance A is more soluble in water than Substance B. Substance A is not soluble in water. Substance B is not soluble in water.

Brass used in musical instruments is 80 percent copper and 20 percent zinc. brass is the solute zinc is the solvent copper is the solvent brass is the solvent

A 31.58-mL barium hydroxide solution of molarity 4.71 M is diluted with water to form 182.03 mL of the solution. Calculate the molarity of the diluted solution. Do not include units in your answer. Round to the tenths place or further.

Calculate the mass in grams of nitric acid dissolved in 0.48 kg of water if the molality of the solution is 1.53 m. The molar mass of nitric acid is 63 g/mol. Do not include units in your answer. Round to the tenths place or further.

You find that a given solution is saturated. Which of the choices below would allow you to dissolve a greater amount of solute? A. increasing the amount of agitation in the solvent B. decreasing the amount of solvent C. increasing the temperature of the solvent D. decreasing the particle size of the solute

Potassium nitrate absorbs a large amount of heat energy from the water as it dissolves. How does this explain the solubility curve you graphed for potassium nitrate?

The solubility of nitrogen gas at 25 °C and 1 atm is 6.8 x 10-4 mol/L. If the partial pressure of nitrogen gas in air is 0.76 atm, what is the concentration (Molarity) of dissolved nitrogen? A) 6.8 × 10-4M B) 5.2 × 10-4M C) 4.9 × 10-4M D) 3.8 × 10-4M E) 1.1 x 10-5M

20.Colligative properties of solutions include all of the following except A) depression of vapor pressure upon addition of a solute to a solvent B) elevation of the boiling point of a solution upon addition of a solute to a solvent C) depression of the freezing point of a solution upon addition of a solute to a solvent D) an increase in the osmotic pressure of a solution upon the addition of more solute E) the increase of reaction rates with increase in temperature

13. The freezing point of an aqueous solution that contains 25.0 g of CaCl₂ in 100.0 g of water is ________°C. (Given; K, for water = 1.86°C/m) A.-13.8°C B.4°C C.-12.6°C D.-4°C E.12.5°C

Determine the volume of solution (in mL) that must be added to a calibrated burette to mix the following IV drug. The medication volume is included in the total dilution volume. Calculate the flow rate in gtt/min for each infusion. A microdrip with a calibration of 60 gtt/mL is used. (Simplify your answers completely. Express your answers to the nearest whole number.) An IV antibiotic of 750 mg in 3 mL has been ordered diluted to a total of 35 mL of D5W to infuse in 40 minutes.

If 40 g of sodium chloride (NaCl) will dissolve in 100 g of water at 80°C, how many grams of NaCl will dissolve in 50 g of water at the same temperature?

When the following equation H₂S + Cr₂O7²- -> S + Cr3+ (acidic sol'n) is balanced, and the stoichiometric coefficients are reduced to their lowest integer values the coefficients of H+ and H₂are respectively. a. 9, 8 b.4, 3 c. 8, 7 d. none of the other answers are correct e. 7, 6

Determine the pH of a buffer that is 0.95 M HBrO and 0.68 M KBrO. The value of pKa for HBrO is 8.68. Based on the given values, set up ICE table in order to determine the unknown. HBrO (aq) + H₂O(l) H3O+ (aq) + BrO- (aq) Initial (M) Change (M) Equilibrium (M)

A bullet jacket is made of 95% copper and 5% zinc. Which is the solute? A solution of silver nitrate is used to develop fingerprints on porous objects such as wood. To make the solution, 30.0 grams of silver nitrate is dissolved in 1.00 liter of water. Which is the solvent? Air is a mixture composed of approximately 78% nitrogen, 21% oxygen, with the remainder being several other gases. Which is(are) the solute?

What mass of precipitate (in g) is formed when 45.5 mL of 0.300 M Na3PO4 reacts with 50.0 mL of 0.200 M Cr(NO3)3 in the following chemical reaction? Na3PO4(aq) + Cr(NO3)3(aq) → CrPO4(s) + 3 NaNO3(aq)

The freezing point depression of a solution of nitrobenzene and a non-ionic (non-electrolyte) unknown was used to determine the molar mass of an unknown. Time-temperature data for the cooling of a solution containing 50.0 g of nitrobenzene and 3.57 g of the unknown is shown in the graph below. The freezing point of pure nitrobenzene is 5.30 °C. The K, of nitrobenzene is 6.87 °C/m.

Determine the mass of sucrose necessary to prepare each of the standard sucrose solutions (from procedural overview step 1). Record the mass to two decimal places. Show the calculations for the mass of sucrose necessary to prepare the 2% solution.

At a certain temperature the vapor pressure of pure heptane (C7H16) is measured to be 93. mmHg. Suppose a solution is prepared by mixing 58.6 g of heptane and 113. g of acetyl bromide (CH3COBr). Calculate the partial pressure of heptane vapor above this solution. Round your answer to 2 significant digits.

Calculate the density of an object, if the mass is 34.8 g and the volume is 6.2 mL. density = mass/volume Remember to select an answer with the correct number of significant figures. 5.6 g 0.18 mL 0.18 g/mL 5.6 g/mL I DON'T KNOW YET

A certain liquid X has a normal boiling point of 107.50 "C and a boiling point elevation constant Kb = 1.95 °C kg mol. Calculate the boiling point of a solution made of 48.0g of zinc chloride (ZnCl₂) dissolved in 550. g of X. Round your answer to 5 significant digits.

A 250-ml flask and stopper have a mass of 110.525 g. A 50.0-mL sample of gasoline is pipetted into the flask, giving a total mass of 146.770 g. Find the density of the gasoline.

What is the total mass of a solution if 47.87 g of a solid is added to a container with 566.7 g of water? Include units and answer to the correct number of significant figures (digits)

Given a solution of 0.630 M Na2SO4, what volume (in mL) would be needed to make 2.000 L of a 0.420 M solution?

A biochemist carefully measures the molarity of calcium lon in 89.3 mL of cell growth medium to be 68.2 µM. Unfortunately, a careless graduate student forgets to cover the container of growth medium and a substantial amount of the solvent evaporates. The volume of the cell growth medium falls to 12.7 ml. Calculate the new molarity of calcium ion in the cell growth medium. Round each of your answers to 3 significant digits.

Part 3: Match each diagram with its correct description. Diagrams will be used once. 1. Pure Element - only one type of atom present. 2. Mixture of two elements - two types of uncombined atoms present. 3. Pure compound - only one type of compound present. 4. Mixture of two compounds - two types of compounds present. 5. Mixture of a compound and an element.

Commercial SCUBA divers use tanks filled with a mixture of gases known as Trimix on very long, deep dives. Trimix is composed of 70% nitrogen, 10% oxygen, and 20% helium. The total pressure of Trimix inside a certain tank at the beginning of the dive is 118.4 atm. Recall that the total pressure of air at sea level is about 1 atm, and that air is 20.9% oxygen. How does the partial pressure of oxygen in the tank compare to the partial pressure of oxygen in the air?

A certain substance X has a normal freezing point of 1.4 °C and a molal freezing point depression constant Kf=6.75 °C-kg-mol. A solution is prepared by dissolving some urea ((NH₂)2CO) in 450. g of X. This solution freezes at -2.7 °C. Calculate the mass of urea that was dissolved. Round your answer to 2 significant digits.

At 25.0 °C the Henry's Law constant for dinitrogen monoxide (N₂O) gas in water is 0.025 M/atm. Calculate the mass in grams of N₂O gas that can be dissolved in 900. mL of water at 25.0 °C and a N₂O partial pressure of 1.84 atm. Round your answer to 2 significant digits.

When 62.3 g of alanine (C3H7NO₂) are dissolved in 850. g of a certain mystery liquid X, the freezing point of the solution is 4.40 °C less than the freezing Calculate the mass of potassium bromide that must be dissolved in the same mass of X to produce the same depression in freezing point. The van't Hoff factor i=1.54 for potassium bromide in X. Be sure your answer has a unit symbol, if necessary, and round your answer to 3 significant digits.

A certain liquid X has a normal boiling point of 124.50 °C and a boiling point elevation constant K,-0.60 °C kg mol^-1. Calculate the boiling point of a solution made of 22.9g of zinc chloride (ZnCl2) dissolved in 300. g of X. Round your answer to 4 significant digits.

A certain liquid X has a normal freezing point of 6.60 °C and a freezing point depression constant X-5.85 °C-kg-mol .A solution is prepared by dissolving some alanine (C3H7NO₂) in 300. g of X. This solution freezes at 2.9 °C. Calculate the mass of C3H7NO2 that was dissolved. Round your answer to 2 significant digits.

When 1.10 g of a certain molecular compound X are dissolved in 35.0 g of benzene (C6H6), the freezing point of the solution is measured to be 3.5 °C. Calculate the molar mass of X. If you need any additional information on benzene, use only what you find rounded to 2 significant digits. the ALEKS Data resource. Also, be sure your answer has a unit symbol, and is

When 160. g of glycine (C₂H5NO₂) are dissolved in 1200. g of a certain mystery liquid X, the freezing point of the solution is 8.3 °C lower than the freezing point of pure X. On the other hand, when 160. g of ammonium chloride (NH4CI) are dissolved in the same mass of X, the freezing point of the solution is 20.5 °C lower than the freezing point of pure X. Calculate the van't Hoff factor for ammonium chloride in X. Be sure your answer has a unit symbol, if necessary, and round your answer to 2 significant digits.

When 193. g of benzamide (C7H7NO) are dissolved in 550. g of a certain mystery liquid X, the freezing point of the solution is 5.4 °C lower than the freezing point of pure X. On the other hand, when 193. g of iron(III) chloride are dissolved in the same mass of X, the freezing point of the solution is 14.3 °C lower than the freezing point of pure X. Calculate the van't Hoff factor for iron(III) chloride in X. Be sure your answer has a unit symbol, if necessary, and round your answer to 2 significant digits.

A student dissolves 6.7 g of glucose (C6H12o6) in 300. mL of a solvent with a density of 0.84 g/mL. The student notices that the volume of the solvent does not change when the glucose dissolves in it. Calculate the molarity and molality of the student's solution. Round both of your answers to 2 significant digits.

When 5.36 g of a certain molecular compound X are dissolved in 25. g of formamide (NH2COH), the freezing point of the solution is measured to be 0.6 C. Calculate the molar mass of X. If you need any additional information on formamide, use only what you find in the ALEKS Data resource. Also, be sure your answer has a unit symbol, and is rounded to 2 significant digits.

A student dissolves 6.2 g of biphenyl (C12H10) in 400. ml of a solvent with a density of 0.83 g/ml.. The student notices that the volume of the solvent does not change when the biphenyl dissolves in it. Calculate the molarity and molality of the student's solution. Round both of your answers to 2 significant digits.

A certain substance X melts at a temperature of 7.6 °C. But if a 750. g sample of X is prepared with 30.54 g of urea ((NH₂)₂CO) dissolved in it, the sample is found to have a melting point of 2.8 °C instead. Calculate the molal freezing point depression constant KF of X. Round your answer to 2 significant digits.

A certain substance X has a normal boiling point of 130.5 °C and a molal boiling point elevation constant K,- 1.33 °C-kg-mol. A solution is prepared by dissolving some urea ((NH₂), CO) in 550. g of X. This solution boils at 132.3 °C. Calculate the mass of urea that was dissolved. Round your answer to 2 significant digits.