ch. 9

Which of the following statements correctly explain the relationship between the solubility of a gas and its pressure?

- The solubility of nitrogen gas at 2.00 atm is twice the solubility of the gas at 1.00 atm. - The solubility of a gas decreases with a decrease in pressure. - The concentration of gas particles in the solution is higher at 4.25 atm than at 1.00 atm

What volume of 2.00 M HCl in liters is needed to react completely (with nothing left over) with 0.500 L of 0.500 M Na2CO3?

.250 L

In order to prepare 10.0 m L (0.0100 L) solution of 1.40 M sodium hydroxide, a mass of ______ would be required.

0.560 g

A 609-mL sample of unknown HCl solution reacts completely with Na2CO3 to form 11.1 g CO2. What was the concentration of the HCl solution?

0.828 M

A CaCl2 solution is given to increase blood levels of calcium. If a patient receives 6.0 mL of a 15 % (m/v) CaCl2 solution, how many grams of CaCl2 were given?

0.90g CaCl2

A patient receives 170 mL of a 6.0 % (m/v) amino acid solution twice a day. 1. How many grams of amino acids are in 170 mL of solution? 2. How many grams of amino acids does the patient receive in 1 day?

1. 10g 2. 20g

A patient receives 100 mL of 21% (m/v) mannitol solution every hour. 1. How many grams of mannitol are given in 1 hour? 2. How many grams of mannitol does the patient receive in 15 hours?

1. 21 g 2. 320 g

In the video, the semipermeable membrane separates the two solutions of different concentrations. Watch the video, and identify which of the following statements are correct.

1. The solvent can ideally move in both directions through the semipermeable membrane. 2. The movement of the solvent particles from the concentrated solution to the dilute solution is known as reverse osmosis.

Watch the animation in the activity, and rank the events in the order that they occur as equilibrium is reached, keeping in mind that some events may occur simultaneously.

1. hydration of cations and anions and dissociation of salt into its cations and anions 2. dissolved cations and anions begin to deposit as a solid salt 3. rate of dissolution is equal to the rate of recrystallization

850. mL of 0.60 %(m/v) NaCl from 4.0 % (m/v) NaCl

1.3*10^2 mL

Calculate the molarity (M) of 156.2 g of H2SO4 in 1.135 L of solution.

1.404 M

Gastric acid pH can range from 1 to 4, and most of the acid is HCl. For a sample of stomach acid that is 8.53×10−3 M in HCl, how many moles of HCl are in 18.2 mL of the stomach acid?

1.55*10^-4 mol

Indicate the compartment that will increase in volume for the following pairs of solutions separated by a semipermeable membrane: - 0.1 % (m/v) starch - 10 % (m/v) starch

10 % (m/v) starch

Indicate the compartment that will increase in volume for the following pairs of solutions separated by a semipermeable membrane: - 5 % (m/v) sucrose - 10 % (m/v) sucrose

10 % (m/v) sucrose

A solution mass of 1 kg is ______ times greater than 100 g, thus one kilogram (1 kg) of a 2.5% KI solution would contain _______ of KI.

10, 25 g

Vinegar is a solution of acetic acid in water. If a 185 mL bottle of distilled vinegar contains 20.3 mL of acetic acid, what is the volume percent (v/v) of the solution?

11.0%

A 877 mL NaCl solution is diluted to a volume of 1.22 L and a concentration of 8.00 M . What was the initial concentration?

11.1 M

If there is 800 mL of champagne in the bottle, how many milliliters of alcohol are present?

110 mL

4.1 g of KOH and 24.5 g of H2O

14% [4.1/(4.1+24.5)]

How many grams (of mass mmm) of glucose are in 265 mL of a 5.50% (m/v) glucose solution?

14.6 g

64 g of NaOH in 399 g of NaOH solution

16% (64g/399g)

What volume of a 6.08 M stock solution do you need to prepare 250. mL of a 0.0581 M solution of HCl?

2.39 mL

A 2.5% (by mass) solution concentration signifies that there is _____ of solute in every 100 g of solution.

2.5 g

Therefore, when 2.5 % is expressed as a ratio of solute mass over solution mass, that mass ratio would be...

2.5g/100g

You need 660. mL of a 10. % (m/v) glucose solution. If you have a 25 % (m/v) glucose solution on hand, how many milliliters do you need?

2.6*10^2 mL

Calculate the mass/volume percent of a NaCl solution in which 113 g of NaCl is dissolved in enough water to give a total volume of 3.78 L .

2.99 % (m/v)

Calculate the mass percent (m/m) of a solution prepared by dissolving 42.56 g of NaCl in 166.6 g of H2O.

20.35%

Calculate the mass/volume percent (m/v) of 15.5 g NaCl in 63.0 mL of solution.

24.6%

You have prepared a saturated solution of X at 20ºC using 33.0 g of water. How much more solute can be dissolved if the temperature is increased to 30ºC

3.96 g

500. mL of 3.00 MNaOH from 5.00 M NaOH

300 mL

The concentration of the KCN solution given in Part A corresponds to a mass percent of 0.358 %. What mass of a 0.358 % KCN solution contains 1080 mg of KCN?

302 g

A 6.00 % (m/v) NaCl solution contains 34.1 g of NaCl. What is the total volume (V) of the solution in milliliters?

568 mL

A solution of rubbing alcohol is 75.9 % (v/v) isopropanol in water. How many milliliters of isopropanol are in a 77.1 mL sample of the rubbing alcohol solution?

58.5 mL

An intravenous solution of mannitol is used as a diuretic to increase the loss of sodium and chloride by a patient. If a patient receives 25.0 mL of a 25. % (m/v) mannitol solution, how many grams of mannitol were given?

6.3 g of mannitol

Indicate the compartment that will increase in volume for the following pairs of solutions separated by a semipermeable membrane: - 4 % (m/v) albumin - 8 % (m/v) albumin

8 % (m/v) albumin

Why do lettuce leaves in a salad wilt after a vinaigrette dressing containing salt is added?

A vinaigrette dressing containing salt is hypertonic to lettuce leaves. Water moves out of the lettuce leaves to the salt solution. The lettuce leaves wilt.

Why does iodine dissolve in hexane, but not in water?

Because iodine is a nonpolar molecule, it will dissolve in hexane, a nonpolar solvent. Iodine does not dissolve in water because water is a polar solvent.

Why would a dialysis unit (artificial kidney) use isotonic concentrations of NaCl, KCl, NaHCO3, and glucose in the dialysate?

Isotonic concentrations of sodium chloride, potassium chloride, sodium bicarbonate, and glucose are used in the dialysate to maintain the concentrations of these various ions and glucose at normal levels in the blood as waste products are removed.

Each of the following is placed in a dialyzing bag and the bag is then immersed in distilled water. Which substances will be found outside the bag? NaCl sol'n albumin mixture starch mixture

NaCl sol'n

Consider a mixture of NaCl, albumin mixture, and starch mixtures in a dialyzing bag. The dialyzing bag is then immersed in distilled water. Which of the following actions should be taken to remove the most salt from the mixture?

Replace the water with fresh distilled water periodically. Submit

A semipermeable membrane is placed between the following solutions. Which solution will decrease in volume? - Solution B: 7.74 % (m/v) starch - Solution A: 1.53 % (m/v) starch

Solution A: 1.53 % (m/v) starch

A semipermeable membrane is placed between the following solutions. Which solution will increase in volume? - Solution D: 14.4 % NaCl - Solution C: 8.87 % NaCl

Solution D: 14.4 % NaCl

When the solute and a total of 10.0 mL of water are both added into the beaker and stirred until the solute dissolves, the solution volume will be _________.

greater than 10.0 mL

Based on that, the concentration of the prepared solution will be ___________.

less than 1.40

Potassium fluoride has a solubility of 92 g of KF in 100 gg of H2O at 18 ºC. State if each of the following mixture forms an unsaturated or saturated solution at 18 ºC: 42 g of KF and 50 g of H2O

unsaturated

Suppose that NaClNaCl is added to hexane instead of water. Which of the following intermolecular forces will exist in the system?

- London dispersion force between two hexane molecules - Ion-ion force between Na+Na+ and Cl−Cl− ions

The dissolution process can be altered by varying these parameters, such as by increasing or decreasing the temperature or by reducing the particle size of the solute. Consider the preparation of a NaClNaCl salt solution using coarse crystals of NaClNaCl in an unstirred container at room temperature. Classify the following conditions based on the change in the rate of dissolution of NaClNaCl in water compared to the initial preparation if the dissolution process is endothermic. SLOWER DISSOLUTION PROCESS

- NaCl salt is added to water, mixture is cooled - a large piece of NaCl salt is added to water

The solubility of solute in a solvent depends on various parameters, such as temperature, pressure, the nature of the solute, and the nature of the solvent. Considering these parameters, identify the statements that are correct for the solubility of a solute in a solvent.

- Table salt dissolves in water to form a solution. - Copper sulfate is soluble in water. - Carbon dioxide gas will be less soluble in water when the partial pressure is low.

The dissolution process can be altered by varying these parameters, such as by increasing or decreasing the temperature or by reducing the particle size of the solute. Consider the preparation of a NaClNaCl salt solution using coarse crystals of NaClNaCl in an unstirred container at room temperature. Classify the following conditions based on the change in the rate of dissolution of NaClNaCl in water compared to the initial preparation if the dissolution process is endothermic. FASTER DISSOLUTION PROCESS

- finely powdered NaCl salt is added to water - NaCl salt is added to water, and the mixture is heated - NaCl salt added to water, and the mixture is stirred

Five different substances are given to you to be dissolved in water. Which substances are most likely to undergo dissolution in water?

- sodium iodide, NaI - ethanol, CH3CH2OH - potassium bromide, KBr

At a pressure of 1.00 atmatm, the solubility of nitrogen in water is 23.5 mg gas/100 g watermg gas/100 g water. Indicate whether each of the following changes would increase or decrease the solubility of nitrogen in water. solubility increases

- sol'm canned at a pressure of 2.04 atm - sol'n is submerged 40m under water

At a pressure of 1.00 atmatm, the solubility of nitrogen in water is 23.5 mg gas/100 g watermg gas/100 g water. Indicate whether each of the following changes would increase or decrease the solubility of nitrogen in water. solubility decreases

- sol'n placed in chamber where pressure is 0.5 atm - sol'n is carried to the top of a mountain - sol'n is brought into outer space

Indicate whether each of the following ionic compounds is soluble or insoluble in water:

insoluble - CuCO3 - FeO - Mg3(PO)4 soluble - (NH4)2SO4 - NaHCO2

The following set of solutions are prepared by dissolving the requisite amount of solute in water to obtain the desired concentrations. The pressure of the system is then manipulated such that movement is from the solution listed first to the solution listed second. REVERSE OSMOSIS

0.01 M sucrose to 1.00M sucrose 0.5M NaCl to 1.00M NaCl 1.6M KCl to 3.2M KCl

Potassium cyanide is a toxic substance, and the median lethal dose depends on the mass of the person or animal that ingests it. The median lethal dose of KCN for a person weighing 175 lb (79.4 kg ) is 9.75×10−3 mol . What volume of a 0.0550 M KCN solution contains 9.75×10−3 mol of KCN?

0.177 L

The following set of solutions are prepared by dissolving the requisite amount of solute in water to obtain the desired concentrations. The pressure of the system is then manipulated such that movement is from the solution listed first to the solution listed second. OSMOSIS

3.00M CH3COOH to 1.5M CH3COOH 3.2M HNO3 to 1.8M HNO3 0.6M KCl to 0.3M KCl

You have a solution that is 18.5 % (v/v) methyl alcohol. If the bottle contains 2.94 L of solution, what is the volume (V) in milliliters of methyl alcohol?

544 mL

Calculate the mass percent of a solution that is prepared by adding 33.7 g of NaOH to 362 g of H2O.

8.52 % (m/m)

Rank the solutions from highest to lowest osmotic pressure. - 8.6% KCl - 1.5% KCl - 5.0% KCl - 0.7% KCl - 1.8% KCl

8.6% KCl > 5.0% KCl > 1.8% KCl > 1.5% KCl > 0.7% KCl

What is the final volume in milliliters when 0.595 L of a 30.8 % (m/v) solution is diluted to 22.8 % (m/v)?

804 mL

A doctor orders 220. mmL of 3 % (m/v) ibuprofen. If you have 8.0 % (m/v) ibuprofen on hand, how many milliliters do you need?

83 mL

450 mL of 2.0 %b(m/v) HCl from 10.0 % (m/v) HCl

90.0 mL

A 10%% (m/vm/v) starch solution is separated from a 1%% (m/vm/v) starch solution by a semipermeable membrane. (Starch is a colloid.) A: 1% (m/v) starch solution or 10% (m/v) starch solution B: In which direction will water flow initially? C: In which compartment will the volume level rise?

A: 10% (m/v) starch solution B: Initially, water will flow out of the 1 %% (m/v) starch solution into 10%% (m/v) starch solution. C: The volume of the 10%% (m/v) starch solution will increase due to inflow of water.

Potassium chloride has a solubility of 43 g of KCl in 100 g of H2O at 50 ºC. Determine if each of the following forms an unsaturated or saturated solution at 50 ºC: A: adding 26 g of KCl to 100. g of H2O B: adding 19 g of KCl to 25. g of H2O C: adding 88 g of KCl to 150. g of H2O

A: unsaturated B: saturated C: saturated

Potassium nitrate has a solubility of 32 gg of KNO3 in 100 gg of H2O at 20 ºC. Determine if each of the following forms unsaturated or saturated solution at 20 ºC: A: adding 32 g of KNO3 to 240. g of H2O B: adding 17 g of KNO3 to 50. g of H2O C: adding 75 g of KNO3 to 150. g of H2O

A: unsaturated B: saturated C: saturated

To make tomato soup, you add one can of water to the condensed soup. Why is this a dilution?

Adding water (solvent) to the soup increases the volume and dilutes the tomato soup concentration.

How would you prepare 2.41 L of a 5.00 M solution from a 12.0 M stock solution?

Dilute 1.00 L of the 12.0 M solution to 2.41 L .

Rank electrolytes from weakest to strongest. - (C2H5)2NH; 5.55×10^−3 mol - C5H11N; 3.54×10^−2 mol - HONH2; 3.02×10^−5 mol - C6H15O3N; 7.61×10−4 mol

HONH2 < C6H15O3N < (C2H5)2NH < C5H11N

Each of the following is placed in a dialyzing bag and the bag is then immersed in distilled water. Which substances will be found inside the bag? NaCl sol'n albumin mixture starch mixture

NaCl sol'n albumin mixture starch mixture

How many liters of a 3.77 M K2SO4 solution are needed to provide 98.3 g of K2SO4 (molar mass 174.01 g/mol)? Recall that MM is equivalent to mol/L.

Volume of K2SO4 = 0.150 L

A student tests four solids for their ability to complete an electrical circuit when dissolved in water by observing their ability to close a circuit containing a light bulb and obtains the following results: The student is told that one of the four solids tested is actually calcium bromide ,CaBr2CaBr2. Which of the solids could be CaBr2CaBr2?

bright light

a mixture that cannot be separated by a semipermeable membrane

characteristic of a solution

a mixture that settles out upon standing

characteristic of a suspension

A red blood cell is placed into each of the following solutions. Indicate whether crenation, hemolysis, or neither will occur. Solution A: 4.02 % (m/v) NaCl Solution B: 2.92 % (m/v) glucose Solution C: distilled H2O Solution D: 7.79 % (m/v) glucose Solution E: 5.0 % (m/v) glucose and 0.9 % (m/v) NaCl

crenation - Solutions A, D & E hemolysis - Solutions B & C

A student tests four solids for their ability to complete an electrical circuit when dissolved in water by observing their ability to close a circuit containing a light bulb and obtains the following results: Which of the solids is a weak electrolyte when dissolved in water?

dim light

Due to the nature of the interaction between ions and solvent molecules, a _______ concentration of ions can be dissolved in water than in alcohol.

higher

When a salt is added to a polar solvent like water, the ions interact with the solvent molecules via _______ ________, which overcome the forces originally holding the ions together.

ion-dipole forces

Which intermolecular forces contribute to the dissolution of NaClNaCl in water?

ion-dipole forces

Salts are composed of ions that form a tightly packed and ordered network, which is called a crystal lattice, and it is held together by...

ionic bonds

A 20 mL solution containing 2 mmol of C12H22O11(aq) was integrated into to a circuit that powers a light bulb. When the power supply was turned on, the light bulb remained off. C12H22O11(aq) is a....

nonelectrolyte

If you carry out the reaction between table salt (NaClNaCl) and copper(II) sulfate (CuSO4CuSO4 ) in 100.0 mL100.0 mL of water, the salt copper(II) sulfate will behave similarly to the salts given in the tab named Slightly Soluble Salts. Enter the formula for the precipitate, without the phase, that will be formed. If no precipitate is formed, simply type "noreaction" in the answer box.

noreaction

The absorbance of a cationic iron(II) sample solution was measured in a spectrophotometer, but the instrument returned an error because the absorbance was too high. The sample was then diluted by using a pipette to take 100.0 μL of the sample and injecting it into a cuvette already containing 2.00 mL of water (total volume is 2.00 mL + 100.0 μL). The absorbance value of the diluted solution corresponded to a concentration of 7.71×10−6 M. What was the concentration of the original solution?

original concentration of Fe2+ = 1.62×10−4 M

Potassium fluoride has a solubility of 92 g of KF in 100 gg of H2O at 18 ºC. State if each of the following mixture forms an unsaturated or saturated solution at 18 ºC: 145 g of KF and 150 g of H2O

saturated

Potassium fluoride has a solubility of 92 g of KF in 100 gg of H2O at 18 ºC. State if each of the following mixture forms an unsaturated or saturated solution at 18 ºC: 35 g of KF and 25 g of H2O

saturated

Making sure the default volume of water is 1.00×10−16 L1.00×10−16 L when using the Slightly Soluble Salts tab, add each of the possible salts to the water. Observe how much salt dissolves before the solution becomes saturated. Arrange the following salts according to their solubility in water. Most to least soluble thallium (I) sulfide copper (i) iodide silver arsenate silver bromide

silver arsenate copper (i) iodide silver bromide thallium (I) sulfide

Identify the type of interactions involved in each of the following processes taking place during the dissolution of sodium chloride (NaCl) in water.

sol'v-sol'v - dipole-dipole attractions - interactions between the water molecules sol't-sol't - interactions involving ion-ion attractions - interaction between the ions of sodium chloride sol'v-sol't - interactions formed during hydration - interactions formed between the sodium ions and the oxygen atoms of water molecules

The ions are then isolated and stabilized in solution via these interactions, and when this occurs for most of the salt compound, it is considered _______ in that solvent.

soluble

A 20 mL solution containing 2 mmol of HBr(g) was integrated into to a circuit that powers a light bulb. When the power supply was turned on, the light bulb produced a bright glow. HBr(g) is a....

strong electrolyte

A 20 mL solution containing 2 mmol of CH3NH2(l) was integrated into to a circuit that powers a light bulb. When the power supply was turned on, the light bulb produced a dim glow. CH3NH2(l) is a...

weak electrolyte

A 20 mL solution containing 2 mmol of Fe2(SO4)3(s) was integrated into to a circuit that powers a light bulb. When the power supply was turned on, the light bulb faintly flickered. Fe2(SO4)3(s) is a...

weak electrolyte