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chemistry principles and practice

Questions and Answers of Chemistry Principles And Practice

A chemist adds 30 g sodium acetate to 50 mL water at room temperature. Only part of the sodium acetate dissolves. The mixture is heated with stirring, and all of the solid dissolves. With slow
Is methyl alcohol (CH3OH) more soluble in water or in hexane? Explain.
In diluting sulfuric acid with water, you should slowly add the acid to the water while stirring. This is sometimes expressed as “Always add acid” (AAA). Give the reasons for this procedure.
What is the molal concentration of nitrogen in this same solution? The mole fraction of nitrogen in air is 0.78.
What is the molal concentration of oxygen in water at 20 °C that has been saturated with air at 1.00 atm ? Assume that the mole fraction of oxygen in air is 0.21 .StrategyUse Henry’s law to
Straight-chain alcohols [CH3(CH2)nOH] that contain more than four carbon atoms have limited solubility in water. Predict how the solubility of these alcohols in water changes as the value of n in the
Explain why opening a warm carbonated beverage results in much more frothing than is observed when the container has been refrigerated.
At 1 atm pressure, the solubility of oxygen is 1.43 × 10-3 molal at 20 °C and 8.71 × 10-4 molal at 60 °C. What is the sign of the enthalpy of solution of oxygen?
The enthalpy of solution of potassium chromate (K2CrO4) in water is +17.4 kJ/mol. How does the solubility of this compound change when the temperature is reduced?StrategyDetermine whether the
Why do carbonated beverages go flat if they are not stored in a tightly sealed container?
What is the solute concentration in a benzene solution that has a vapor pressure of 90.6 torr at 25 °C?
What is the boiling point of a 0.32-molal solution of iodine (I2) in benzene at 1 atm?StrategyUse the value of kb for benzene given in Table 12.4 and the molal concentration of the solute to find the
At 25 °C the vapor pressure of pure benzene is 93.9 torr . A solution of a nonvolatile solute in benzene has a vapor pressure of 91.5 torr at the same temperature. What is the concentration of the
Explain why the solubilities of solids in a liquid change little with pressure.
What is the boiling point of a 0.60-molal solution of sucrose in water at 1 atm?
The numeric values of the molarity and molality of a dilute solution can be very similar or quite different, depending on the density of the solvent. Explain why.
Find the(a) Molality(b) Mole fraction of a 24.5% solution of ammonia (NH3) in water.
Consider the Lake Nyos situation as discussed in the chapter introduction. Is such a situation more likely to occur with a gas that has a high Henry’s law constant or a low Henry’s law constant?
Find the molar mass of a nonvolatile solute, if a solution of 1.20 g of the compound dissolved in 20.0 g benzene has a boiling point of 80.94 °C.
List and define the colligative properties, and give the units used for concentrations for each.
Benzophenone has a freezing point of 49.00 °C. What is the freezing point of a 0.450-molal solution of urea in this solvent if the freezing-point depression constant is equal to 9.80 °C/m?
Pure ethylene dibromide freezes at 9.80 °C . A solution is made by dissolving 0.213 g ferrocene (molecular formula Fe(C5H5)2, molar mass = 186.04 g/mol) in 10.0 g ethylene dibromide. The
Create a flow diagram, similar to those used in the example problems of this chapter, that outlines the determination of the molar mass of a compound from freezing point depression measurements.
A solution of 0.134 g of a compound in 4.76 g ethylene dibromide has a freezing point of 7.62 °C. Find the molar mass of this solute.
To identify a newly prepared substance, a scientist needs to measure its molar mass. The scientist prepares a solution by dissolving 0.350 g of the unknown compound in 5.42 g ethylene dibromide. This
A 5.70-mg sample of a protein is dissolved in water to give 1.00 mL of solution. If the osmotic pressure of this solution is 6.52 torr at 20 °C, what is the molar mass of the protein?
Specific samples of aqueous solutions of sucrose and urea both freeze at 0.25 °C. What other properties of these two solutions should be the same?
Hemoglobin is a large molecule that carries oxygen in human blood. A water solution that contains 0.263 g of hemoglobin (abbreviated here as Hb) in 10.0 mL of solution has an osmotic pressure of 7.51
Arrange the following solutions in order of increasing osmotic pressure: 0.02 M sucrose, 0.02 M HNO3, 0.01 M BaCl2.
Compare the freezing points of 0.1-m aqueous solutions of NaCl and CaCl2. Explain why one of these solutions has a lower freezing point.
Arrange the following aqueous solutions in order of increasing freezing point, assuming ideal behavior: 0.05 m sucrose, 0.02 m NaCl, 0.01 m CaCl2, 0.03 m HCl.StrategyThe freezing point of a solution
What is the vapor pressure, at 60 °C, of a solution with Use the data given in this example. Xtoluene = 0.10 and Xbenzene 0.90?
At 60 °C, the vapor pressure of pure benzene is 384 torr , and that of pure toluene is 133 torr . A mixture is made by combining 1.20 mol toluene with 3.60 mol benzene. Find:(a) The mole fraction of
A solution contains 1.20 g benzoic acid (C6H5CO2H) in 750.0 g water. Express the concentration of benzoic acid as(a) Mass percentage.(b) Mole fraction.(c) Molality.
A solution is prepared by dissolving 25.0 g BaCl2 in 500 g water. Express the concentration of BaCl2 in this solution as(a) Mass percentage.(b) Mole fraction.(c) Molality.
A solution contains 4.50 g calcium nitrate [Ca(NO3)2] in 430.0 g water. Express the concentration of Ca(NO3)2 as(a) Mass percentage.(b) Mole fraction.(c) Molality.
A solution contains 3.80 g urea [CO(NH2)2] in 125.0 g water. Express the concentration of urea as(a) Mass percentage.(b) Mole fraction.(c) Molality.
How many moles of hydrogen peroxide are present in 25.0 g of a 3.0% solution? HYDROGEN PEROXIDE SOLUTION SA U.S.P. ACTIVE INGREDIENT: HYDROGEN PEROXIDE 3% INERT INGREDIENTS FOR EXTERNAL USE:
How many grams of sodium chloride, NaCl, are present in 35.0 g of a 3.5% solution?
Give quantitative directions for preparing 15.5 g of a 1.00% solution of boric acid (H3BO3). What is the molal concentration of this solution?
Describe how you would prepare 465 mL of 0.355 M potassium dichromate solution.
A 2.77 M NaOH solution in water has a density of 1.109 g/mL. Express the concentration of this solution as(a) Mass percentage.(b) Mole fraction.(c) Molality.
A 0.631 M H3PO4 solution in water has a density of 1.031 g/mL. Express the concentration of this solution as(a) Mass percentage.(b) Mole fraction.(c) Molality.
Vinegar is a 5.0% solution of acetic acid (CH3CO2H) in water. Th e density of vinegar is 1.0055 g/mL. Express the concentration of acetic acid as(a) Molality.(b) Molarity.(c) Mole fraction.
A 10.0% solution of sucrose (C12H22O11) in water has a density of 1.038 g/mL. Express the concentration of the sugar as(a) Molality.(b) Molarity.(c) Mole fraction.
Rubbing alcohol is a water solution that contains 70% isopropanol (C3H7OH). What is the mole fraction of isopropanol in rubbing alcohol?
A water solution of sodium hypochlorite (NaOCl) is used as laundry bleach. The concentration of sodium hypochlorite is 0.75 m. Express this concentration as a mole fraction.
What is the mole fraction of bromine (Br2) in an aqueous 0.10-molal solution?
What is the mole fraction of nitrous oxide (N2O) in an aqueous 0.020-molal solution?
What is the molality of copper(II) bromide (CuBr2) in an aqueous 0.50% solution of that compound?
What is the molality of silver nitrate (AgNO3) in an aqueous 0.10% solution of that compound?
A solution contains 10.0 g ethanol (C2H5OH), 20.0 g ethylene glycol [C2H4(OH)2], and 90.0 g water. What is the mole fraction of water in the sample?
A solution contains 12.0 g hexane (C6H14), 20.0 g octane (C8H18), and 98.0 g benzene (C6H6). What is the mole fraction of benzene in the solution?
Complete the following table for ammonia (NH3) solutions in water. Density (g/cm) (a) 0.973 (b) 0.936 (c) 0.950 (d) 0.969 Molality Molarity 8.02 8.80 Mass % NH3 6.00 Mole Fraction 0.0738
Complete the following table for perchloric acid (HClO4) solutions in water. Density (g/cm) Molality Molarity (a) 1.060 (b) 1.011 (c) 1.143 (d) 1.086 2.807 0.2012 Mass % HCIO 10.0 Mole Fraction 0.0284
The density of a 3.75 M aqueous sulfuric acid solution in a car battery is 1.225 g/mL. Express the concentration of the solution in molality, mole fraction H2SO4, and mass percentage of H2SO4.
Household bleach is a 5.00% solution of NaClO in water and has a density of 1.10 g/mL. Express the concentration of the solution in molality, mole fraction NaClO, and molarity of NaClO.
Using the intermolecular attractions as a guide, arrange the following solutes in order of increasing solubility in benzene (C6H6): hexane (C6H14), ethanol (C2H5OH), water.
Which pairs of liquids will be soluble in each other?(a) H2O and CH3CH2CH2CH3(b) C6H6 (benzene) and CCl4(c) H2O and CH3CO2H
Predict the relative solubility of each compound in the two solvents, on the basis of intermolecular attractions.(a) Is Br2 more soluble in water or in carbon tetrachloride?(b) Is CaCl2 more soluble
Predict the relative solubility of each compound in the two solvents, on the basis of intermolecular attractions.(a) Is NaCl more soluble in water or in carbon tetrachloride?(b) Is I2 more soluble
Identify the most important types of solute-solvent interactions in each of the following solutions.(a) (CH3)2CO in water(b) IBr in CHCl3(c) CaCl2 in water(d) krypton in CH3OH
Identify the most important types of solute-solvent interactions in each of the following solutions.(a) CH3OH in water(b) IBr in CH3CN(c) KBr in water(d) Argon in water
Choose the solute of each pair that would be more soluble in hexane (C6H14). Explain your answer.(a) CH3(CH2)10OH or CH3(CH2)2OH(b) BaCl2 or CCl4(c) Fe(C5H5)2 (a nonelectrolyte) or FeCl2
Choose the solute of each pair that would be more soluble in water. Explain your answer.(a) NaOH or CO2(b) TiCl3 or CHCl3(c) C3H8 or C3H7OH
The solubility of acetylene (C2H2) in water at 20 °C and 0.200 atm pressure is 9.38 × 10-3 molal.(a) Calculate the Henry’s law constant for this gas in units of molal/torr.(b) How many grams of
The solubility of ethylene (C2H4) in water at 20 °C and 0.300 atm pressure is 1.27 × 10-4 molal.(a) Calculate the Henry’s law constant for this gas in units of molal/torr.(b) How many grams of
The enthalpy of solution of ozone (O3) in water is -17 kJ/mol, and its solubility at 0 °C and 1.00 atm is 0.105 g per 100 g water.(a) What is the Henry’s law constant (in molal/torr) at 0
The enthalpy of solution of nitrous oxide (N2O) in water is -12.0 kJ/mol, and its solubility at 20 °C and 1.00 atm is 0.121 g per 100 g water.(a) What is the Henry’s law constant (in molal/torr)
The solubility of potassium chloride in water increases from 34.7 g/100 mL at 20 °C to 56.7 g/100 mL at 100 °C. Is the enthalpy of solution for this compound endothermic or exothermic? Explain your
The solubility of lead bromide in water is 0.844 g per 100 g water at 20 °C and 4.71 g per 100 g water at 100 °C. Is the dissolution of lead bromide an endothermic or exothermic process? Explain
The solubility of calcium hydroxide in water is 0.165 g per 100 g water at 20 °C and 0.128 g per 100 g water at 50 °C. Is the dissolution of calcium hydroxide an endothermic or exothermic process?
The solubilities of most gases in water decrease as the temperature increases. Are the enthalpies of solution for such gases negative or positive? Explain your answer.
From the data presented in Figure 12.11, determine which has the more positive enthalpy of solution: NaCl or NH4Cl. Explain.Figure 12.11 Solubility (g/100 mL) 100 80 60 40 20 NaNO3 Pb(NO3)2KNO3 NHC
From the data presented in Figure 12.11, determine which has the more positive enthalpy of solution: NaCl or KNO3. Explain.Figure 12.11 Solubility (g/100 mL) 100 80 60 40 20 NaNOs Pb (NO3)2KNO3 NH4CI
At 22 °C and 1.0 atm, the enthalpy of solution of nitrogen in water is -11.0 kJ/mol, and its solubility is 6.68 × 10-4 m. State whether the solubility of nitrogen is greater or less than 6.68 ×
At 25 °C and 2.0 atm, the enthalpy of solution of neon in water is -2.46 kJ/mol, and its solubility is 9.07 × 10-4 m. State whether the solubility of neon is greater or less than 9.07 × 10-4 m
The enthalpy of solution of nitrous oxide (N2O) in water is -12.0 kJ/mol, and its solubility at 20 °C and 2.00 atm is 0.055 m. State whether the solubility of nitrous oxide is greater or less than
The enthalpy of solution of ozone (O3) in water is -17 kJ/mol, and its solubility at 25 °C and 1.00 atm is 0.0052 m. State whether the solubility of ozone is greater or less than 0.0052 m at(a) 1.00
The vapor pressure of chloroform (CHCl3) is 360 torr at 40.0 °C. Find the vapor-pressure depression (in torr) produced by dissolving 10.0 g phenol (C6H5OH) in 95.0 g chloroform. What is the vapor
A solution is prepared by dissolving 8.89 g of ordinary sugar (sucrose, C12H22O11, 342 g/mol) in 34.0 g water. Calculate the boiling point of the solution using kb as 0.512 °C/m. Sucrose is a
A 0.350-g sample of a nonvolatile compound dissolves in 12.0 g cyclohexane, producing a solution that freezes at 0.83 °C. Cyclohexane has a freezing point of 6.50 °C and a freezing-point depression
Cyclohexane has a normal boiling point of 80.72 °C. The solution described in Exercise 12.67 boils at 81.94 °C. Find the boiling-point elevation constant for cyclohexane.Exercise 12.67The freezing
The freezing point of cyclohexane is 6.50 °C. A solution that contains 0.500 g phenol (molar mass = 94.1 g/mol) in 12.0 g cyclohexane freezes at -2.44 °C. Calculate the freezing-point depression
Cyclohexane (C6H12) has a vapor pressure of 99.0 torr at 25 °C. What is the vapor pressure (in torr) of cyclohexane above a solution of 14.0 g naphthalene (C10H8) in 50 g cyclohexane at 25 °C?
A solution contains 2.00 g of the nonvolatile solute urea (molar mass = 60.06 g/mol) dissolved in 25.0 g water. Using the data in Table 12.4, calculate the freezing and boiling points of the solution
How many grams of water must be added to 4.00 g urea [CO(NH2)2; molar mass = 60.06 g/mol] to produce a 0.250-m solution of the compound?
The concentration of a solution is often used as a conversion factor. For example, molarity is a conversion factor to find the moles of solute in a specified volume of solution. What conversions are
Determine the molality of the solution in Example 12.1 (5.00 g NaCl in 200 g water).StrategyDetermine the amount of solute and the mass of solvent before using the definition of molality.Example
Concentration units all express the quantity of solute present in some quantity of solution or solvent. For molarity, mole fraction, and mass percentage, how is the quantity of solution expressed?
A chemical analysis shows that 25.0 g of a solution contains 2.00 g glucose. Calculate the concentration in mass percentage of glucose.
The thermite reaction is a reaction between solid iron(III) oxide and solid aluminum to make aluminum oxide and elemental iron. Usually the reactants are fine powders, to increase the contact between
Two compounds, A and B, have the molecular formula C3H9N. One isomer has no hydrogen atoms bonded to the nitrogen atom and has a boiling point of 2.9 °C. The other isomer (boiling point of 47.8 °C)
Consider a sealed flask with a movable piston that contains 5.25 L O2 saturated with water vapor at 25 °C. The piston is depressed at constant temperature so that the gas is compressed to a volume
A white crystalline compound that has a high melting point has the formula MCl. A 2.13-g sample dissolves in 200 mL of water, and addition of excess AgNO3 gives a 4.09-g precipitate of AgCl. What is
Draw the Lewis structures of CF4 and CF2CCl2. What is the hybridization of the carbon atoms in these compounds? Predict whether each is polar or nonpolar. What types of intermolecular forces do you
How much heat is absorbed by a 15.0-g sample of water in going from liquid at 10 °C to steam at 105 °C and a pressure of 1.00 atm? Use the data in the accompanying table. Some Thermal Properties of
How much heat is absorbed by a 10.0-g sample of water in going from ice at -10 °C to liquid water at 95 °C? Use the data in the accompanying table.
The cooling process in a refrigeration unit involves reducing the pressure above a liquid called the refrigerant. The pressure reduction causes vaporization, which cools the remaining liquid. A
A 1.50-g sample of water is placed in an evacuated 1.00-L container at 30 °C.(a) Calculate the pressure in the container if all of the water is vaporized. (Assume the ideal gas law, PV =

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