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chemistry and chemical reactivity

Questions and Answers of Chemistry And Chemical Reactivity

CaTiO3, a perovskite, has the structure below.(a) If the density of the solid is 4.10 g/cm3, what is the length of a side of the unit cell?(b) Calculate the radius of the Ti4+ ion in the center of
Molecular solids, network solids, and amorphous solids all contain atoms that are joined together by covalent bonds. However, these classes of compounds are very different in overall structure, and
Potassium bromide has the same lattice structure as NaCl. Given the ionic radii of K+ (133 pm) and Br− (196 pm), calculate the density of KBr.
Boron phosphide, BP, is a semiconductor and a hard, abrasion-resistant material. It is made by reacting boron tribromide and phosphorus tribromide in a hydrogen atmosphere at high temperature (>750
Why is it not possible for a salt with the formula M3X (Na3PO4, for example) to have a face centered cubic lattice of X anions with M cations in octahedral holes?
Two identical swimming pools are filled with uniform spheres of ice packed as closely as possible. The spheres in the first pool are the size of grains of sand; those in the second pool are the size
Spinels are described in Study Question 53. Consider two normal spinels, CoAl2O4 and SnCo2O4. What metal ions are involved in each? What are their electron configurations? Are the metal ions
Prepare a graph of lattice enthalpy for lithium, sodium, and potassium halides (Table 12.1) vs. the sum of the ionic radii for the component ions (Figure 7.11). Evaluate the results and comment on
Outline a procedure to calculate the percent of space occupied by the atoms in an fcc arrangement.
Phase diagrams for materials that have allotropes can be more complicated than those shown in the chapter. Use the phase diagram for carbon given here to answer the following questions.(a) How many
The sample of nephrite jade shown on page 545 has the formula Ca2(Mg, Fe)5(Si4O11)2(OH)2. (Iron in this formula is in the +2 oxidation state.)(a) What is the charge on the (Si4O11)n− ion in this
Fill in the blanks in the table. Aqueous solutions are assumed. Weight Mole Compound Molality Percent Fraction 0.15 Nal C₂H5OH C12H22011 0.15 5.0
You dissolve 2.56 g of succinic acid, C2H4(CO2H)2, in 500. mL of water. Assuming that the density of water is 1.00 g/cm3, calculate the molality, mole fraction, and weight percent of acid in the
Fill in the blanks in the table. Aqueous solutions are assumed. Compound KNO3 CH3CO,H HOCH₂CH₂OH Molality 0.0183 Weight Mole Percent Fraction 10.0 18.0 RE
You dissolve 45.0 g of camphor, C10H16O, in 425 mL of ethanol, C2H5OH. Calculate the molality, mole fraction, and weight percent of camphor in this solution. (The density of ethanol is 0.785 g/mL.)
What mass of Na2CO3 must you add to 125 g of water to prepare 0.200 m Na2CO3? What is the mole fraction of Na2CO3 in the resulting solution?
What mass of NaNO3 must be added to 500. g of water to prepare a solution that is 0.0512 m in NaNO3? What is the mole fraction of NaNO3 in the solution?
You wish to prepare an aqueous solution of glycerol, C3H5(OH)3, in which the mole fraction of the solute is 0.093. What mass of glycerol must you add to 425 g of water to make this solution? What is
You want to prepare an aqueous solution of ethylene glycol, HOCH2CH2OH, in which the mole fraction of solute is 0.125. What mass of ethylene glycol, in grams, should you combine with 955 g of water?
Hydrochloric acid is sold as a concentrated aqueous solution. If the concentration of commercial HCl is 12.0 M and its density is 1.18 g/cm3, calculate the following:(a) The molality of the
Concentrated sulfuric acid has a density of 1.84 g/cm3 and is 95.0% by weight H2SO4. What is the molality of this acid? What is its molarity?
The average lithium ion concentration in seawater is 0.18 ppm. What is the molality of Li+ in seawater?
Acetone, CH3COCH3, is quite soluble in water. Explain why this should be so. O H₂CCCH3 Acetone
Silver ion has an average concentration of 28 ppb (parts per billion) in U.S. water supplies.(a) What is the molality of the silver ion?(b) If you wanted 1.0 × 102 g of silver and could recover it
Use the data of Table 13.1 to calculate the enthalpy of solution of LiCl.Data given in Table 13.1 TABLE 13.1 Data for Calculating Enthalpy of
Which pairs of liquids will be miscible?(a) H2O and CH3CH2CH2CH3(b) C6H6 (benzene) and CCl4(c) H2O and CH3CO2H
You make a saturated solution of NaCl at 25°C. No solid is present in the beaker holding the solution.What can be done to increase the amount of dissolved NaCl in this solution? (See Figure
Use the following data to calculate the enthalpy of solution of sodium perchlorate, NaClO4:ΔfH°(s) = −382.9 kJ/mol andΔfH°(aq, 1 m) = −369.5 kJ/mol
Some lithium chloride, LiCl, is dissolved in 100 mL of water in one beaker, and some Li2SO4 is dissolved in 100 mL of water in another beaker. Both are at 10°C, and both are saturated solutions;
The partial pressure of O2 in your lungs varies from 25 mm Hg to 40 mm Hg. What mass of O2 can dissolve in 1.0 L of water at 25°C if the partial pressure of O2 is 40 mm Hg?
The Henry’s law constant for O2 in water at 25°C is given in Table 13.2. Which of the following is a reasonable constant when the temperature is 50°C? Explain the reason for your choice.(a) 6.7
An unopened soda can has an aqueous CO2 concentration of 0.0506 m at 25°C. What is the pressure of CO2 gas in the can?
Hydrogen gas has a Henry’s law constant of 7.8 ×10−4mol/kg∙ bar at 25°C when dissolving in water. If the total pressure of gas (H2 gas plus water vapor) over water is 1.00 bar, what is the
A sealed flask contains water and oxygen gas at 25°C. The O2 gas has a partial pressure of 1.5 atm.(a) What is the concentration of O2 in the water?(b) If the pressure of O2 in the flask is raised
Butane, C4H10, has been suggested as the refrigerant in household compressors such as those found in air conditioners.(a) To what extent is butane soluble in water? Calculate the butane concentration
A 35.0-g sample of ethylene glycol, HOCH2CH2OH, is dissolved in 500.0 g of water. The vapor pressure of water at 32°C is 35.7 mm Hg. What is the vapor pressure of the water–ethylene glycol
Urea, (NH2)2CO, which is widely used in fertilizers and plastics, is quite soluble in water. If you dissolve 9.00 g of urea in 10.0 mL of water, what is the vapor pressure of the solution at 24°C?
Pure ethylene glycol, HOCH2CH2OH, is added to 2.00 kg of water in the cooling system of a car. The vapor pressure of the water in the system when the temperature is 90°C is 457 mm Hg. What mass of
Pure iodine (105 g) is dissolved in 325 g of CCl4 at 65°C. Given that the vapor pressure of CCl4 at this temperature is 531 mm Hg, what is the vapor pressure of the CCl4–I2 solution at 65°C?
What is the boiling point of a solution containing 0.200 mol of a nonvolatile solute in 125 g of benzene (C6H6)?
You dissolve 15.0 g of sucrose, C12H22O11, in a cup of water (225 g). What is the freezing point of the solution?
A typical bottle of wine consists of an 11% solution (by weight) of ethanol (C2H5OH) in water. If the wine is chilled to −20°C, will the solution begin to freeze?
Estimate the osmotic pressure of human blood at 37°C. Assume blood is isotonic with a 0.154 M NaCl solution, and assume the van’t Hoff factor, i, is 1.90 for NaCl.
What is the boiling point of a solution composed of 15.0 g of urea, (NH2)2CO, in 0.500 kg of water?
What is the boiling point of a solution composed of 15.0 g of CHCl3 and 0.515 g of the nonvolatile solute acenaphthene, C12H10, a component of coal tar?
A solution of glycerol, C3H5(OH)3, in 735 g of water has a boiling point of 104.4°C at a pressure of 760 mm Hg. What is the mass of glycerol in the solution? What is the mole fraction of the solute?
A mixture of ethanol, C2H5OH, and water has a freezing point of −16.0°C.(a) What is the molality of the alcohol?(b) What is the weight percent of alcohol in the solution?
Some ethylene glycol, HOCH2CH2OH, is added to your car’s cooling system along with 5.0 kg of water. If the freezing point of the water–glycol solution is −15.0°C, what mass of HOCH2CH2OH must
An aqueous solution contains 3.00% phenylalanine (C9H11NO2) by mass. (Phenylalanine is nonionic and nonvolatile.) Find the following:(a) the freezing point of the solution(b) the boiling point of the
An aqueous solution containing 1.00 g of bovine insulin (a protein, not ionized) per liter has an osmotic pressure of 3.1 mm Hg at 25°C. Calculate the molar mass of bovine insulin.
Calculate the osmotic pressure of a 0.0120 M solution of NaCl in water at 0°C. Assume the van’t Hoff factor, i, is 1.94 for this solution.
You add 0.255 g of an orange, crystalline compound whose empirical formula is C10H8Fe to 11.12 g of benzene. The boiling point of the benzene rises from 80.10°C to 80.26°C. What are the molar mass
Butylated hydroxyanisole (BHA) is used in margarine and other fats and oils. (It is used as an antioxidant and prolongs the shelf life of the food.) What is the molar mass of BHA if 0.640 g of the
Benzyl acetate is one of the active components of oil of jasmine. If 0.125 g of the compound is added to 25.0 g of chloroform (CHCl3), the boiling point of the solution is 61.82°C. What is the molar
Anthracene, a hydrocarbon obtained from coal, has an empirical formula of C7H5. To find its molecular formula, you dissolve 0.500 g in 30.0 g of benzene. The boiling point of pure benzene is
An aqueous solution contains 0.180 g of an unknown, nonionic solute in 50.0 g of water. The solution freezes at −0.040°C. What is the molar mass of the solute?
Aluminon, an organic compound, is used as a reagent to test for the presence of the aluminum ion in aqueous solution. A solution of 2.50 g of aluminon in 50.0 g of water freezes at −0.197°C. What
If 52.5 g of LiF is dissolved in 306 g of water, what is the expected freezing point of the solution? (Assume the van’t Hoff factor, i, for LiF is 2.)
To make homemade ice cream, you cool the milk and cream by immersing the container in ice and a concentrated solution of rock salt (NaCl) in water. If you want to have a water–salt solution that
List the following aqueous solutions in order of increasing melting point. (The last three are all assumed to dissociate completely into ions in water.)(a) 0.1 m sugar(b) 0.1 m NaCl(c) 0.08 m
Arrange the following aqueous solutions in order of decreasing freezing point. (The last three are all assumed to dissociate completely into ions in water.)(a) 0.20 m ethylene glycol (nonvolatile,
The dispersed phase of a certain colloidal dispersion consists of spheres of diameter 1.0 × 102 nm.(a) What are the volume (V = 4⁄3πr3) and surface area (A = 4πr2) of each sphere?(b) How many
Phenylcarbinol is used in nasal sprays as a preservative. A solution of 0.52 g of the compound in 25.0 g of water has a melting point of −0.36°C. What is the molar mass of phenylcarbinol?
(a) Which aqueous solution is expected to have the higher boiling point: 0.10 m Na2SO4 or 0.15 m sugar?(b) For which aqueous solution is the vapor pressure of water higher: 0.30 m NH4NO3 or 0.15 m
Dimethylglyoxime [DMG, (CH3CNOH)2] is used as a reagent to precipitate nickel ion. Assume that 53.0 g of DMG has been dissolved in 525 g of ethanol (C2H5OH).(a) What is the mole fraction of DMG?(b)
Arrange the following aqueous solutions in order of(i) Increasing vapor pressure of water and(ii) Increasing boiling point.(a) 0.35 m HOCH2CH2OH (a nonvolatile solute)(b) 0.50 m sugar(c) 0.20 m KBr
Making homemade ice cream is one of life’s great pleasures. Fresh milk and cream, sugar, and flavorings are churned in a bucket suspended in an ice–water mixture, the freezing point of which has
A 10.7 m solution of NaOH has a density of 1.33 g/cm3 at 20°C. Calculate the following:(a) The mole fraction of NaOH(b) The weight percent of NaOH(c) The molarity of the solution
Concentrated aqueous ammonia has a molarity of 14.8 mol/L and a density of 0.90 g/cm3. What is the molality of the solution? Calculate the mole fraction and weight percent of NH3.
If you dissolve 2.00 g of Ca(NO3)2 in 750 g of water, what is the molality of Ca(NO3)2? What is the total molality of ions in solution? (Assume total dissociation of the ionic solid.)
If you want a solution that is 0.100 m in ions, what mass of Na2SO4 must you dissolve in 125 g of water? (Assume total dissociation of the ionic solid.)
Consider the following aqueous solutions:(i) 0.20 m HOCH2CH2OH (nonvolatile, nonelectrolyte);(ii) 0.10 m CaCl2;(iii) 0.12 m KBr; and(iv) 0.12 m Na2SO4.(a) Which solution has the highest boiling
(a) Which solution is expected to have the higher boiling point: 0.20 m KBr or 0.30 m sugar?(b) Which aqueous solution has the lower freezing point: 0.12 m NH4NO3 or 0.10 m Na2CO3?
The solubility of NaCl in water at 100°C is 39.1 g/100. g of water. Calculate the boiling point of this solution. (Assume i= 1.85 for NaCl.)
Instead of using NaCl to melt the ice on your sidewalk, you decide to use CaCl2. If you add 35.0 g of CaCl2 to 150. g of water, what is the freezing point of the solution? (Assume i =2.7 for CaCl2.)
The smell of ripe raspberries is due to 4-(p-hydroxyphenyl)- 2-butanone, which has the empirical formula C5H6O. To find its molecular formula, you dissolve 0.135 g in 25.0 g of chloroform, CHCl3. The
Hexachlorophene has been used in germicidal soap. What is its molar mass if 0.640 g of the compound, dissolved in 25.0 g of chloroform, produces a solution whose boiling point is 61.93°C?
The solubility of ammonium formate, NH4CHO2, in 100. g of water is 102 g at 0°C and 546 g at 80°C. A solution is prepared by dissolving NH4CHO2 in 200. g of water until no more will dissolve at
How much N2 can dissolve in water at 25°C if the N2 partial pressure is 585 mm Hg?
Cigars are best stored in a “humidor” at 18°C and 55% relative humidity. This means the pressure of water vapor should be 55% of the vapor pressure of pure water at the same temperature. The
Calculate the enthalpies of solution for Li2SO4 and K2SO4. Are the solution processes exothermic or endothermic? Compare them with LiCl and KCl. What similarities or differences do you find?
An aqueous solution containing 10.0 g of starch per liter has an osmotic pressure of 3.8 mm Hg at 25°C.(a) What is the average molar mass of starch?(The result is an average because not all starch
Vinegar is a 5% solution (by weight) of acetic acid in water. Determine the mole fraction and molality of acetic acid. What is the concentration of acetic acid in parts per million (ppm)? Explain why
Water at 25°C has a density of 0.997 g/cm3. Calculate the molality and molarity of pure water at this temperature.
If a volatile solute is added to a volatile solvent, both substances contribute to the vapor pressure over the solution. Assuming an ideal solution, the vapor pressure of each is given by Raoult’s
A solution is made by adding 50.0 mL of ethanol (C2H5OH, d = 0.789 g/mL) to 50.0 mL of water (d = 0.998 g/mL). What is the total vapor pressure over the solution at 20°C? (See Study Question 75.)
The following table lists the concentrations of the principal ions in seawater:(a) Calculate the freezing point of seawater.(b) Calculate the osmotic pressure of seawater at 25°C. What is the
A 2.0% (by mass) aqueous solution of novocainium chloride (C13H21ClN2O2) freezes at −0.237°C. Calculate the van’t Hoff factor, i. How many moles of ions are in the solution per mole of compound?
A solution is 4.00% (by mass) maltose and 96.00% water. It freezes at −0.229°C.(a) Calculate the molar mass of maltose (which is not an ionic compound).(b) The density of the solution is 1.014
A 2.00% solution of H2SO4 in water freezes at −0.796 °C.(a) Calculate the van’t Hoff factor, i.(b) Which of the following best represents sulfuric acid in a dilute aqueous solution: H2SO4, H3O+
A tree is 10.0 m tall.(a) What must be the total molarity of the solutes if sap rises to the top of the tree by osmotic pressure at 20°C? Assume the groundwater outside the tree is pure water and
A compound is known to be a potassium halide, KX. If 4.00 g of the salt is dissolved in exactly 100 g of water, the solution freezes at −1.28°C. Identify the halide ion in this formula.
Nitrous oxide, N2O, laughing gas, is used as an anesthetic. Its Henry’s law constant is 2.4 × 10−2 mol/kg ∙ bar. Determine the mass of N2O that will dissolve in 500. mL of water, under an N2O
If a carbonated beverage is bottled under 1.5 bar CO2 pressure, what will be the concentration of dissolved CO2 in that beverage? (kH for CO2 is 0.034 mol/kg bar.) After the pressure is released,
You are given a flask filled with a colored liquid. Suggest several tests that would allow you to determine whether this is a solution or a colloid.
A solution of benzoic acid in benzene has a freezing point of 3.1°C and a boiling point of 82.6°C. (The freezing point of pure benzene is 5.50°C, and its boiling point is 80.1°C.) The structure
You dissolve 5.0 mg of iodine, I2, in 25 mL of water. You then add 10.0 mL of CCl4 and shake the mixture. If I2 is 85 times more soluble in CCl4 than in H2O (on a volume basis), what are the masses
If one is very careful, it is possible to float a needle on the surface of water. (If the needle is magnetized, it will turn to point north and south and become a makeshift compass.) What would
A solution of 5.00 g of acetic acid in 100. g of benzene freezes at 3.37°C. A solution of 5.00 g of acetic acid in 100. g of water freezes at −1.49°C. Find the molar mass of acetic acid from each
In a police forensics lab, you examine a package that may contain heroin. However, you find the white powder is not pure heroin but a mixture of heroin (C21H23O5N) and lactose (C12H22O11). To

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