General Chemistry: Principles and Modern Applications (11th Edition)
11th Edition
ISBN: 9780132931281
Author: Ralph H. Petrucci, F. Geoffrey Herring, Jeffry D. Madura, Carey Bissonnette
Publisher: PEARSON
expand_more
expand_more
format_list_bulleted
Concept explainers
Videos
Textbook Question
Chapter 14, Problem 135SAE
What is the osmotic pressure, in bar, of 15.2L of a 0.312M starch solution at
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Students have asked these similar questions
3. A bacteria is able to grow on hexadecane as a substrate:
C16H34 + 16.28 O2 + 1.42 NH3 →1.65 C4.4HBO₂N8 + a CO₂ + 13.11 H₂O
(a) What is the respiratory quotient (mol/mol)?
(b) What is the cell formula for this microorganism?
(c) Assuming 100% conversion, calculate the yield of cells from hexadecane (Yx/s) and from oxygen
(YX/0₂).
When a Vitamin C (ascorbic acid; MM = 176.12 g mol-1) tablet is crushed, dissolved and titrated with 0.0340 M KIO3(aq) to a purple/blue endpoint (given by a starch indicator), the volume of KIO3 used is 29.80 mL. If 60 mg of ascorbic acid is the recommended dietary allowance (i.e., 100% of the RDA), then what is the % RDA for the Vitamin C in the tablet?
KIO3(aq) + 5 KI + 6 H+ → 3 I2(aq) + 3 H2O
I2 (aq) + ascorbic acid → 2 I- + dehydroascorbic acid
(Q71) The osmotic pressure of a solution containing 24.1 mg of an unknown protein dissolved in
8.57 mL of solution is 2.08 torr at 37°C. What is the molar mass (in g/mol) of this unknown protein?
(The molar mass of the protein will be relatively high - express to 5 sig figs).
Chapter 14 Solutions
General Chemistry: Principles and Modern Applications (11th Edition)
Ch. 14 - Which of the following do you expect to be most...Ch. 14 - Which of the following is moderately soluble both...Ch. 14 - Substances that dissolve in water generally do not...Ch. 14 - Prob. 4ECh. 14 - Two of the substances listed here highly soluble...Ch. 14 - Benzoic acid, C8H8COOH, is much more soluble in...Ch. 14 - Prob. 7ECh. 14 - Explain the observation that all metal nitrates...Ch. 14 - A saturated aqueous solution of NaBr at 20C...Ch. 14 - Prob. 10E
Ch. 14 - Prob. 11ECh. 14 - You are asked to prepare 125.0 mL of 0.0321 M...Ch. 14 - Prob. 13ECh. 14 - Prob. 14ECh. 14 - Prob. 15ECh. 14 - Prob. 16ECh. 14 - The sulfate ion level in a municipal water supply...Ch. 14 - A water sample is found to have 9.4 ppb of...Ch. 14 - Prob. 19ECh. 14 - Prob. 20ECh. 14 - How many milliliters at the ethanol-water solution...Ch. 14 - Prob. 22ECh. 14 - What is the molarity of CO2 in liter ocean water...Ch. 14 - Prob. 24ECh. 14 - Prob. 25ECh. 14 - Prob. 26ECh. 14 - How many grams of iodine, l2 , must be dissolved...Ch. 14 - How many grams of water would you add to 1.00 kg...Ch. 14 - Prob. 29ECh. 14 - A 10.00%-by-man solution of ethanol, CH2CH2OH , in...Ch. 14 - Prob. 31ECh. 14 - Prob. 32ECh. 14 - Prob. 33ECh. 14 - Prob. 34ECh. 14 - What volume of glycerol,...Ch. 14 - Prob. 36ECh. 14 - Prob. 37ECh. 14 - The amount of CO2 in the ocean is approximately...Ch. 14 - Prob. 39ECh. 14 - Prob. 40ECh. 14 - Prob. 41ECh. 14 - Prob. 42ECh. 14 - Under an O2(g) pressure of 1.00 atm, 28.31mL of...Ch. 14 - Prob. 44ECh. 14 - Natural gas consists about 90% methane, CM. Assume...Ch. 14 - At 1.00 atm, the solubility of O2 in water is...Ch. 14 - The aqueous solubility at 20C of Ar at 1.00 atm...Ch. 14 - Prob. 48ECh. 14 - Prob. 49ECh. 14 - Prob. 50ECh. 14 - What are the partial and total vapor pressures of...Ch. 14 - Prob. 52ECh. 14 - Calculate the vapor pressure at 25C of a solution...Ch. 14 - Calculate the vapor pressure at 20C of a saturated...Ch. 14 - Styrene, used in the manufacture of polystyrene...Ch. 14 - Prob. 56ECh. 14 - A benzene-toluene solution with banz=0.300 has a...Ch. 14 - Prob. 58ECh. 14 - Prob. 59ECh. 14 - Prob. 60ECh. 14 - Prob. 61ECh. 14 - Prob. 62ECh. 14 - Prob. 63ECh. 14 - Prob. 64ECh. 14 - Prob. 65ECh. 14 - Use the concentration of an istonic solution,...Ch. 14 - Prob. 67ECh. 14 - The two solutions pictured here are separated by a...Ch. 14 - of an unknown compound reduces e freezing point of...Ch. 14 - Prob. 70ECh. 14 - Prob. 71ECh. 14 - Prob. 72ECh. 14 - A compound is 42.9% C, 2.4% H, 16.7%N, and 38.1%...Ch. 14 - Nicotinamide is a water-soluble vitamin important...Ch. 14 - Prob. 75ECh. 14 - Coniferin is glycoside (a derivative of a sugar)...Ch. 14 - Cooks often add some salt to water before boding...Ch. 14 - An important test for the purity of an organic...Ch. 14 - Prob. 79ECh. 14 - If ocean water consisted of 3.5% salt, what would...Ch. 14 - Predict the approximate freezing points of 0.10m...Ch. 14 - Calculate the van’t Hoff factors of the following...Ch. 14 - NH2(aq) conducts electric current only weakly. The...Ch. 14 - Prob. 84ECh. 14 - Prob. 85ECh. 14 - Prob. 86ECh. 14 - Prob. 87IAECh. 14 - Prob. 88IAECh. 14 - Prob. 89IAECh. 14 - Prob. 90IAECh. 14 - A solid mixture consists of 85.0% KNO2 and 15.0%...Ch. 14 - Suppose you have available 2.50 L of a solution (d...Ch. 14 - Prob. 93IAECh. 14 - Prob. 94IAECh. 14 - Prob. 95IAECh. 14 - Nitrobenzene, C6H2NO2 , and benzene, C6H8 , are...Ch. 14 - Prob. 97IAECh. 14 - Prob. 98IAECh. 14 - Prob. 99IAECh. 14 - Suppose that I 00mg of gold obtained in a...Ch. 14 - At 20C , liquid benzene has a density of...Ch. 14 - The two compounds whose structures are depicted...Ch. 14 - Prob. 103IAECh. 14 - Prob. 104IAECh. 14 - Prob. 105IAECh. 14 - We noted m Figure 14-17 that the liquid and vapor...Ch. 14 - A saturated solution prepared at 70C contains...Ch. 14 - Prob. 108IAECh. 14 - Prob. 109IAECh. 14 - Prob. 110IAECh. 14 - Prob. 111IAECh. 14 - Prob. 112IAECh. 14 - Prob. 113FPCh. 14 - The phase diagram shown is for mixtures of HCI and...Ch. 14 - The laboratory device pictured on the following...Ch. 14 - Prob. 116FPCh. 14 - Prob. 117SAECh. 14 - Briefly describe each of the following ides or...Ch. 14 - Explain the important distinctions between each...Ch. 14 - Prob. 120SAECh. 14 - Prob. 121SAECh. 14 - Prob. 122SAECh. 14 - Prob. 123SAECh. 14 - An ideal liquid solution has two volatile...Ch. 14 - Prob. 125SAECh. 14 - Prob. 126SAECh. 14 - A solution (d=1.159g/mL) is 62.0% glycerol,...Ch. 14 - Prob. 128SAECh. 14 - Prob. 129SAECh. 14 - Prob. 130SAECh. 14 - Prob. 131SAECh. 14 - Prob. 132SAECh. 14 - Prob. 133SAECh. 14 - What is the mole fractions of a monvolatile solute...Ch. 14 - What is the osmotic pressure, in bar, of 15.2L of...Ch. 14 - What is the weight percent of 23.4 g of CaF2 if...Ch. 14 - Prob. 137SAECh. 14 - Prob. 138SAE
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- (a) A commercial 737 jet transporting 143 passengers and 5 crew members from Kansas City (MCI) to Baltimore (BWI) burned 11,800 lb (about 1700 gallons) of Jet A fuel en route. Jet A fuel is kerosine based, consisting primarily of CnH2n+2 hydrocarbons, with n =6 to 16, so the carbon:hydrogen ratio is close to 1:2. During this flight, how much CO2 was released into the atmosphere? Assume the combustion of the fuel was complete, so all the fuel was burned to form CO2 and H2O. Give both the mass of CO2 produced (in kg and in lbs) and the volume it would occupy at 298 K, 1 atm.(b) How much CO2 would be released into the atmosphere if those passengers and crew made the trip instead, in pairs, in hybrid cars at 40 miles per gallon. Assume the density of the gasoline is 0.75 kg L-1 and that carbon and hydrogen dominate the composition in a ratio of 1:2. The road trip is 1082 miles.arrow_forward(d) A sample contains a mixture of ammonium carbonate (NH4)2CO3, sodium carbonate Na2CO3, and sodium chloride NaCl. Thermogravimetric analysis indicates that a 0.0965-g portion of this sample loses 0.0574 g over a temperature range of 50-75 oC and then loses another 0.0124 g at 800 oC.(i) What causes the weight loss at 50-75 oC? (ii) What species will remain after being heated to 800 oC? (iii) What is the composition of the original sample? Given: Atomic masses: H = 1.008; C = 12.011; N = 14.007; Na = 22.99; O = 15.999;Cl = 35.45.arrow_forwardDissolve 0.25g NaClI, 0.20g NaHCO3. 0.35g KCI, and 1.5g of glucose in 100 ml distilled water using a 250 mL capacity beaker. Use the formula to create a 60 mL ORS. Based on the given procedure, calculate the total amount of glucose in the prepared solution. (MW: Na: 23, K: 39, CI: 35, H: 1, C: 12, 0: 16) O 83.33 mmol/L 66.91 mmol/L 90.40 mmol/L 71.11 mmol/L O 23.81 mmol/L O 47.30 mmol/Larrow_forward
- 2. Calculate the enthalpy of hydration of CuSO, if 16.34 g of CUSO, dissolves in water and gives out 55.51 kJ of heat (Q) and 25.17 g of CuSO4 • SH;O dissolves in water and absorbs 95.31 kJ of heat (Q). The molecular weight for CusO, is 160.00 g/mol, CusO, • SH;0 is 250.00 g/mol. Show ALL calculations-no calculations, no credit! CusO, (s) excess H,O Cu" (aq) so- (aq) AH1 + SH;0 АНа АНа excess H;0 CusO4 • SH20 (s)arrow_forwardAlthough other solvents are available, dichloromethane(CH₂Cl₂) is still often used to “decaffeinate” drinks because thesolubility of caffeine in CH₂Cl₂ is 8.35 times that in water.(a) A 100.0-mL sample of cola containing 10.0 mg of caffeine is extracted with 60.0 mL of CH₂Cl₂. What mass of caffeine re-mains in the aqueous phase? (b) A second identical cola sampleis extracted with two successive 30.0-mL portions of CH₂Cl₂.What mass of caffeine remains in the aqueous phase after each extraction? (c) Which approach extracts more caffeine?arrow_forwardCalculate the molar concentration of a thiosulfate solution from the following information:A 40.-mL aliquot of a 0.00653 M KIO3 solution is added to a flask containing 2 g of KI and 10 mL of 0.5 M H2SO4. The resulting solution is titrated to a starch endpoint with 38 mL of the thiosulfate solution.arrow_forward
- Oral rehydration salts are stated to contain the following components: Sodium Chloride 3.5g Potassium Chloride 1.5g Sodium Citrate 2.9g Anhydrous Glucose 20.0g 8.342 g of oral rehydration salts are dissolved in 500 ml of water. 5 ml of the solution is diluted to 100 ml and then 5 ml is taken from the diluted sample and is diluted to 100 ml. The sodium content of the sample is then determined by flame photometry. The sodium salts used to prepare the mixture were: Trisodium citrate hydrate (C6H5Na3O7, 2H2O) MW 294.1 and sodium chloride (NaCl) NW 58.5. Atomic weight of Na = 23. The content of Na in the diluted sample was determined to be 0.3210 mg/100 ml. Determine the % of stated content of Na in the sample. The stated should be 104.5, how??arrow_forward(Q68) What mass (in grams) of ethylene glycol (C2H6O2) must be added to 1,296 grams of water to lower the freezing point to -1.10 °C? (3 sf)arrow_forward(1) (2) ] A certain species of trout requires dissolved oxygen of 7.5 mg/L. Would it be wise to release the trout in a mountain stream at an altitude with a Po2 = 0.17 atm. (KH (02) = 1.3x10-³ mol/Latm). Calculate the mole fraction for the following: 14.5 g of HNO3 in 150 g of H₂O. (b) moles of Solute kg Solvent X (a) H=1.01 N = 14.00- 50 mm= 63.01 g/mol 03=16.0x3 Imol 14.6g HNO3 63.01g 149 150 g 1000g = 0.15 kg 6.00 M HCI. (notice, concentration is an extensive property. You can assume any volume!) 0.23 mol HNO3 0.16 kg H2O 1.53 = 0.23 mol HNO3arrow_forward
- Oral rehydration salts are stated to contain the following components: Sodium Chloride 3.5g Potassium Chloride 1.5g Sodium Citrate 2.9g Anhydrous Glucose 20.0g 8.342 g of oral rehydration salts are dissolved in 500 ml of water. 5 ml of the solution is diluted to 100 ml and then 5 ml is taken from the diluted sample and is diluted to 100 ml. The sodium content of the sample is then determined by flame photometry. The sodium salts used to prepare the mixture were: Trisodium citrate hydrate (C6H5Na3O7, 2H2O) MW 294.1 and sodium chloride (NaCl) NW 58.5. Atomic weight of Na = 23. The content of Na in the diluted sample was determined to be 0.3210 mg/100 ml. Determine the % of stated content of Na in the sample.arrow_forwardThe ethyl acetate concentration in an alcoholic solution was determined by diluting a 10.00-mL sample to 100.00 mL. A 19.00-mL portion of the diluted solution was refluxed with 40.00 mL of 0.04601 M KOH: CH3 СОО С2H; + ОН — СH3 COO + C2H; ОН After cooling, the excess OH was back-titrated with 3.02 mL of 0.05056 M H2 SO4. Calculate the amount of ethyl acetate (88.11 g/mol) in the original sample in grams. Amount of ethyl acetate =arrow_forwardThe calcium (AW= 40.08 g/mol) from a sample of limestone weighing 607.4 mg was precipitated as calcium oxalate hydrate (CaC204.H20, FW 146.12 g/mol) and ignited to calcium carbonate (CaCO3, FW= 100.09 g/mol) weighing 246.7 mg. (c) If the precipitate had been ignited at a higher temperature giving calcium oxide (CaO, FW= 56.08 g/mol), what would be its weight?arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Solutions: Crash Course Chemistry #27; Author: Crash Course;https://www.youtube.com/watch?v=9h2f1Bjr0p4;License: Standard YouTube License, CC-BY