... متعد د الخيارات What is the volume of sulfuric acid H2S04 needed to prepare a dilute solution of it with a volume of 1 liter and a concentration of 1 N if you know that the Specific Gravity = 1.84,% = 98, H = 1, S = 32, 0 = 16 27.17ml 17.27ml 12.77ml 77.12ml STRY سياء التي تهتم بدر( 155

... متعد د الخيارات What is the volume of sulfuric acid H2S04 needed to prepare a dilute solution of it with a volume of 1 liter and a concentration of 1 N if you know that the Specific Gravity = 1.84,% = 98, H = 1, S = 32, 0 = 16 27.17ml 17.27ml 12.77ml 77.12ml STRY سياء التي تهتم بدر( 155

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Grams of solute per 100 g H₂O 5870 1. 2. 150 140 130 120 110 100 3. 90 80 4. 60 50 40 30 20 10 X KI NH₂ NaNO3 KCIÓ -Ce₂(SO4)3 0 0 10 20 30 40 50 60 70 80 90 100 Temperature (°C) The graph below shows how temperature affects the solubility of select compound. Answer the questions that follow using this graph. Question 7 options: KNO3 NH,C KCI Naci KI NaCl Ce₂(SO4)3 128 g Substance whose solubility is least affected by temperature lonic compound whose solubility decreases with increasing temperature. Compound with the highest solubility at 20 °C Amount of KNO3 that will dissolve in 100 g H₂0 at 70 °C
Calculate the number of moles of H2O2 in 450ml of a 35% H2O2 solution. Molar mass of H2O2 = 34 Report your answer to 3 significant figures. Do not include the unit when writing your answer.
A certain substance X has a normal freezing point of - 5.2 °C and a molal freezing point depression constant K, = 1.97 °C- kg mol. Calculate the freezing point of a solution made of 38.70 g of urea ((NH,),Co) dissolved in dlo 900. g of X. Round your answer to 2 significant digits. Ar х10 ?
At 25 C, a solution is prepared by dissolving 22.1 grams of toluene, C,H, in 250.0 mL of benzene, C,H, density 0.866 g/mL. For your calculations use 12.0 as the molar mass of carbon, and 1.00 as the molar mass of hydrogen. Calculate the mole fraction of benzene Calculate the mole fraction of toluene Calculate the mass percent of benzene Calculate the mass percent of toluene Calculate the concentration of benzene in ppm Calculate the concentration of toluene in ppm Calculate the molality of toluene in the solution What type of intermolecular force would exist between benzene and toluene What type of intermolecular force would exist between two molecules of benzene What type of intermolecular force would exist between two molecules of toluene
Assuming that the volumes are additive, what volume of water must be added to 35mL of 15% KOH to make a solution which is 10%?
[References] What is the composition of a methanol (CH; OH) – propanol (CH, CH, CH, OH) solution that has a vapor pressure of 192 torr at 40°C? At 40°C, the vapor pressures of pure methanol and pure propanol are 303 and 44.6 torr, respectively. Assume the solution is ideal. Mole fraction of methanol Mole fraction of propanol
The solubility in water of ionic compound X is measured and found to be 38.7 at 10. °C. Calculate the volume of a saturated solution of X in water that would L contain 420. mg of X at this temperature. Be sure your answer has the correct unit symbol and 3 significant digits. x10 ?
D) 1.32 m E) 3.29 x 10-1 m 4 13)** Determine the freezing point of a solution that contains 78.8 g of naphthalene (C10H8, molar mass = 128. g/mol) dissolved in 722 mL of benzene (d = 0.877 g/mL). Pure benzene has a melting point of 5.50°C and a freezing point depression constant of 4.90°C/m. A) 4.76°C %3D B) 1.33°C C) 1.68°C D) 0.74°C E) 4.17°C 14) ** Which of the following will have the lowest freezing point when dissolved in water?
The freezing point of 59.49 g of a pure solvent is measured to be 44.96 ºC. When 2.18 g of an unknown solute (assume the van 't Hoff factor = 1.0000) is added to the solvent the freezing point is measured to be 42.65 ºC. If the freezing point depression constant of the pure solvent is 7.66 ºC·kg solvent/mol solute calculate the molar mass of the solute. ?=g/mol
Ben prepared a salicylic acid in pentanol solution by adding 4.77 g of salicylic acid to 91.88 mL of pentanol. Calculate the mole fraction of salicylic acid in this solution. MW of salicylic acid= 138.12 g/mol MW of pentanol= 88.15 g/mol Density of pentanol= 0.8144 g/mL
What would be the boiling point of a solution formed by adding 1.0 mole of sucrose (a molecular compound) to the following amounts of water? Make your answer with 1 decimal place (uncertainty of ± 0.1). a) 250 g (0.25 kg) b) 2000 g (2.000 kg)
Calculate the freezing point of a 14.00?14.00m aqueous solution of methanol. Freezing point constants can be found in the list of colligative constants. Solvent Formula K f value* (°C/ m ) Normal freezing point ( °C) K b value (°C/ m ) Normal boiling point ( °C) water H 2 O 1.86 0.00 0.512 100.00 benzene C 6 H 6 5.12 5.49 2.53 80.1 cyclohexane C 6 H 12 20.8 6.59 2.92 80.7 ethanol C 2 H 6 O 1.99 –117.3 1.22 78.4 carbon tetrachloride CCl 4 29.8 –22.9 5.03 76.8 camphor C 10 H 16 O