Sulfuric acid is generally sold as a concentrated solution that is 98.7% (by mass) sulfuric acid in water and has a density of 1.84 g/mL.
What is the concentration (in M) of the commercially available concentrated sulfuric acid as described above?
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Sulfuric acid is generally sold as a concentrated solution that is 98.7% (by mass) sulfuric acid...
A concentrated sulfuric acid solution is 65.0% H2SO4by mass and has a density of 1.55 g/mL at 20°C. What is the mass in kg of 3.00 L of the concentrated sulfuric acid solution
A tanker truck carrying 2.01x103 kg of concentrated sulfuric acid solution tips over and spills its load. The sulfuric acid solution is 95.0% H2SO4 by mass and has a density of 1.84 g/mL. Part A Sodium carbonate (Na2CO3) is used to neutralize the sulfuric acid spill. How many kilograms of sodium carbonate must be added to neutralize 2.01x103 kg of sulfuric acid solution? Express your answer with the appropriate units. View Available Hint(s) THRÅ OF ? Value Units Submit
Sulfuric acid is used in the synthesis and processing of many chemicals and metals, and it is the electrolyte in common lead-acid batteries. It is used in various strengths, ranging from concentrated (100%) to dilute; so being able to estimate its concentration from a simple measurement of specific gravity is quite useful. Suppose you prepare a solution that is 20 wt% H2SO4 in water and intend to confirm the concentration by comparing the specific gravity of the solution to that...
The concentrated sulfuric acid we use in the laboratory is 98.0 percentH2SO4 by mass. Calculate the molality and molarity of theacid solution. The density of the solution is 1.83 g/mL.
TReferencer A solution is prepared by adding 49.9 ml concentrated hydrochloric acid and 19.7 ml concentrated nitric acid to 300 ml water More water is added until the final volume is 1.00 L. Calculate H".COH)and the pH for this solution. (Hint: Concentrated HCl is 38% HCI (by mass) and has a density of 1.19 g ml., concentrated HNO, is 70% HNO, (by mass) and has a density of 1.42 g/mL.] OH")= M pH-
SUTULUI 4. Calculate the molarity of a 50% sulfuric acid solution by mass. The density of g/mL. 5. How many grams of CO2 are there in a 250.0 mL sample of sea water if the concentration of CO2 is 295 ppm? Assume the density of sea water is 1.03 g/ml.
c) Initially, a tank is filled with 130 kmol of an aqueous sulfuric acid solution (H2SO4) which contains 5.0 mol% of H2SO4. The solution in the tank is concentrated by adding pure sulfuric acid at a rate of 20.0 L/min. i) Derive an equation to relate the mole balance of sulfuric acid with time. ii) Evaluate the time taken to concentrate the solution to 5%, 35%, 65%, 90% and 95% of H2SO4 and sketch a graph incorporating the values obtained....
The density of a 8.01 m sulfuric acid solution is 1.354 g/mL. What is the molar concentration (molarity) of this solution? The molar mass of sulfuric acid, H2SO4, is 98.98 g/mol A. 6.07 M B.5.26 M C. 0.598 M D.4.20 M
A solution of sulfuric acid contains 43.2% by mass of H2SO4 and has a density of 1.34 g/mL. What is the molarity of H2SO4 in this solution?
A.) An aqueous solution of sulfuric acid is made by dissolving 585.0 g of sulfuric acid in enough distilled water to make a one liter solution. Calculate the molarity, the molality, the mass% and the mole fraction of sulfuric acid in this solution. The density of this solution is 1.350 g/mL. MW H2SO4 = 98.00 g/mol. Please explain!! Thank you B.) Which substance(s) is (are) miscible in water? CH3CH2OH CI4 C6H6 CH3(CH2)13CH2OH CH3OH HOCH2CH2OH