To carry out a reaction, 20 mL of a solution of sulfuric acid (H2SO4) having a density of 1.84 g / mL and 85% by weight of the solute was used. Calculate the grams of H2SO4 that were used.
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To carry out a reaction, 20 mL of a solution of sulfuric acid (H2SO4) having a...
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....
A solution is prepared by dissolving 27.75 g sulfuric acid, H2SO4, in enough water to make exactly 200.0 mL of solution. If the density of the solution is 1.1094 g/mL, what is 1. Weight % of H2SO4 in the solution? 2. Mole fraction of H2SO4 in the solution? 3. Molarity of H2SO4 in the solution? 4. Molality of H2SO4 in the solution?
Density of a 3.75 M sulfuric acid (H2SO4) solution is 1.23 g/ml. Calculate its mass %, XH2SO4, molality & normality.
5. Sodium bicarbonate (baking soda) will neutralize sulfuric acid according to the following reaction: 2 H200) + 2 CO2()+ Na2SOs(aq) 2 NAHCO3(aq)+H2SO4(aq) If a student spills 250.0 mL of sulfuric acid, how many grams of sodium bicarbonate should they use in order to completely neutralize it? Assume the density of sulfuric acid is 1.84 g/m L.
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 sulfuric acid solution containing 571.6 g of H2SO4 per liter of solution has a density of 1.329 g/cm3. Calculate the following quantities for the solute in this solution. 9 pts 1. i. Mass percent ii. Molality iii. Molarity Table 1. Reference data Density @ Vapor Normal 20°C Pressure (torr) H20 1.86 0.00 0.512 100.00 0.998 17.5 2.53 80.1 0.8765 98.5 Normal point (oC) lKb value) boiling! (PC/m) point (C) Substance Formula Formula Kr value* Krvalue -20°C (°C/m) freezingb (g/mL)...
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?
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
a sulfuric acid solution containing 551.5 (a) A sulfuric acid solution containing 551.5g of H2SO4 per liter of Solution has a density of 1-339 Icme. Calculate molality of HaSO4 in this solution. the
2. Given 3.98 mL of sulfuric acid (98.0%) calculate the number of mmols in the solution. (MW H2SO4: 98.08 g/mol, density: 1.840 g/mL) 3. Given 7.04 g of HBr calculate the volume (mL) of a 48.0% solution. (MW HBr: 80.91 g/mol, density: 1.49 g/mL)