Calculate the weight of H2SO4 in 25 mL of concentrated acid that has a specific gravity of 1.84 and purity of 97%
Calculate the weight of H2SO4 in 25 mL of concentrated acid that has a specific gravity...
the specific gravity concentrated hydrochloric acid is 1.18. If 25 grams is needed for an experiment what is the volume that would be used ?
Concentrated sulfuric acid has a density of 1.76 g/cm3 and is 84.0% by weight H2SO4 . What is the molality of this acid?
Concentrated HCL is 37.5% by weight and has a density of 1.19g/ml. Calculate the (a) molarity of the concentrated acid (b) mL of concentrated HCL required to make 500mL of 0.2 HCl (c) ml of concentrated HCL required to make 350 ml of 0.5 N HCL
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.
Concentrated hydrochloric acid is 38% HCl by weight and has a density of 1.19 g/mL. A solution is prepared by measuring 67 mL of the concentrated HCl, adding it to water, and diluting to 0.800 L. Calculate the approximate molarity of this solution from the volume, percent composition, and density.
Cadliy U.2JI2Cl 207nu will ILS THUlalily! 4. Concentrated sulfuric acid has a density of 1.83 g/mL. If the concentrated acid is 97% H2SO4, what is its molarity and normality? TE ! noneontatado adil.dadah dimillad... n
Given 1.0 mL of methyl benzoate, 3.0 mL conc. H2SO4, 1.0 mL of concentrated nitric acid calculate thr theoretical yield of of methyl 3-nitrobenzoate
Concentrated hydrochloric acid is 38% HCl by weight and has a density of 1.19 g/mL. A solution is prepared by measuring 36 mL of the concentrated HCI, adding it to water, and diluting to 0.500 L. Calculate the approximate molarity of this solution from the volume, percent composition, and density. Answer:
You need a 5% HCL solution. The concentrated HCL available has a specific gravity of 1.19 and an assay of 37%. How would you make 100 mL of the needed soulution? (MW HCL = 36.5)
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....