Commercially available concentrated phosphoric acid is 15.2M . Calculate the volume of concentrated phosphoric acid required to prepare 1.50 L of 1.50M solution.
Volume = L
Commercially available concentrated phosphoric acid is 15.2M . Calculate the volume of concentrated phosphoric acid required...
A test procedure requires 500mL of a 4N phosphoric acid solution. The concentrated phosphoric acid available has a specific gravity of 1.69 and an assay of 85%. How would you prepare this solution? (MW H3PO4 = 98) (Valence is 3)
Calculate the volume in milliliters of a 6.00 N phosphoric acid solution that would contain 35.0 g of phosphoric acid.
2. a. Both concentrated sulfuric acid and concentrated phosphoric acid are known to catalyze the conversion of cyclohexanol to cyclohexene via dehydration reaction. Concentrated hydrochloric acid, however, is not a viable option. Provide two reasons on what make sulfuric acid and phosphoric acid advantageous over hydrochloric acid. Look up additional information on these acids if needed. b. In preparation of the bromohydrin (trans-2-bromo-1-methylcyclohexanol) with bromine, side products dibromides shown below are often observed. This side reaction can be essentially avoided...
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?
Nitric acid, HNO3, is available commercially at a concentration of 16 M. What volume would you need to obtain 0.100 mol HNO3?
Calculate the concentration of phosphoric acid in a solution if 25.0 mL of that solution required 35.2 mL of 0.189 M KOH for neutralization
A 10.00 mL sample of phosphoric acid is titrated with 20.15 mL of a 2.50 mol/L sodium hydroxide solution. H3PO4 (aq) + NaOH ----> H2O (l) + Na3PO4 (aq) a) Balance the molecular equation and write the net ionic equation. b) calculate the molarity of phosphoric acid. c) calculate the mass percent of phosphoric acid in the water mixture (density = 1.50 g/mL)
A 10.00 mL sample of phosphoric acid is titrated with 20.15 mL of a 2.50 mol/L sodium hydroxide solution. H3PO4 (aq) + NaOH ----> H2O (l) + Na3PO4 (aq) a) Balance the molecular equation and write the net ionic equation. b) calculate the molarity of phosphoric acid. c) calculate the mass percent of phosphoric acid in the water mixture (density = 1.50 g/mL)
1. Glucose (C6H12O6, M= 180.16 g/mol) solutions are commercially available. A concentrated sample of an aqueous glucose solution has a density of 1.25 g/mL and contains 55.0 % glucose by mass at 20 °C a) What is the molarity of this glucose solution? b) What is the molality of this solution? c) What is the mole fraction of glucose in this solution?
If concentrated phosphoric acid is 14.7 M, how many ml of acid would you use to make 400 ml of 2N phosphoric acid?