6. What is the molarity of a solution that is 26.0 % by mass phosphoric acid...
Question 17 5 points Save Arywer What is the molarity of a solution that is 26.0% by mass phosphoric acid (H3PO4)? The molar mass of H3PO4 i 98.0 g/mol and the density of the solution is 1.155 g/ml a. 3.06 M b. 2.30 M 4.2.30 10M d. 3.00 x 102M e. 0.30 M Which one of the following is a buffer solution? a. HCN and KCN b. HNO3 and NaNO3 O C. HC2H302 and KOH d. HCIO4 and NaClO3 e....
Calculate the molarity and molality of a solution that is 18.0% by mass phosphoric acid (H_3PO_4) and that has a density of 1.155 g/mL.
Calculate the mole fraction of phosphoric acid (H3PO4) in a 25.4% (by mass) aqueous solution. (Assume 750 mL of solution.) What is the molarity of the solution? What is the molality? (At 20 ° C, the density of phosphoric acid is 1.1462 g/mL and the density of water is 0.99823 g/mL.)
what is the molarity of a solution of a phosphoric acid that is made by dissolving 8.00 g of H3PO4 on 0.1 L of water. A.) 0.0816M B.) 0.816 M C.) 0.1 M D.) 1.6 M Write the correct molecular equation, complete ionic equation, and net ionic equation, for the reaction that occurs between cobalt(II)chloride and sodium hydroxide
What is the mole fraction of phosphoric acid in a solution that is 5% by mass phosphoric acid and has a density of 1.025 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)
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 (1) + 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 solution of phosphoric acid with a molality of 7.435 A solution of phosphoric acid with a molality of 7.435 m has a density of 1.780 g/mL. What is the concentration of this solution? Give you answer to four significant figures and don't forget your units Answer:
what is the molarity of a hydrochloric acid solution that is 21.2% HCI by mass and has a density of 2.19 g/ML