Density is 2.4 g/mL
1000 mL (1 L ) of solution contains g of solution.
The weight percent of solution is 48.0 wt%
2400 g of solution contains g of phosphoric acid.
The molecular weight of phosphoric acid is 98 g/mol.
The number of moles of phosphoric acid moles.
Since total volume is 1 L, the number of moles is equal to molar concentration.
The ionic strength
Calculate the ionic strength of a 48.0 wt% phosphoric acid, if the phosphoric acid has a...
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)
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.)
An aqueous solution of phosphoric acid, that is 0.500 percent by weight phosphoric acid, has a density of 1.0010 g/mL. A student determines that the freezing point of this solution is -0.129 °C. Based on the observed freezing point, what is the percent ionization of the acid and the value of Ka1? Assume that only the first ionization of the acid is important. Kf for H2O is 1.86 °C/m. % ionized = % Ka1 =
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 mole fraction of phosphoric acid in a solution that is 5% by mass phosphoric acid and has a density of 1.025 g/mL
Acid-base titration questions. Please help! Thanks. 2. Given that 20.00 mL of phosphoric acid solution required 15.50 mL of 0.200M NaOH for the first equivalent point. What is the molarity of the phosphoric acid? 3. A student titrated 25.00 mL of cola and it required 18.27 mL of 0.0100 M NaOH to reach the 1'equivalence point. Calculate the molar concentration of phosphoric acid in this brand of cola. 4. If the density of the "Cola" drink is 1.00 g/mL. What...
I'm having trouble with these questions from the lab: polyprotic acids: titration of phosphoric acid and determination of the molar concentration of phosphoric acid in cola. 3.A student titrated 25.00 mL of cola and it required 18.27 mL of 0.0100 M NaOH to reach the 1st equivalence point. Calculate the molar concentration of phosphoric acid in this brand of cola. 4. If the density of the "Cola" drink is 1.00 g/mL. What is the mass percent of phosphoric acid in...