Balance the chemical equation given below, and determine the
number of milliliters of 0.00300 M phosphoric acid required to
neutralize 30.00 mL of 0.00150 M calcium hydroxide.
_____ Ca(OH)2(aq) + _____
H3PO4(aq) → _____
Ca3(PO4)2(aq) + _____
H2O(l)
15.0 mL |
2.02 mL |
10.0 mL |
22.5 mL |
Balance the chemical equation given below, and determine the number of milliliters of 0.00300 M phosphoric...
7. (8 points) Balance the chemical equation given below, and determine the number of milliliters of 0.00300 M phosphoric acid required to react completely 45.00 mL of 0.00150 M calcium hydroxide. Ca(OH)2(aq) + H3PO4(aq) → C a3(PO4)2(aq) + H2O(1)
Consider this equation, describing a titration you performed during the electrolytes lab in Chem 151: 2 H3PO4 (aq) + 3 Ca(OH)2 (aq) → Ca3(PO4)2 (s) + 6 H2O (l) a) Calculate the volume of 0.0500 M phosphoric acid that would be required to exactly react with 20.0 mL of 0.100 M calcium hydroxide b) What mass of calcium phosphate will precipitate?
7) Titrate 20.0 mL of HNO3 with an unknown concentration with 15.4 mL of 0.300M NaOH. Determine HNO3 concentration. Neutralization equation of nitric acid (HNO3) with NaOH is: HNO3 + NaOH + H2O + NaNO3 8) Titrate 25.00 mL of Ca(OH)2 solution with unknown concentration with 15.65 mL of 1.50M H3PO4. Determine the Ca(OH)2 concentration. Neutralization equation of phosphoric acid with calcium hydroxide is: H3PO4 + Ca(OH)2 + H2O + Ca3(PO4)2 (unbalanced)
9. Write a balanced chemical equation for the neutralization of NH3(aq) with HCl(aq). 10. How many moles of sodium hydroxide (NaOH) are needed to neutralize 0.844 mol of acetic acid (HC2H3O2)? (Hint: begin by writing a balanced chemical equation for the process.) 11. How many moles of perchloric acid (HClO4) are needed to neutralize 0.052 mol of calcium hydroxide [Ca(OH)2]? (Hint: begin by writing a balanced chemical equation for the process.) 12. Hydrazoic acid (HN3) can be neutralized by a...
If 47.60 mL of 0.480 M lithium hydroxide is required to neutralize 53.6 mL of phosphoric acid, what is the molarity of the acid? H3PO4(aq)+3LiOH(aq)→Li3PO4(aq)+3H2O(l)
H3PO4 + 3NaOH Na3PO4 + 3H2O How many milliliters of 2.2 M sodium hydroxide would be required to neutralize a 500.0 mL, 3.0 M solution of phosphoric acid?
An aqueous solution of 0.100 M phosphoric acid (12.0 mL) is titrated with 0.400 M KOH as shown below. phosphoric acid has three pKas: 2.148, 7.198, 12.375. H3PO4(aq) + OH-(aq) H2PO4-(aq) + H2O(l) H2PO4-(aq) + OH-(aq) HPO42-(aq) + H2O(l) HPO42-(aq) + OH-(aq) PO43-(aq) + H2O(l) Calculate the pH of phosphoric acid solution before any KOH has been added. We were unable to transcribe this imageWe were unable to transcribe this imageWe were unable to transcribe this image
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)
Consider the following unbalanced equation: H3PO4(aq) + Ca(OH)2(s) → H2O(l) + Ca3(PO4)2(s) If 34.1 moles of H3PO4(aq) reacts with an excess of Ca(OH)2(s), what is the theoretical yield of H2O(l) in moles? O 6.34x102 moles 6.42x102 moles 1.02x102 moles 8.34x102 moles 8.37x102 moles 0 O