What famous equation was used to determine the first and second K_a for phosphoric acid?
1. If 0.513g of potassium bicarbonate was used to neutralize 35.00mL of phosphoric acid, what was the molarity of the phosphoric acid solution? Is it 0.1464? 2. In order to determine the concentration of a phosphoric acid solution, it was titrated with potassium bicarbonate. Assuming the phosphoric acid reacts completely, write the balanced chemical equation for the reaction between phosphoric acid and potassium bicarbonate.
How would I determine the mmoles of phosphoric acid used in an experiment? experiment details: phosphoric acid 85% in water amount used: 1mL molecular weight: ? density: ?
Phosphoric acid, a mild acid used among other things as a rust inhibitor, food additive, and etching agent for cavity repair by dentists, can be made from elemental phosphorus in a two step process. In the first step, phosphorus and oxygen react to form diphosphorus pentoxide: P4(s) + 502(g) → 2P205(8) In the second step, diphosphorus pentoxide and water react to form phosphoric acid (H2PO4): P2O3(g) + 3 H20(1) ► 2H3PO4(1) Suppose the yield of the first step is 75.%...
Phosphorous acid dissociates to form dihydrogen phosphate and hydronium ion. Phosphorous acid has K_a of 5.0 times 10^2 Write the equation dissociation for phosphorous acid. Express your answer as a chemical equation. Identify all of the phases in your answer. What is the expression constant dissociation for phosphorous acid? K_a = [H_2 PO_3]/[H_3 PO_3] K_a = [H_3 PO_3]/[H_3 O^+] [H_2 PO_3] K_a = [H_3 O^+] [H_2 PO_3]/[H_3 PO_3] K_a = [H_3 O^+] [H_2 PO_3]/[H_2 PO_3]^2
Determination of the dissociation Constant (K_a) of a weak Acid. The pH of a 0.10 M solution of formic acid (HCOOH) is 2.39, what is the K_a of the acid? K_a = Hydrofluoric Acid, A weak Acid with K_a = 7.1 times 10^-4 A. For a 0.50 M solution of HF, calculate the equilibrium concentrations of HF, H^+ and F^-. [HF] = [H^+] = [F^-] = % Dissociation =, pH = B. Now consider a 0.050 M solution of HF....
Name POSTLAB Write the chemical equation for the titration of phosphoric acid (HPOs) with sodium by acid is the acid calculations for this experiment? droxide.(Phosphoric in CocaCola8.) Other than the different molar mass, what would be the difference(s) in the 2. Convert your average mass % acetic acid into: a. The volume % (The density of pure acetic acid is 1.049 g/ml, and the density of vinegar is 1.006 gmL) b. The molarity of acetic acid in vinegar
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 =
Phosphoric acid is a triprotic acid. Write the ionization equation(s) and circle any species that are amphoteric.
If the K_a of a monoprotic weak acid is 5.6 times 10^-6, what is the pH of a 0.46 M solution of this acid? pH = 6.79
For the reaction: phosphoric acid reacts with strontium hydroxide, write a balanced equation including states of matter. What is the formula for the conjugate acid? What is the formula for the conjugate base?