Calculate the pH and PO, concentration in 2.25 M phosphoric acid (H;PO.) solution?H3PO,(aq) + H2O(1) = H;O^(aq) + H,PO, (aq) Ka1 = 7.1×10H2PO, (aq) + H,O(1) = H,O*(aq) + HPO,² (aq) K, 2 = 6.3×10¯HPO (aq) + H,O(1) = H;O*(aq) + PO," (aq) K,3 = 4.2×101³O a. pH = 0.948; [PO,"] = 2.38×10 *° M.onO b. pH = 0.875; [PO,"] = 1.99×10¬1º MOc pH = 0.986; [PO, 1 = 2.56×10¬1ª MO d. pH = 0.924; [PO,"] = 2.22×10¬1° MO e. pH = 0.898; [PO,1 = 2.09×10 1º M

Since H3PO4(aq) is a triprotic acid, it undergoes dissociation 3 times to form 3H+(aq) and…

Calculate the pH and PO, concentration in 2.25 M phosphoric acid (H;PO,) solution? H,PO.(aq) + H,0(1) = H;O*(aq) + H2PO, (aq) K, = ¯ H&PO (aq) + H;O(1) = H,O*(aq) + HPO,*"(aq) K, 2 = 6.3×10¯º HPO (aq) + H,O(1) = H;O^(aq) + PO, (aq) Ka3 = 4.2×10¬" 7.1x10 %3D O a. pH = 0.948; [PO,"] = 2.38×10 1º M. %3D O b. pH = 0.875; [PO,"]= 1.99×10¬1º M Oc. pH = 0.986; [PO,"1 = 2.56×101º M O d. pH = 0.924; [PO,"1 = 2.22× 101º M O e. pH = 0.898; [PO, ] = 2.09×10*° M

Calculate the pH and PO, concentration in 2.25 M phosphoric acid (H;PO,) solution? H,PO.(aq) + H,0(1) = H;O(aq) + H2PO, (aq) K, = ¯ H&PO (aq) + H;O(1) = H,O(aq) + HPO,"(aq) K, 2 = 6.3×10¯º HPO (aq) + H,O(1) = H;O^(aq) + PO, (aq) Ka3 = 4.2×10¬" 7.1x10 %3D O a. pH = 0.948; [PO,"] = 2.38×10 1º M. %3D O b. pH = 0.875; [PO,"]= 1.99×10¬1º M Oc. pH = 0.986; [PO,"1 = 2.56×101º M O d. pH = 0.924; [PO,"1 = 2.22× 101º M O e. pH = 0.898; [PO, ] = 2.09×10° M

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter17: Principles Of Chemical Reactivity: Other Aspects Of Aqueous Equilibria

Section17.6: Equilibria Involving Complex Ions

Problem 2.1ACP: Phosphate ions are abundant in cells, both as the ions themselves and as important substituents on...

See similar textbooks

Similar questions

When acidulated water (dil.H2SO2solution) is electrolysed, will the pH of the solution be affected? Justify your answer.
Estimate the pH of 1.5 x 10-4 M CH3COOH (aq), being careful to treat this solution as dilute, and not open to the approximations used as given below.
Calculate the ph of a solution prepared by dissolving 1.00g of sodium acetate,CH^3COONa, in 50.0ml of 0.15 M acetate acid, CH^3COOH(aq)
Nitrous acid, HNO2 (aq) has a Ka value of 4.0 x 10-4. What is the pH and POH of a 0.0500 M solution of lithium nitrite? (Assumptions may not be valid.)
The pH of human blood is steady at a value of approximately 7.4 owing to the following equilibrium reactions: Acids formed during normal cellular respiration react with the HCO3- to form carbonic acid, which is in equilibrium with CO2(aq) and H2O(l). During vigorous exercise, a person’s H2CO3 blood levels were 26.3 mM, whereas his CO2 levels were 1.63 mM. On resting, the H2CO3 levels declined to 24.9 mM. What was the CO2 blood level at rest?
Calculate the pH of the following acid solutions at 25 °C: (a) 1.0 x 10-4 M H3BO3(aq) (boric acid acts as a monoprotic acid), (b) 0.015 M H3PO4 (aq), (c) 0.10 M H2SO3(aq). Values for the successive acidity constants for each of these acids are given in the below table.
Estimate the pH of 0.010 M NaCH3CO2(aq).
The solution of total volume 0.50 L was prepared by the addition of 0.10 moles of KF to sifficient water. What are the major species of the solution and pH ?
The pH of an aqueous solution of 0.176 M tellurous acid, H2TeO3 (aq), is
Sodium acetate, NaCH3CO2, of mass 7.4 g is used to prepare 250 cm3 of aqueous solution. What is the pH of the solution?
Calculate the pH, pOH, and fraction of solute protonated or deprotonated in the following aqueous solutions: (a) 0.150 M CH3CH(OH)COOH(aq) (lactic acid), (b) 2.4 x 10-4 M CH3CH(OH)COOH(aq), (c) 0.25 M C6H5SO3H(aq) (benzenesulfonic acid). The appropriate values for pKa or pKb are given inthe table.
Calculate the pH of 1.00M acetic acid, HC2H3O2(aq). (Ka = 1.8 x 10-5)