Question

In: Chemistry

What is the pH and the equilibrium concentration of PO43- in a 0.511 M solution of...

What is the pH and the equilibrium concentration of PO43- in a 0.511 M solution of H3PO4(aq)? Ka1=7.5*10-3, Ka2=6.2*10-8, Ka3=4.8*10-13

Solutions

Expert Solution

The calculations of this question uploaded as images.

queen_honey_blossom answered 4 weeks ago
Next > < Previous

Related Solutions

What is the concentration of PO43- in a 4.79 M solution of phosphoric acid (H3PO4) at...
What is the concentration of PO43- in a 4.79 M solution of phosphoric acid (H3PO4) at equilibrium? ka1=7.5e-3 ka2=6.2e-8 ka3=4.8e-13 please show work *It's not 5.93e-4 or 3.44e-19
A) What is the pH of a solution with a fluoride concentration of 0.272 M? The...
A) What is the pH of a solution with a fluoride concentration of 0.272 M? The Kb for F- is 1.47 x 10^-11. B) Calculate the pH value of of a 0.015 M solution of pyridine, C5H5N. The Kb of pyridine is 1.7 x 10^-9. Enter your values for a, b, and c for the quadratic equation along with the final answer.
Calculate the pH and the equilibrium concentration of Se2- in a 8.75×10-2 M hydroselenic acid solution,...
Calculate the pH and the equilibrium concentration of Se2- in a 8.75×10-2 M hydroselenic acid solution, H2Se (aq). For H2Se, Ka1 = 1.3×10-4 and Ka2 = 1.0×10-11 pH = [Se2-] = M Calculate the pH and the equilibrium concentrations of HS- and S2- in a 0.0425 M hydrosulfuric acid solution, H2S (aq). For H2S, Ka1 = 1.0×10-7 and Ka2 = 1.0×10-19 pH = [HS-] = M [S2-] = M
What is the equilibrium concentration of PO4 in a 0.511 M solution of H3PO4 (Ka1 =...
What is the equilibrium concentration of PO4 in a 0.511 M solution of H3PO4 (Ka1 = 7.5E-3, ka2= 6.2E-8, ka3= 4.8E-13) I troes using the 5% rule but when i checked my work i was at 11%. I dont know how to solve this if i cant use the 5% rule. Help please.
What is the equilibrium concentration of ammonium ion in a 0.33 M solution of ammonia (NH3,...
What is the equilibrium concentration of ammonium ion in a 0.33 M solution of ammonia (NH3, Kb = 1.8 × 10–5) at 25oC? An initially 1.0 M aqueous solution of a weak monoprotic acid has a total ion concentration of M when equilibrium is established. What is the acid-ionization constant, Ka, of the weak acid? (assume Ca/Ka ≥ 102) For the reaction ΔG°700K = –13.457 kJ. What is Kp for this reaction at 700. K?
Using the aqueous equilibrium constants, calculate the concentration of OH- in M and pH for the...
Using the aqueous equilibrium constants, calculate the concentration of OH- in M and pH for the following solutions (given that all are at 25 degrees celsius): 0.15 M NaBrO 8.2×10−2 M NaHS. A mixture that is 0.13 M in NaNO2 and 0.25 M in Ca(NO2)2. Thank you! :)
What is the pH of a 1.0 M solution of potassium formate, KHCO2? (No equilibrium constant...
What is the pH of a 1.0 M solution of potassium formate, KHCO2? (No equilibrium constant given).
What is the equilibrium Mg2+ concentration when 1.75 L of a 0.153 M magnesium acetate solution...
What is the equilibrium Mg2+ concentration when 1.75 L of a 0.153 M magnesium acetate solution are mixed with 1.69 L of a 0.292 M ammonium carbonate solution? [Mg2+] =
Calculate the pH of a 5.0 M H3PO4 solution and the equilibrium concentrations of the species...
Calculate the pH of a 5.0 M H3PO4 solution and the equilibrium concentrations of the species H3PO4, H2PO4-, HPO42- and PO43- (ka1 = 7.5 x 10-3, ka2 = 6.2 x 10-8, ka3 = 4.8 x 10-13)
What is the concentration of a NH3 solution having a pH of 11.15?
What is the concentration of a NH3 solution having a pH of 11.15?
ADVERTISEMENT
Subjects
ADVERTISEMENT
Latest Questions
ADVERTISEMENT