Calculate the pH of the following aqueous solution: 0.17MHOCl (pKa= 7.46)
Select one:
a. 9.89
b. 4.11
c. 5.77
d. 8.23
We need at least 10 more requests to produce the answer.
0 / 10 have requested this problem solution
The more requests, the faster the answer.
Calculate the pH of the following aqueous solution: 0.17MHOCl (pKa= 7.46) Select one: a. 9.89 b....
Which of the following 0.10 M aqueous solutions gives the highest pH? A) CH3COOH (pKa = 4.75) B) HF (PK:= 3.45) C) H3PO4 (pKal = 2.12) D) HCIQ (Ka=2.00) E) Since all are acids, the pH is the same for all solutions. 5. Which one of the following salts gives an acidic aqueous solution? A) CsNO3 B) CaCl2C ) LiF D) Cr(CIO4)3 E) NaCH3CO2 6. 7. All of the following are strong acids except A) HCIQB) HC104 C) HI D)...
1. Calculate the concentration of H3O+ for an aqueous solution with a pH of 1.2 A) 6.3 x 10-7M B ) 1.6 x 108 M. C) 1.0 x 10-14 M. D) 6.20 x 10-2 M E) 4.0 x 10-4M 2. Calculate the concentration of OH- for an aqueous solution with a pH of 13.8. A) 0.64 M B) 4.0 x 10-5M C) 1.5 x 10-5M D) 1.0 x 10-14 M E) 2.5 x 10-10 M 3. Which of the following...
In an aqueous solution of a certain acid with pKa = 7.33 the pH is 4.59. Calculate the percent of the acid that is dissociated in this solution. Round your answer to 2 significant digits.
Calculate the approximate pH of an aqueous solution of sodium carbonate Na2CO3 , 0.28 M, at 25°C. (Note: consider one decimal place for the pH answer.) pKa H2CO3 /HCO3− = 6.35, pKa HCO3- /CO32-= 10.30
Calculate the concentrations of the molecular and ionic species and the pH in aqueous solution that has a formal composition of 0.2350 M KH2PO4 + 0.4300 M K2HPO4. ph of 7.46 What is the concentration of the molecular species H3PO4?
Calculate the approximate pH of an aqueous solution of a mixture of CH3COOH, 0.27 M, and CH3COONa, 0.15 M, at 25°C. (Note: consider one decimal place for the pH answer.) pKa = 4.76.
Calculate the approximate pH of an aqueous solution of ammonium chloride, NH4Cl , 0.03 M, and sodium acetate, CH3COONa, 0.12 M at 25°C. (Note: consider one decimal place for the pH answer.) pKa NH4+/NH3 = 9.24 pKa CH3COOH/CH3COO- = 4.76
Calculate the pH and pOH of the following aqueous solutions: (a) 0.15 mol·L–1 CH3COOH(aq); (b) 0.15 mol·L–1 CCl3COOH (aq); (c) 0.15 mol·L–1 HCOOH(aq). When the pH of a 0.10 mol·L–1 HClO2 aqueous solution was measured, it was found to be 1.2. What are the values of Ka and pKa of chlorous acid? (b) The pH of a 0.10 mol·L–1 propylamine, C3H7NH2, aqueous solution was measured as 11.86. What are the values of Kb and pKb of propylamine?
Calculate the pH and pOH of the following aqueous solutions: (a) 0.15 mol·L–1 CH3COOH(aq); (b) 0.15 mol·L–1 CCl3COOH (aq); (c) 0.15 mol·L–1 HCOOH(aq). When the pH of a 0.10 mol·L–1 HClO2 aqueous solution was measured, it was found to be 1.2. What are the values of Ka and pKa of chlorous acid? (b) The pH of a 0.10 mol·L–1 propylamine, C3H7NH2, aqueous solution was measured as 11.86. What are the values of Kb and pKb of propylamine?
Calculate the approximate pH of an aqueous solution of H2S , 0.05 M, and H3PO4, 0.21 M at 25°C. (Note: consider one decimal place for the pH answer.) pKa H2S/HS- = 7.02, pKa HS-/S2- = 13.99 pKaH3PO4/ H2PO4- =2.15, pKaH2PO4-/HPO42-=7.15, pKa HPO42-/ PO43- =12.38