Determine the pH of a 0.188 M NH3 solution at 25°C. The Kb of NH3 is 1.76 × 10-5.
20) Determine the pH of a 0.188 M NH3 solution at 25°C. The K of NH3 is 1.76 x 10-5. 20) B) 12.656 A) 5.480 C) 8.520 D) 11.260 E) 2.740
18) Which of the following is TRUE? 18) A) A basic solution does not contain H3O+ B) An acidic solution has [H3O+]> [OH-] C) A neutral solution contains [H20] = [H3O+] D) An neutral solution does not contain any H3O+ or OH- E) None of the above are true. 19) Determine the pH of a 0.023 M HNO3 solution. 19) A) 2.49 B) 3.68 C) 1.64 D) 12.36 E) 2.30 20) Determine the pH of a 0.188 M NH3 solution...
Determine the pH of a 0.188 M NH3 solution at 25°C. The Kb of NH3 is 1.76x10-5.
Ammonia, NH3, is a weak monoprotic base with Kb = 1.76 × 10−5. Calculate the pH of a 0.00779 M solution of this base. Report your answer to TWO places past the decimal.
What is the pH of a 0.10 M NH4Cl solution? (Kb(NH3) = 1.8 x 10-5 A. 7.25 B. 11.3 C. 5.63 D. 3.40 E. 10.6
What is the pH of a 0.01 M NH4Cl solution? (Kb(NH3) = 1.8 x 10-5 A. 7.25 B. 11.3 C. 5.63 D. 3.40 E. 10.6
What is the pH value of a 0.10 M NH3 solution? Kb = 1.8 x 10-5 A. 11.1 B. 10.2 C. 6.25 D. 8.25 E. 11.6
In the titration of a 25 mL of 0.245 M weak base (Kb = 1.76*10^-5) being titrated by 0.365 M HCl determine the following: a. The PH at the initial point b. The PH after 12.3 mL of HCl has been added c. The PH at the equivalence point d. The PH after 18.4 mL of HCl has been added
3) Kb for NH3 1.8 x 10-5 a) Calculate the pH of a buffer solution that is 0.100 M NH3 and 0.120 M NHANO3. b) What is the pH after 60.0 mL of 0.010 M HCl is added to 90.0 mL of the buffer solution in 2(a). Assume the change in volume is additive. c) What is the pH after 60.0 mL of 0.010 M Ca(OH)2 is added to 90.0 mL of the buffer solution in 2(a). Assume the change...
Calculate the pH of a 500.0 mL solution that is 0.30 M NH3 and 0.50 M NH4Br. For NH3, Kb = 1.76 × 10-5 .