Review Problem 16.110 A buffer is prepared containing 0.11 M NH3 and 0.44 M NH4+. Calculate...
A buffer solution is prepared by combining 750.0 ml of 1.00 M of ammonia and 250 ml of 1.00 M ammonium chloride. What is the pH of the buffer? ( Ka of NH4+=5.6*10^-10, Kb of NH3= 1.8*10^-5)
A buffer solution is prepared by combining 750.0 ml of 1.00 M of ammonia and 250 ml of 1.00 M ammonium chloride. What is the pH of the buffer? ( Ka of NH4+=5.6*10^-10, Kb of NH3= 1.8*10^-5)
If you mix 100. mL of 0.11 M HCl with 50.0 mL of 0.22 M NH3, what is the pH of the resulting solution? For NH4+, Ka = 5.6 x 10-10 A. 4.63 B. 8.37 C. 9.37 D. 5.19 E. 6.02
One liter of a buffer containing 0.5 M NH3 and 0.5 M NH4+ has a pH of 9.3. If 200 mL of 1 M HNO3 is added to it, what is the new pH? 4.4 8 OOOOOO 9.6
What is the pH of a buffer solution containing 0.11 M HC2H3O2 (acetic acid) and 0.19 M C2H3O2−? Express your answer using two decimal places. Acetic acid has a Ka of 1.8×10−5.
A buffer solution is prepared by placing a 25.00 mL aliquot of 0.165 M NH3 and a 25.00 mL aliquot of 0.150 M NH4Cl into a 100.00 mL volumetric flask and diluting to the mark. Using activities, calculate the pH of the buffer solution. Use the Davies equation to determine activity coefficients. (pKa of NH4+ = 9.245)
A buffer solution contains NH3 0.20 M and NH4 + 0.30 M. Calculate the pH after 2.0 mmol of HCl is added to that solution. The volume of the solution is 50.0 mL and pKa (NH4 +) = 9.25 A 4.89 B. 8.92 C. 9.02 D. 9.07 E 9.58
Calculate the molar solubility of Sn(OH)2 in a buffer solution containing equal concentrations of NH3 and NH4+.
Ammonia react with water as shown in the following equation: NH3(aq) + H2O(l) NH4+(aq) + OH-(aq) Kb = 1.77 x 10-5 and Ka = 5.65 x 10-10 a) Calculate the pH of the 0.030 M NH3 solution (Use a labeled ICE table) b) Calculate the pH of the solution at the equivalent point (when equal amount of acid is added. Assume the volume doubles). (Use a labeled ICE table) c) Over which pH range (actual numbers) do you expect...
A solution is prepared by adding 20.0 mL of 0.15 M HCl to 80.0 mL of 0.20 M NH3. Ka(NH4+)= 5.8 x 10-10 a. Is this solution a buffer? Why or why not? b. What is the pH of the solution?