Find the pH of a 0.1 M NH3 solution. (Kb= 1.76x10-5)
what is the pH of a 0.150M NH4Cl solution? Kb of NH3 = 1.76x10^-5
Calculate the pH of 0.25 M NH4CL given kb= 1.76x10^-5 for NH3 (ans. 4.92)
Determine the pH of a 0.188 M NH3 solution at 25°C. The Kb of NH3 is 1.76x10-5.
NH3 is a weak base with a Kb value of 1.76x10–5. Suppose 25.0 mL of a0.180 MNH3 is titrate using HCl. The end point is reach after 35.0 mL HCl had been added. Calculate the pH of the resulting solution at the equivalence-point. Here is the titration equation:NH3(aq) + HCl(aq) →NH4Cl(aq)
A 30.0 mL sample of .200 M NH3 is titrated with .100M HI. The Kb for NH3 is 1.76X10^-5 A. what is the initial pH of the solution? B. What is the pH of the solution after the addition of 30.00 mL of HI? C. What is the pH of the solution at the equivalence point? D. What is the pH of the solution after the addition of 90.0mL of HI?
What is the pH of a 1.0028 M ammonia solution given that Kb = 1.80E-5? NH3 (aq) + H2O (l) --> OH1- (aq) + NH41+ (aq) What is the pH of a 1.0028 M ammonia solution given that Kb = 1.80E-5? NH3 (aq) + H20 (1) --> OH1- (aq) + NH41+ (aq)
Determine the pH of a 0.188 M NH3 solution at 25°C. The Kb of NH3 is 1.76 × 10-5.A) 2.740 B) 5.480 C) 8.520 D) 12.656 E) 11.260
Kb for NH3 is 1.8x10^-5. What is the pH of a 0.35-M aqueous solution of NH4Cl at 25°C?
What is the pH of a 0.4647 M aqueous solution of ammonia? Kb (NH3) = 1.8x10-5
What is the pH of a 0.720 M aqueous solution of NH4NO3? The Kb for NH3 is 1.8 x 10-5.