NH4Cl(aq) -------------> NH4^+ (aq) + Cl^- (aq)
0.0321M 0.0321M
NH4^+ (aq) + H2O(l) --------------> NH3(aq) + H3O^+ (aq)
I 0.0321 0 0
C -x +x +x
E 0.0321-x +x +x
Ka = Kw/Kb
= 1*10^-14/(1.75*10^-5)
= 5.7*10^-10
Ka = [NH3][H3O^+]/[NH4^+]
5.7*10^-10 = x*x/(0.0321-x)
5.7*10^-10*(0.0321-x) = x^2
x = 4.27*10^-6
[H3O^+] = x = 4.27*10^-6M
PH = -log[H3O^+]
= -log4.27*10^-6
= 5.3696>>>>>answer
the Kb of ammonia (NH3) at 25.0 C is 1.75 x 10-5. Calculate the pH of...
Given the solution 0.50 M NH3 (aq) with Kb = 1.75 * 10-5, calculate the pH using an I.C.E. table
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 6.0 M aqueous solution of NH3 (ammonia). It's Kb = 1.8 x 10-5.
What is the pH of a 0.4647 M aqueous solution of ammonia? Kb (NH3) = 1.8x10-5
How many grams of dry NH4ClNH4Cl need to be added to 2.50 LL of a 0.800 MM solution of ammonia, NH3NH3, to prepare a buffer solution that has a pHpH of 8.86? KbKbK_b for ammonia is 1.8×10−51.8×10−5.
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
Part A Ammonia, NH3, is a weak base with a Kb value of 1.8×10−5. pH of 0.500 M ammonia solution is 11.48 What is the percent ionization of ammonia at this concentration? Express your answer with the appropriate units.
Kb for NH3 is 1.8x10^-5. What is the pH of a 0.35-M aqueous solution of NH4Cl at 25°C?
Given that at 25.0 ∘C Ka for HCN is 4.9×10^-10 Kb for NH3 is 1.8×10^−5 - Part C Calculate the pH of a 0.20 M solution of KCN at 25.0 °C. Express the pH numerically using two decimal places. View Available Hint(s) Templates Symbols uido redo reset keyboard shortcuts help pH = Submit Request Answer - Part D Calculate the pH of a 0.20 M solution of NH Brat 25.0°C. Express the pH numerically using two decimal places. View Available...