1. Find the pH of 0.55M XNO3. The Kb for XOH is 4.5 x 10-5.
*Hint: X is not a spectator
2. A 0.00597 M solution of a weak base has a pH of 8.65.
Find the percent ionization of this base.
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1. Find the pH of 0.55M XNO3. The Kb for XOH is 4.5 x 10-5. *Hint:...
1. Calculate the pH of a 0.447 M aqueous solution of aniline (C6H5NH2, Kb = 7.4×10-10). 2. Calculate the pH of a 0.0590 M aqueous solution of the weak base caffeine (C8H10N4O2, Kb = 4.10×10-4). 3. Calculate the percent ionization of a 0.545 M solution of hydrocyanic acid.
1. The weak base hydrazine, N2H4, has a Kb = 1.7 x 10-6. What is the percent ionization of a 0.15 M solution? 2. Hydrofluoric Acid has a Ka of 6.8 x 10-4. Calculate the [H+] in 0.25 M HF: 3. What is the pH of a 0.050 M solution of Acetic Acid, HC2H3O2? 4. A solution has a pOH of 10.25. Calculate the [H+].
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1.) If the Kb of a weak base is 3.4 x 10^-6, what is the pH of a 0.11M solution of this base? 2.) A certain weak base has a Kb of 7.00 x 10^-7. What concentration of this base will produce a pH of 10.16?
1) Determine the pH of a 0.0785 M unknown weak base solution. Kb of the unknown weak base is 4.7 x 10−6. 2) An unknown weak acid solution with a concentration of 0.0850 M has a pH of 4.35. What is the Ka for this weak acid? 3) What is the pH of a 0.0380 M solution of HNO2? (Use your workbook to find Ka) 4) An unknown weak base solution with a concentration of 0.187 M has a pH...
Ammonia, NH3, is a weak base with a Kb value of 1.8×10−5. Part A What is the pH of a 8.50×10−2 M ammonia solution? Part B What is the percent ionization of ammonia at this concentration?
Ammonia, NH3, is a weak base with a Kb value of 1.8×10−5. What is the pH of a 0.320 mol L−1 ammonia solution? Answer is 11.38 Part B What is the percent ionization of ammonia at this concentration?Express your answer with the appropriate units.
1)If the Kb of a weak base is 1.3 × 10-6, what is the pH of a 0.13 M solution of this base? 2) A certain weak base has a Kb of 7.40 × 10-7. What concentration of this base will produce a pH of 10.33?
1. If the Kb of a weak base is 7.4×10−6, what is the pH of a 0.39 M solution of this base? 2. A certain weak base has a Kb of 7.10×10−7 What concentration of this base will produce a pH of 10.30?
Find the pH of a 0.0015 M morphine solution (weak base), Kb= 1.6 x 10−6.