Multiple Choice
Calculate the pH of a solution that is 0.205 M in CH3NH2 and 1.55 M in CH3NH3Br. Assume the Kb for CH3NH2 is 4.4 x 10^-4.
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17. Acid and Base Equilibrium
pH of Weak Bases
Back17. Acid and Base Equilibrium
pH of Weak Bases
- Open Question
What is the pH of a 0.750 M solution of NaCN (Ka of HCN is 4.9 × 10-10)?
- Multiple ChoiceWhat is the pH of a 0.145 M solution of (CH3)3N (trimethylamine), given that Kb for (CH3)3N is 6.4 × 10^{-5}?1views
- Multiple ChoiceCalculate the pH of a 0.30 M solution of barium nitrite. Given that the Ka of HNO2 is 4.5 x 10^-4, what is the pH of the solution?1views
- Multiple ChoiceDetermine the pH of a solution that is 0.125 M in CO3^2−. For carbonic acid (H2CO3), Ka1=4.3×10^−7 and Ka2=5.6×10^−11. What is the pH of the solution?
- Open Question
What is the pH of a solution with a hydroxyl ion (OH-) concentration of 10-10 M?
1views - Multiple ChoiceA 0.050 M solution of hydroxylamine, NH2OH, having Kb = 9.1 × 10^-9 has a pH of ________.
- Multiple ChoiceWhat is the pH of a 0.145 M solution of (CH3)3N, given that the Kb of (CH3)3N is 6.4 × 10⁻⁵?
- Multiple ChoiceWhat is the pH of a 0.05 M sodium fluoride solution, given that F⁻ has a Kb of 1.59 x 10⁻¹¹?
- Multiple ChoiceA student claims that the pH of a aqueous solution of methylamine, , is 12.54. Given for at 25 °C, which pH is most reasonable (assuming )?
- Open Question
The Kb of methylamine is 4.4 x 10–4. What is the approximate [OH–] of a 1 M solution of methylamine?
1views - Multiple ChoiceWhat is the theoretical pH of a 0.1 M solution of sodium acetate (NaC2H3O2), a weak base?1views
- Multiple ChoiceCalculate the pH of a solution that is 0.205 M in CH3NH2 and 0.155 M in CH3NH3Br. Assume the Kb for CH3NH2 is 4.4 x 10^-4.1views
- Multiple ChoiceCalculate the pH of a 0.205 M KNO2 solution, given that the Ka of nitrous acid (HNO2) is 4.6 × 10^(-4).
- Multiple ChoiceCalculate the pH of a 0.400 M NaF solution, given that the Ka of HF is 6.4 x 10^-4.