Multiple Choice
Consider the titration of 300.0 mL of 0.414 M NH3 (Kb = 1.8 ×10-5) with 0.500 M HNO3.After 150.0 mL HNO3 has been added,what is the pH of the solution?
A) 4.93
B) 9.07
C) 6.07
D) 11.07
E) 7.00
Correct Answer:

Verified
Correct Answer:
Verified
Related Questions
Q3: Given the two equilibria below, Ag(NH<sub>3</sub>)<sub>2</sub><sup>+</sup>(aq) <img
Q4: Which of the following is the common
Q5: What is the pH of a solution
Q6: If the ratio of acid to base
Q7: What is the molar solubility of Mn(OH)<sub>2</sub>(s)in
Q9: What is the value of the dissociation
Q10: A 50.0 mL sample of 0.155 M
Q11: The K<sub>sp</sub> of BaSO<sub>4</sub> is 1.1 ×
Q12: What is the molar solubility of solid
Q13: The K<sub>sp</sub> of Ca(OH)<sub>2</sub> is 5.5 ×