Problem 2
Define Bronsted-Lowry base. How does it differ from an Arrhenius base?
Problem 3
Identify each as a strong acid or a weak acid. Assume aqueous solutions. a) HF b) \(\mathrm{HCl}\) c) \(\mathrm{HC}_{2} \mathrm{O}_{4}\)
Problem 3
Write the dissociation of hydrogen bromide in water as a Brønsted-Lowry acid- base reaction and identify the proton donor and proton acceptor.
Problem 3
What is the relationship between \(\left[\mathrm{H}^{+}\right]\) and \(K_{\mathrm{w}} ?\) Write a mathematical expression that relates them.
Problem 3
Why isn't an oxide compound like CaO considered a salt? (Hint: what acid-base combination would be needed to make it if it were a salt?)
Problem 3
True or false: An acid is always the titrant. Explain your answer.
Problem 3
What is the pH range for an acidic solution?
Problem 3
What are some general properties of Arrhenius acids?
Problem 3
Which combinations of compounds can make a buffer? Assume aqueous solutions. a) \(\mathrm{HCl}\) and \(\mathrm{NaCl}\) b) \(\mathrm{HNO}_{2}\) and \(\mathrm{NaNO}_{2}\) c) \(\mathrm{NH}_{4} \mathrm{NO}_{3}\) and \(\mathrm{HNO}_{3}\) d) \(\mathrm{NH}_{4} \mathrm{NO}_{3}\) and \(\mathrm{NH}_{3}\)
Problem 4
True or false: An analyte is always dissolved before reaction. Explain your answer.
