Discussion:
Questions on Acids and Bases
1- What is the difference between a strong acid and a weak acid? Choose from:
A strong acid is dangerous to human health, a weak acid is not.
A strong acid dissociates completely in solution, while a weak acid only dissociates partway.
A strong acid will neutralize a base, but a weak acid isn't strong enough to do so.
A weak acid will not add protons to solution.
2- What is the H+ concentration for an aqueous solution with pOH = 4.21 at 25 ° C ?
3- Arrange the following aqueous solutions, all at 25 ° C, in order of decreasing acidity.(ph=5.45,0.0023 M HCl, pOH=8.55, 0.0018 M KOH)
4- At a certain temperature, the pH of a neutral solution is 7.79. What is the value of K w at that temperature?
5- Calculate [H30+] in each aqueous solution at 25 C and classify each solution as acidic or basic one.
[OH - ]= 5.2×10-4M Express your answer using two significant figures.
OH - ]= 1.9×10-12M Express your answer using two significant figures.
6- 0.45g of hydrogen chloride (HCl ) is dissolved in water to make 5.5Lof solution. What is the pH of the resulting hydrochloric acid solution? Express the pH numerically to two decimal places.
7- 0.25g of sodium hydroxide (NaOH ) pellets are dissolved in water to make 7.0L of solution. What is the pH of this solution? Express the pH numerically to two decimal places.
8- What assumption is commonly used to simplify the process of finding the pH for a solution of a weak acid? Choose from:
~The quadratic equation is the fastest way to find the pH of a weak acid, and the assumption is that the quadratic equation will work.
~For many weak acid solutions, it is assumed that [H3O+] is small relative to the initial concentration of acid, so the "x is small" approximation is used.
~The concentration of H3O+ is assumed to be directly found from the Ka expression, so all that is needed is to plug the initial concentrations of each species into the Ka expression.
~The concentration of H3O+ in solution is assumed to be equal to the concentration of the weak acid.
9- A certain weak acid, HA , has a K a value of 8.5×10-7. Calculate the percent ionization of HA in a 0.10 M solution. Express your answer to two significant figures and include the appropriate units. Calculate the percent ionization of HA in a 0.010 M solution. Express your answer to two significant figures and include the appropriate units.
10- What mass of HClO 4 should be present in 0.600L of solution to obtain a solution with each pH ?
pH = 2.50 Express your answer using two significant figures.
pH = 1.50 Express your answer using two significant figures.
11- A 0.115M solution of a weak acid (HA ) has a pH of 3.31. Calculate the acid ionization constant (K a ) for the acid. Express your answer using two significant figures.
12- Find the pH of a 0.150M solution of a weak monoprotic acid having K a = 1.6×10-5. Express your answer to two decimal places.
13- Find the percent ionization of a 0.150M solution of a weak monoprotic acid having K a = 1.6×10-5. Express your answer using two significant figures.