In the Brønsted–Lowry definition of acids and bases, an acid __________
is the proton donor
In the following reaction in aqueous solution CH3COOH + NH3 = CH3COO- + NH4+, the acid reactant is __________ and its conjugate base product is __________.
CH3COOH; CH3COO-
The conjugate acid of the hydrogen phosphate ion, HPO4 2– is?
H2PO4 –
If the pH of a solution increases by 2 units (e.g., from 1 to 3), then the ratio of the new to the original hydronium ion concentration is __________
1/100
A solution with an [OH– ] concentration of 1.20 × 10–7 M has a pOH and pH of __________
6.92; 7.08
A solution with a pOH of 4.3 has a [H+ ] of __________
2.0 x 10 ^(-10)
What is the pH of a 0.010 M solution of acetic acid? Ka for acetic acid is 1.8 × 10–5
3.37
The first disinfectant used by Joseph Lister was called carbolic acid. This substance now is known as phenol, C6H5OH (pKa = 10.0). What is the pH of a 0.10 M solution of phenol?
5.5
The pH of a popular soft drink is 3.4; what is its hydronium ion concentration?
4.0 x 10 ^(-4)
Boric acid frequently is used as an eyewash to treat eye infections. The pH of a 0.050 M solution of boric acid is 5.28. What is the value of the boric acid ionization constant, Ka?
5.51 × 10 ^(-10)
The pH of a solution is 2. If its pH is increased to 6, how many times greater is the [H+ ] of the original solution?
10000
