Acids and Bases | Baamboozle - Baamboozle | The Most Fun Classroom Games!

Define the term buffer solution.

a solution that resists pH change/maintains a (nearly) constant pH; when small amounts of acid or alkali are added

The indicator bromophenol blue, HIn(aq), has a form that is yellow and an In– (aq) form that is blue. Write an equation to show how bromophenol blue acts as an indicator.

HIn(aq) = H + (aq) + In– (aq)

10 cm3 of 0.01 mol dm–3 nitric acid (HNO3 ) is diluted with 90 cm3 of water. What is the pH of the resulting solution?

3

The pKa values of four acids are as follows. (W 4.87; X 4.82; Y 4.86; Z 4.85). What is the correct order when these acids are arranged in order of increasing acid strength?

W < Y < Z < X

Draw the titration curve that shows how the pH changes when a weak base is added to a strong acid

(start low; eq point below 7; end just above 7)

Vinegar has a pH of approximately 3 and some detergents have a pH of approximately 8. State and explain which of these has the higher concentration of H+ and by what factor.

Vinegar; factor of 100000

Suggest one method, other than measuring pH, which could be used to distinguish between solutions of a strong acid and a weak acid of the same concentration. State the expected results.

measure electrical conductivity; strong acids are good conductors/weak acids are poor conductors (other relevant answers)

What is the conjugate base of the HSO4 – (aq) ion?

SO4 2-

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

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 popular soft drink is 3.4; what is its hydronium ion concentration?

4.0 x 10 ^(-4)

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

What is the pH of a 0.010 M solution of acetic acid? Ka for acetic acid is 1.8 × 10–5

3.37

A solution with a pOH of 4.3 has a [H+ ] of __________

2.0 x 10 ^(-10)

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 pH of 9.50 has a pOH of __________

4.5

When [H+ ] = 4.0 × 10–9 M in water at 25°C, then pH = __________

8.40

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

Ammonia (NH3) acts as a weak base in aqueous solution. What is the acid that reacts with this base when ammonia is dissolved in water?

H2O

The conjugate acid of the hydrogen phosphate ion, HPO4 2– is?

H2PO4 –

In the following reaction in aqueous solution CH3NH2 + HSO4- = CH3NH3+ + SO4 2–, the acid reactant is __________, and its conjugate base product is __________.

HSO4– ; SO4 2–

In the following reaction in aqueous solution CH3COOH + NH3 = CH3COO- + NH4+, the acid reactant is __________ and its conjugate base product is __________.

CH3COOH; CH3COO-

In the Brønsted–Lowry definition of acids and bases, an acid __________

is the proton donor