Free Printable UNIT 8

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UNIT 8 - QUIZ # 1

Total questions: 18

Worksheet time: 1hrs 7mins

Name

Class

Date

What is the conjugate base of HCO₃^-?

HCO₃^-

H₂CO₃^-

H₂CO₃

CO₃^2-

Which of the following is not a strong acid?

HCl

HBr

HNO₃

If a solution has a [H⁺] of 1.2 x 10^-4M what is the [OH^-]?

8.3 x 10^-4M

8.3 x 10^-11M

1.2 x 10¹⁰M

1.2 x 10^-4M

A larger K means there are ______ products at equilibrium

less

Which of the following is a conjugate acid/base pair?

HCl/OCl^-

H₂SO₄/SO₄^2-

NH₄⁺/NH₃

H₃O⁺/OH^-

Ammonia, NH₃, behaves as a base when placed in water according to the following equilibrium:

NH₃(aq) + H₂O(l) ⥨ NH₄⁺(aq) + OH^-(aq)

Calculate the pH of a 0.47M NH₃ (K_b = 1.8 x 10^-5) solution. (For partial credit - submit your work for this question on Google Classroom - HINT:ICE Table)

2.54

8.93

5.07

11.46

Listed below are weak acids with their K_a values. Which of the following is the strongest acid?

CH₃COOH (K_a = 1.8 × 10^–5)

HF (K_a = 6.5 × 10^–4)

HCN (K_a = 6.3 × 10^–10)

HClO (K_a = 3.0 × 10^–8)

Listed below are weak acids along with the pK_a. Which of the acids is the strongest?

HF (pK_a = 3.17)

HCO₃^– (pK_a = 10.32)

H₂PO₄^– (pK_a = 7.18)

NH₄⁺ (pK_a = 9.20)

A 1.0 molar solution of a very weak monoprotic acid (HA) has a pH of 5. What is the value of K_a for the acid? (Hint- the pH gives you the value of [H⁺]_eq)

1 × 10^–10

1 × 10^–7

1 × 10^–5

1 × 10^–2

10.

A 25.0 mL sample of HCl was titrated to the endpoint with 15.0 mL of 2.0 M NaOH. What is the molarity of HCl?

1.6 M HCl

0.03 M HCl

0.6 M HCl

1.2 M HCl

11.

Which point on the titration curve corresponds to the point at which the moles of the added strong base are equal to the moles of the weak acid initially present?

12.

A 5.00 mL sample of household ammonia was analyzed by titration with hydrochloric acid according to the following reaction: $HCl\ \ +\ \ NH_3\ \ \rightarrow\ \ NH_4^{\ +}\ \ \ +\ \ Cl^{\ -}$
This titration required 19.5 mL of 0.750 M HCl. What is the molarity of the ammonia sample?

1.97 M

2.19 M

2.44 M

2.92 M

13.

Equal moles of the indicated acids are dissolved in the amounts of water shown in the beakers below. In which solution will the percent ionization of the acid be the lowest?

Beaker A

Beaker B

Beaker C

Impossible to tell from the information given.

14.

Which represents an acid with the smallest K_a value?

15.

An acid that dissociatels, 100%, completely. Typically 0-4 on the pH scale.

Strong Acid

Weak Acid

16.

An acid that does not dissociate complete, with less than 100%. Typically pH range is between 4 - 7.

Strong Acid

Weak Acid

17.

HC₆H₇O₇(aq) + OH⁻(aq) → C₆H₇O₇⁻(aq) + H₂O(l)

A 25.00 mL sample containing 2.5 × 10⁻³ moles of citric acid is titrated to the equivalence point with 0.100 M KOH as shown in the net ionic reaction above. What are the relative amounts of acid and conjugate base at the equivalence point?

[HC₆H₇O₇] ≅ 0.100 M and [C₆H₇O₇⁻ ] << 0.100 M

[HC₆H₇O₇] = [C₆H₇O₇⁻ ]

[HC₆H₇O₇] << 0.050 M and [C₆H₇O₇⁻ ] ≅ 0.0.050 M

[HC₆H₇O₇] << 0.100 M and [C₆H₇O₇⁻ ] ≅ 0.100 M

18.

Each particle diagram shown is a representation of an aqueous solution of one of the acids listed in the table. The molarity of the acids in the solutions is the same. Based on the information, which particle diagram best corresponds to the indicated acid?

Diagram 3 is HClO

Diagram 1 is HIO

Diagram 3 is HBro

Diagram 2 is HClO

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UNIT 8 - QUIZ # 1

Total questions: 18

Worksheet time: 1hrs 7mins

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