Free Printable Titration, Ka, Acid Base review

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Titration, Ka, Acid Base review

Total questions: 24

Worksheet time: 46mins

Name

Class

Date

what is the reading on this burette?

4.40mL

3.50mL

3.60mL

4.50mL

I have 25mLof 1M HCl which neutralises 20mL of NaOH. What is the concentration of the NaOH?

0.8 M

1 M

1.25 M

Identify the products of the chemical equation
3 LiOH + H₃PO₄ →

Li₃PO₄ + 3 H₂O

LiPO₄ + 3 H₂O

Li(PO₄)₃ + 3 H₂O

BOY + La + N₂

A 50.0 mL sample of Ca(OH)₂ is neutralized by 300.0 mL of HCl solution with a pH of 1.3. Calculate the molarity of the Ca(OH)₂ solution.

1.0 M

0.50 M

0.15 M

0.30 M

If phenolphthalein turns bright pink, it indicates

an acid

a base

a neutral

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

HCl/OCl^-

H₂SO₄/SO₄^2-

NH₄⁺/NH₃

H₃O⁺/OH^-

Calculate the average volume of acid needed for this neutralisation

15.2cm³

15.0cm³

35.5cm³

30.1cm³

30cm³ of NaOH is neutralised by 12.3cm³ of 0.2mol/l HCl. What is the concentration of the NaOH.

82 mol/l

0.82 mol/l

0.49 mol/l

0.082 mol/l

A solution of HCl has a [H⁺] = 7.2 x 10^-9. Is this and acid or a base?

Acid

Base

10.

Acetic Acid (HC₂H₃O₂) is a weak monoprotic acid. It's concentration is 0.20M and it's Ka value is 1.8x10 -5. Calculate it's pH value.

.698

2.72

11.28

None of the answers are correct

11.

What is the [OH-] if the [H+] is 1.0 x 10-3M?

1.0 x 10-3 M

6.02 x 10-23 M

1.0 x 10-14 M

1.0 x 10-11 M

12.

Complete the following reaction:

HCl + Mg(OH)₂ -->

MgCl₂ + H₂O

Mg +H₂O

MgCl₂ + H₂

MgCl₂ + H₂O + CO₂

13.

What is the molarity of a 30 mL HCl which is neutralized by 48 mL of 0.1 M NaOH?

HCl + NaOH --> H₂O + NaCl

0.16 M

6.25 M

0.063 M

14.

What might happen if you mixed a strong acid with an equally strong base?

You would see an explosive chemical reaction.

The acid would destroy the base.

The base would destroy the acid.

You'd wind up with a pH-neutral substance.

15.

If it takes 54 mL of 0.1 M NaOH to neutralize 125 mL of an HCl solution, what is the concentration of HCl?

0.043 M

23.148 M

0.231 M

16.

Which of the following would be a weak base?

17.

How many moles of Ca(OH)₂ are needed to neutralize three moles of HCl?

1.5

18.

What is the pH at the equivalence point.

The pH is approximately 5

The pH is approximately 6

The pH is approximately 8

The pH is approximately 9

19.

In which of the following reactions does H₂PO₄^-act as an acid?

H₃PO₄ + H₂O --> H₃O⁺ + H₂PO₄^-

H₂PO₄^- + H₂O --> H₃O⁺ + HPO₄^2-

H₂PO₄^- + OH^- --> H₃PO₄ + O^2-

The ion cannot act as an acid

20.

What is the volume of strong base 0.1M needed to neutralize 25 ml 0.1M CH₃COOH?

12.5 ml

25 ml

50 ml

less than 25 ml

21.

What is the hydrogen ion concentration in a solution with pOH = 3.3?

10.7 M

0.00050 M

0.000025 M

2.0 x 10^-11 M

22.

A 0.95 M solution of 10.0 mL Al(OH)₃ is neutralized using a 2 M solution of H₂SO₄. How much H₂SO₄ was needed?

3H₂SO₄ + 2Al(OH)₃ --> 6H₂O + 1Al₂(SO₄)₃

0.1 mL

7.1 mL

5.0 mL

0.22 mL

23.

1) 0.04 M NaOH is load into a buret - initial reading is 4.5 mL

2) 60 mL of unknown monoprotic acid, HA, is placed under the buret.

3) 2 drops of phenolphthalein is added to the acid.

4) The base is slowly added to the acid until it turns pink. - final reading from the buret is 34.6 mL.

WHAT IS THE MOLARITY OF THE ACID?

0.04 M

0.0012 M

0.02 M

30.1 M

24.

If 100 mL of 0.1 M solution is diluted to 550 mL what is the concentration?

0.02 M

0.04 M

0.1 M

0.003 M

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Titration, Ka, Acid Base review

Total questions: 24

Worksheet time: 46mins

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