Chapter 4 3 How many grams of CH3OH must be added to water to prepare

took 23.9 mL of the base to reach the endpoint of the titration. The concentration (M) of the acid was

________.

A) 0.0102

B) 0.00508

C) 0.0204

D) 0.102

E) 0.227

4.3 Algorithmic Questions

1) Of the species below, only ________ is not an electrolyte.

A) HBr

B) LiCl

C) Ne

D) KOH

E) NaNO3

2) What is the formula for phosphoric acid?

A) H3PO4

B) H2PO4

C) H4PO4

D) H3PO3

E) none of the above

3) The total concentration of ions in a 0.250 M solution of HCl is ________.

A) 0

B) 0.125 M

C) 0.250 M

D) 0.500 M

E) 0.750 M

4) Which hydroxides are weak bases?

A) KOH

B) Ba(OH)2

C) RbOH

D) CsOH

E) None of these choices are weak bases.

5) Which of the following is soluble in water at 25 °C?

A) AgNO3

B) Hg2Cl2

C) PbCl2

D) Ag2S

E) AgCl

6) With which of the following will the Potassium ion form an insoluble salt?

A) Phosphate

B) Sulfate

C) Sulfide

D) Iodide

E) Potassium will form soluble salts with all choices.

7) Which one of the following solutions will have the greatest concentration of hydroxide ions?

A) 1.10 M rubidium hydroxide

B) 0.368 M calcium hydroxide

C) 0.368 M ammonium hydroxide

D) 0.368 M potassium hydroxide

E) 0.368 M sulfuric acid

8) With which ion will the mercury ion form an insoluble salt?

A) phosphate

B) nitrate

C) sulfate

D) chloride

E) acetate

9) In which species does chlorine have an oxidation number of zero?

A) Cl2

B) HClO4

C) NaClO3

D) Cl–

E) HCl

10) In which species does nitrogen have the highest oxidation number?

A) NaNO3

B) HNO2

C) NO2–

D) NH3

E) N2

11) What is the concentration (M) of sodium ions in 4.57 L of a 2.98 M Na3PO4 solution?

12) How many grams of NaOH (MW = 40.0) are there in 500.0 mL of a 0.250 M NaOH solution?

A) 0.00219

B) 114

C) 14.0

D) 5.00

E) 0.125

13) How many grams of NaOH (MW = 40.0) are there in 200.0 mL of a 0.175 M NaOH solution?

A) .00219

B) 114

C) 1.40

D) 0.0350

E) 14.0

14) How many grams of CH3OH must be added to water to prepare 150 mL of a solution that is 2.0 M

CH3OH?

A) 0.0096

B) 430

C) 2.4

D) 9.6

E) 4.3

15) There are ________ mol of bromide ions in 0.500 L of a 0.350 M solution of AlBr3.

A) 0.150

B) 0.0500

C) 0.525

D) 0.167

E) 0.500

16) What is the concentration (M) of KCl in a solution made by mixing 25.0 mL of 0.100 M KCl with 50.0

mL of 0.100 M KCl?

A) 0.100

B) 0.0500

C) 0.0333

D) 0.0250

E) 125

17) What is the concentration (M) of CH3OH in a solution prepared by dissolving 34.4 g of CH3OH in

sufficient water to give exactly 230 mL of solution?

A) 11.9

B) 0.00159

C) 1.59

D) 4.67

E) 5.31

18) What is the concentration (M) of CH3OH in a solution prepared by dissolving 11.7 g of CH3OH in

sufficient water to give exactly 330. mL of solution?

A) 11.9

B) 1.11

C) 0.00159

D) 1.59

E) 0.0841

40

19) How many grams of H3PO4 are in 145 mL of a 3.50 M solution of H3PO4?

A) 0.508

B) 49.7

C) 20.0

D) 4.90

E) 612

20) How many grams of H3PO4 are in 175 mL of a 4.00 M solution of H3PO4?

A) 0.700

B) 20.0

C) 68.6

D) 4.90

E) 612

21) What is the concentration (M) of CH3OH in a solution prepared by dissolving 10.2 g of CH3OH in

sufficient water to give exactly 230 mL of solution?

22) How many grams of H3PO4 are in 415 mL of a 4.00 M solution of H3PO4?

23) What is the concentration (M) of a NaCl solution prepared by dissolving 3.8 g of NaCl in sufficient

water to give 245 mL of solution?

24) How many grams of NaOH (MW = 40.0) are there in 375.0 mL of a 0.325 M NaOH solution?

25) How many grams of CH3OH must be added to water to prepare 175 mL of a solution that is 1.0 M

CH3OH?

26) There are ________ mol of bromide ions in 0.700 L of a 0.400 M solution of AlBr3.

27) How many moles of Co2+ are present in 0.300 L of a 0.500 M solution of CoI2?

28) What are the respective concentrations (M) of Cu+2 and Cl– afforded by dissolving 0.871 mol CuCl2 in

water and diluting to 259 mL?

A) 3.36 and 6.73

B) 0.00336 and 3.36

C) 0.00336 and 0.00336

D) 3.36 and 3.36

E) 0.297 and 0.113

29) What mass (g) of barium iodide is contained in 188 mL of a barium iodide solution that has an iodide

ion concentration of 0.532 M?

A) 19.6

B) 39.1

C) 19,600

D) 39,100

E) 276

30) Calculate the concentration (M) of sodium ions in a solution made by diluting 50.0 mL of a 0.874 M

solution of sodium sulfide to a total volume of 250 mL.

31) What volume (mL) of a concentrated solution of sodium hydroxide (6.00 M) must be diluted to

185.6 mL to make a 3.23 M solution of sodium hydroxide?

A) 99.9

B) 3600

C) 287

D) 0.104

E) 0.0100

32) What volume (mL) of a 5.45 M lead nitrate solution must be diluted to 820.7 mL to make a 1.41 M

solution of lead nitrate?

A) 212

B) 6310

C) 3170

D) 0.00936

E) 0.00471

33) How many milliliters of a stock solution of 11.7 M HNO3 would be needed to prepare 0.500 L of 0.500

M HNO3?

A) 0.0468

B) 21.4

C) 2.93

D) 46.8

E) 0.0214

34) A stock solution of HNO3 is prepared and found to contain 12.7 M of HNO3. If 25.0 mL of the stock

solution is diluted to a final volume of 0.500 L, the concentration of the diluted solution is ________ M.

A) 0.254

B) 1.57

C) 0.635

D) 635

E) 254

35) Pure acetic acid (HC2H3O2) is a liquid and is known as glacial acetic acid. Calculate the molarity of a

solution prepared by dissolving 20.00 mL of glacial acetic acid at 25 °C in sufficient water to give 500.0

mL of solution. The density of glacial acetic acid at 25 °C is 1.05 g/mL.

A) 2.52 × 103

B) 42.0

C) 0.0420

D) 0.699

E) 6.99 × 10-4

36) A solution is prepared by mixing 15.0 mL of 0.100 M HCl and 5.00 mL of 0.200 M NaCl. What is the

molarity of chloride ion in this solution?

A) 0.175

B) 8.00

C) 1.25

D) 0.0250

E) 0.125

37) What mass (g) of AgBr is formed when 57.8 mL of 0.423 M AgNO3 is treated with an excess of

aqueous hydrobromic acid?

A) 4.59

B) 2.30

C) 25.7

D) 0.130

E) 25,700

44

38) A solution is prepared by adding 1.50 g of solid NaCl to 50.0 mL of 0.100 M CaCl2. What is the

molarity of chloride ion in the final solution? Assume that the volume of the final solution is 50.0 mL.

A) 0.713

B) 0.613

C) 0.130

D) 0.230

E) 0.513

39) Calculate the number of grams of solute in 500.0 mL of 0.159 M KOH.

A) 176

B) 1.42

C) 4.46 × 103

D) 4.46

E) 1.42 × 10-3

40) What mass (g) of CaF2 is formed when 30.4 mL of 0.438 M NaF is treated with an excess of aqueous

calcium nitrate?

A) 0.520

B) 1.04

C) 1040

D) 0.171

E) 5420

41) What is the molarity of a NaOH solution if 15.5 mL of a 0.220 M H2SO4 solution is required to

neutralize a 25.0-mL sample of the NaOH solution?

A) 0.273

B) 0.355

C) 0.710

D) 42.6

E) 0.136

42) Lead ions can be precipitated from aqueous solutions by the addition of aqueous iodide:

Pb2+ (aq) + 2I– (aq) → PbI2 (s)

Lead iodide is virtually insoluble in water so that the reaction appears to go to completion. How many

milliliters of 3.550 M HI(aq) must be added to a solution containing 0.600 mol of Pb(NO3)2 (aq) to

completely precipitate the lead?

A) 2.96 × 10-3

B) 338

C) 169

D) 0.169

E) 0.338

43) Silver ions can be precipitated from aqueous solutions by the addition of aqueous chloride:

Ag+ (aq) + Cl– (aq) → AgCl (s)

Silver chloride is virtually insoluble in water so that the reaction appears to go to completion. How many

grams of solid NaCl must be added to 25.0 mL of 0.149 M AgNO3 solution to completely precipitate the

silver?

A) 3.73 × 10-3

B) 6.37 × 10-5

C) 0.218

D) 0.0637

E) 1.57 × 104

44) How many milliliters of 0.188 M HClO4 solution are needed to neutralize 50.00 mL of 0.0832 M

NaOH?

A) 0.782

B) 8.85 × 10-3

C) 113

D) 0.0452

E) 22.1

45) What volume (mL) of 0.102 M NaOH is required to neutralize 17.1 mL of 0.443 M HCl?

A) 74.3

B) 3.94

C) 0.773

D) 0.0135

E) 0.000773

46) A 24.5 mL aliquot of 0.0938 M H2SO4 (aq) is to be titrated with 0.0295 M NaOH (aq). What volume

(mL) of base will it take to reach the equivalence point?

A) 156

B) 0.136

C) 77.9

D) 39.0

E) 4430

47) A 11.5 mL aliquot of 0.162 M H3PO4 (aq) is to be titrated with 0.229 M NaOH (aq). What volume (mL)

of base will it take to reach the equivalence point?

A) 24.4

B) 1.28

C) 8.14

D) 2.71

E) 103

48) What volume (mL) of 142 M phosphoric acid can be neutralized with 0.367 mL of 0.0824 M sodium

hydroxide?

A) 211

B) 12.9

C) 1900

D) 632

E) 1570

49) What is the concentration (M) of 39.88 mL of an unknown NaOH solution if it required 46.08 mL of

0.6592 M HCl to neutralize?

A) 0.7617

B) 2788

C) 1211

D) 1.313

E) 1.211

50) A titration reached the equivalence point when 16.1 mL of 0.209 M H2SO4 (aq) was added to 12.0 mL

of NaOH (aq) of unknown concentration. What is the concentration (M) of this unknown NaOH solution?

A) 0.561

B) 80.8

C) 0.280

D) 0.140

E) 3.21

4.4 Short Answer Questions

1) The solvent in an aqueous solution is ________.

2) Calculate the concentration (M) of arsenic acid (H3AsO4) in a solution if 25.00 mL of that solution

required 35.21 mL of 0.1894 M KOH for neutralization.

3) How many moles of BaCl2 are formed in the neutralization of 393 mL of 0.171 M Ba(OH)2 with

aqueous HCl?

4.5 True/False Questions

1) Ca(OH)2 is a strong base.

2) The compound HClO4 is a weak acid.

3) HNO2 is a strong acid.

4) The compound NH4Cl is a weak acid.

5) Ammonia is a strong base.