Chapter 4 3 What is the concentration (M) of a NaCl solution prepared

A) 0.193 M

B) 0.386 M

C) 0.0965 M

D) 0.579 M

E) 0.0643 M

50) The concentration of species in 500 mL of a 2.104 M solution of sodium sulfate is __________ M

sodium ion and __________ M sulfate ion.

A) 2.104, 1.052

B) 2.104, 2.104

C) 2.104, 4.208

D) 1.052, 1.052

E) 4.208, 2.104

51) When 0.500 mol of HC2H3O2 is combined with enough water to make a 300.0 mL solution, the

concentration of HC2H3O2 is __________ M.

A) 3.33

B) 1.67

C) 0.835

D) 0.00167

E) 0.150

52) In a titration of 35.00 mL of 0.737 M H2SO4, __________ mL of a 0.827 M KOH solution is

required for neutralization.

A) 35.0

B) 1.12

C) 25.8

D) 62.4

E) 39.3

53) Oxalic acid is a diprotic acid. Calculate the percent of oxalic acid (H2C2O4) in a solid given that a

0.7984-g sample of that solid required 37.98 mL of 0.2283 M NaOH for neutralization.

A) 48.89

B) 97.78

C) 28.59

D) 1.086

E) 22.83

54) Oxalic acid is a diprotic acid. If a solid material contains 53.66 percent of oxalic acid (H2C2O4), by

mass, then a 0.6543-g sample of that solid will require __________ mL of 0.3483 M NaOH for

neutralization.

A) 11.19

B) 97.78

C) 28.59

D) 1.119

E) 22.39

55) A 17.5 mL sample of an acetic acid (CH3CO2H) solution required 29.6 mL of 0.250 M NaOH for

neutralization. The concentration of acetic acid was __________ M.

A) 0.158

B) 0.423

C) 134

D) 6.88

E) 0.214

56) A 25.5 mL aliquot of HCl (aq) of unknown concentration was titrated with 0.113 M NaOH (aq). It

took 51.2 mL of the base to reach the endpoint of the titration. The concentration (M) of the acid was

__________.

A) 1.02

B) 0.114

C) 0.454

D) 0.113

E) 0.227

57) A 31.5 mL aliquot of HNO3 (aq) of unknown concentration was titrated with 0.0134 M NaOH (aq).

It 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) 0.0051

C) 0.0204

D) 0.227

E) 1.02

58) A 31.5 mL aliquot of H2SO4 (aq) of unknown concentration was titrated with 0.0134 M NaOH (aq).

It 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) The total concentration of ions in a 0.625 M solution of HCl is __________.

A) 0

B) 0.500 M

C) 0.625 M

D) 1.25 M

E) 1.50 M

2) What is the concentration (M) of sodium ions in 4.57 L of a 1.25 M Na3PO4 solution?

3) How many grams of NaOH (MW = 40.0) are there in 500.0 mL of a 0.225 M NaOH solution?

A) 0.00219

B) 114

C) 14.0

D) 4.50

E) 0.113

35

4) How many grams of NaOH (MW = 40.0) are there in 100.0 mL of a 0.175 M NaOH solution?

A) .00219

B) 114

C) 0.700

D) 0.0175

E) 14.0

5) How many grams of CH3OH must be added to water to prepare 150 mL of a solution that is 1.0 M

CH3OH?

A) 0.15

B) 430

C) 2.4

D) 4.8

E) 4.3

6) There are __________ mol of bromide ions in 0.500 L of a 0.100 M solution of AlBr3.

A) 0.0500

B) 0.450

C) 0.150

D) 0.167

E) 0.500

7) What is the concentration (M) of KCl in a solution made by mixing 30.0 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

8) What is the concentration (M) of CH3OH in a solution prepared by dissolving 29.3 g of CH3OH in

sufficient water to give exactly 230 mL of solution?

A) 11.9

B) 0.00159

C) 1.59

D) 3.97

E) 4.31

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

sufficient water to give exactly 230. mL of solution?

A) 11.9

B) 1.59

C) 0.00159

D) 3.17

E) 0.0841

10) How many grams of H3PO4 are in 175 mL of a 3.50 M solution of H3PO4?

A) 0.610

B) 60.0

C) 20.0

D) 4.90

E) 612

11) How many grams of H3PO4 are in 175 mL of a 2.50 M solution of H3PO4?

A) 0.438

B) 20.0

C) 42.9

D) 4.90

E) 612

12) What is the concentration (M) of CH3OH in a solution prepared by dissolving 16.8 g of CH3OH in

sufficient water to give exactly 230 mL of solution?

13) How many grams of H3PO4 are in 265 mL of a 1.50 M solution of H3PO4?

14) What is the concentration (M) of a NaCl solution prepared by dissolving 7.2 g of NaCl in sufficient

water to give 425 mL of solution?

15) How many grams of NaOH (MW = 40.0) are there in 250.0 mL of a 0.275 M NaOH solution?

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

CH3OH?

17) There are __________ mol of bromide ions in 0.900 L of a 0.500M solution of AlBr3.

18) How many moles of Co2+ are present in 0.150 L of a 0.200 M solution of CoI2?

19) Calculate the concentration (M) of sodium ions in a solution made by diluting 40.0 mL of a 0.474 M

solution of sodium sulfide to a total volume of 300 mL.

20) How many milliliters of a stock solution of 11.1 M HNO3 would be needed to prepare 0.500 L of

0.500 M HNO3?

A) 0.0444

B) 22.5

C) 2.78

D) 44.4

E) 0.0225

21) A stock solution of HNO3 is prepared and found to contain 13.5 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) 0.270

B) 1.48

C) 0.675

D) 675

E) 270

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

a solution prepared by dissolving 10.00 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) 1.26 × 103

B) 21.0

C) 0.0210

D) 0.350

E) 3.50 × 10-4

23) A solution is prepared by mixing 50.0 mL of 0.100 M HCl and 10.0 mL of 0.200 M NaCl. What is

the molarity of chloride ion in this solution?

A) 0.183

B) 8.57

C) 3.50

D) 0.0500

E) 0.117

24) A solution is prepared by adding 1.60 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) 0.747

B) 0.647

C) 0.132

D) 0.232

E) 0.547

25) Calculate the number of grams of solute in 500.0 mL of 0.189 M KOH.

A) 148

B) 1.68

C) 5.30 × 103

D) 5.30

E) 1.68 × 10-3

26) What is the molarity of a NaOH solution if 28.2 mL of a 0.355 M H2SO4 solution is required to

neutralize a 25.0-mL sample of the NaOH solution?

A) 0.801

B) 0.315

C) 0.629

D) 125

E) 0.400

27) 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 0.700 mol of Pb(NO)3)2 (aq) to

completely precipitate the lead?

A) 2.54 × 10-3

B) 394

C) 197

D) 0.197

E) 0.394

28) 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 0.366 M AgNO3 solution to completely precipitate

the silver?

A) 9.15 × 10-3

B) 1.57 × 10-4

C) 0.535

D) 0.157

E) 6.39 × 103

29) How many milliliters of 0.132 M HClO4 solution are needed to neutralize 50.00 mL of 0.0789 M

NaOH?

A) 0.521

B) 0.0120

C) 83.7

D) 0.0335

E) 29.9

4.4 Short Answer Questions

1) The solvent in an aqueous solution is __________.

2) What is aqua regia?

3) When gold dissolves in aqua regia, into what form is the gold converted?

4) 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.

5) 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.