Home Chapter 4 Problem Solving Center Practice Exercises

# Practice Exercises

This activity contains 40 questions.

## A certain volume of a 0.50 Msolution contains 4.5 g of a certain salt. What mass of the salt is present in the same volume of a 2.50 Msolution?Online Text

 0.90 g 4.5 g 9.0 g 14 g 18 g 23 g

## How many milliliters of 1.50 MKOH solution are needed to supply 0.125 mol of KOH? Online Text

 0.0833 mL 0.188 mL 12.0 mL 83.3 mL 188 mL 1.20 x 104 mL

Pure acetic acid, known as glacial acetic acid, is a liquid with a density of 1.049 g/mL at 25°C. Calculate the molarity of a solution of acetic acid made by dissolving 10.00 mL of glacial acetic acid at 25°C in enough water to make 100.0 mL of solution.

Online Text

 1.747 x 10-3 M 1.665 M 1.747 M 100.0 M 104.9 M

Which of the following are nonelectrolytes in water?

(i) HF

(ii) ethanol, C2H5OH

(iii) CH3CH3

(iv) KClO3

(v) Cu(NO3)2

Online Text

 ii and iii i, ii, and iii i, iv, and v ii iii

## Indicate the concentration of each ion or molecule present in a 0.14 MNaOH solution.Online Text

 0.070 MNa+, 0.070 M OH- 0.14 MNa+, 0.14 M OH- 0.14 MNaOH 0.28 MNa+, 0.14 M OH- 0.14 MNa+, 0.28 M OH- 0.28 MNaOH

## Indicate the concentration of each ion or molecule present in a 0.25 MCaBr2 solution.Online Text

 0.25 M Ca2+, 0.25 MBr- 0.25 M Ca2+, 0.50 MBr- 0.25 M CaBr2 0.50 M Ca2+, 0.50 MBr- 0.50 M Ca2+, 0.25 MBr-

An aqueous solution of an unknown solute is tested with litmus paper and found to be acidic. The solution is weakly conducting compared with a solution of NaCl of the same concentration. Which of the following substances could the unknown be: KOH, NH3, HNO3, KClO2, H3PO3, CH3COCH3?

Online Text

 KOH NH3 HNO3 KClO2 H3PO3 CH3COCH3

## Complete and balance the equation HBr (aq) + Ca(OH)2 (aq) --> Online Text

 HBr (aq) + Ca(OH)2 (aq) --> H2O (l) + Ca+ (aq) + Br- (aq) 2HBr (aq) + Ca(OH)2 (aq) --> 2H2O (l) + Ca2+ (aq) + 2Br- (aq) HBr (aq) + Ca(OH)2 (aq) --> H2O (l) + Ca2+ (aq) + 2Br- (aq) 2HBr (aq) + Ca(OH)2 (aq) --> 2H2O (l) + CaBr2 (s) HBr (aq) + Ca(OH)2 (aq) --> H2O (l) + CaBr2 (s) 2HBr (aq) + Ca(OH)2 (aq) --> H2O (l) + Ca2+ (aq) + 2Br- (aq)

## Complete and balance the equation HClO4 (aq) + Cu(OH)2 (s) --> Online Text

 2HClO4 (aq) + Cu(OH)2 (aq) --> 2H2O (l) + Cu(ClO4)2 (s) HClO4 (aq) + Cu(OH)2 (aq) --> H2O (l) + Cu+ (aq) + ClO4- (aq) HClO4 (aq) + Cu(OH)2 (aq) --> H2O (l) + Cu2+ (aq) + 2ClO4- (aq) 2HClO4 (aq) + Cu(OH)2 (aq) --> 2H2O (l) + Cu2+ (aq) + 2ClO4- (aq) HClO4 (aq) + Cu(OH)2 (aq) --> H2O (l) + Cu(ClO4)2(s) 2HClO4 (aq) + Cu(OH)2 (aq) --> H2O (l) + Cu2+ (aq) + 2ClO4- (aq)

Write a balanced net ionic equation for the following reaction and identify the spectator ion or ions present.

FeO (s) + 2HClO4 (aq) --> H2O (l) + Fe(ClO4)2 (aq)

Online Text

 FeO (s) + 2H+ (aq) + 2ClO4- (aq) --> H2O (l) + Fe2+ + 2ClO4- (aq); no spectator ions FeO (s) + 2H+ (aq) + 2ClO4- (aq) --> H2O (l) + Fe2+ (aq) + 2ClO4- (aq); ClO4- spectator ion FeO (s) + 2H+ (aq) --> H2O (l) + Fe2+ (aq); ClO4- spectator ion FeO (s) + 2H+ (aq) --> H2O (l) + Fe2+ (aq); ClO4-, H+, and Fe2+ spectator ions FeO (s) + 2HClO4 (aq) --> H2O (l) + Fe(ClO4)2 (aq); no spectator ions

Which of the following are soluble?

(i) NiCl2

(ii) Ag2S

(iii) Cs3PO4

(iv) SrCO3

(v) (NH4)2SO4

Online Text

 i, ii, and iii i, ii, and v i and v i only iv and v ii only

## Write a balanced net ionic equation for the reaction, if any, that may occur when the following pair is mixed: AgNO3 (aq) and Na2CO3 (aq) Online Text

 there are only spectator ions 2Na+ (aq) + 2NO3- (aq) --> 2NaNO3 (s) 2Ag+ (aq) + CO32- (aq) --> Ag2CO3 (s) 2Na+ (aq) + 2Ag+ (aq) + 2NO3- (aq) + CO32- (aq) --> Ag2CO3 (s) + 2NaNO3 (s)

## Write a balanced net ionic equation for the reaction, if any, that may occur when the following pair is mixed: Pb(NO3)2 (aq) and MgSO4 (aq). Online Text

 all are spectator ions Pb+ (aq) + SO4- (aq) --> PbSO4 (s) Pb2+ (aq) + SO42- (aq) --> PbSO4 (s) Mg2+ (aq) + 2NO3- (aq) --> Mg(NO3)2 (s) Mg+ (aq) + NO3- (aq) --> MgNO3 (s)

## Write a balanced molecular equation for the reaction of hydrobromic acid with zinc. Online Text

 Zn(s) + HBr(aq) --> ZnBr(aq) + H+(aq) Zn(s) + HCl(aq) --> ZnCl2(aq) + H2(g) Zn(s) + 2HCl(aq) --> ZnCl2(aq) + H2(g) Zn(s) + 2HBr(aq) --> ZnBr2(aq) + H2(g) Zn(s) + HBr(aq) --> ZnBr(aq) + H2(g)

Based on the activity series (Table 4.4), which of the following reactions will occur?

(i)Al (s) + NiCl2 (aq) -->

(ii)Ag (s) + Pb(NO3)2 (aq) -->

(iii)Cr (s) + NiSO4 (aq) -->

Online Text

 i only ii only iii only i and ii i and iii ii and iii

## What volume of 0.115 MHClO4 solution is required to neutralize 50.00 mL of 0.0875 MNaOH? Online Text

 0.115 mL 38.0 L 38.0 mL 50.0 mL 65.7 L 65.7 mL

## What volume of 0.128 MHCl is required to neutralize 2.87 g of Mg(OH)2? Online Text

 0.0126 L 0.385 L 0.769 L 22.4 L 44.8 L

Some sulfuric acid is spilled on a lab bench. It can be neutralized by sprinkling sodium bicarbonate on it and then mopping up the resultant solution. The sodium bicarbonate reacts with sulfuric acid in the following way:

2NaHCO3 (s) + H2SO4 (aq) --> Na2SO4 (aq) + 2CO2 (g) + 2 H2O (l)

Sodium bicarbonate is added until the fizzing due to the formation of CO2 (g) stops. If 35 mL of 6.0 MH2SO4 was spilled, what is the minimum mass of NaHCO3 that must be added to the spill to neutralize the acid?

Online Text

 0.42 g 8.8 g 18 g 35 g 3500 g

## A solution is made by mixing 30.0 mL of 8.00 MHCl, 100 mL of 2.00 M MHCl, and enough water to make 200.0 mL of solution. What is the molarity of HCl in the final solution?Online Text

 0.455 M 1.00 M 1.20 M 2.20 M 0.440 M 9.00 M

Tartaric acid, H2C4H4O6, has two acidic hydrogens. The acid is often present in wines and precipitates from solution as the wine ages. A solution containing an unknown concentration of the acid is titrated with NaOH. It requires 22.62 mL of 2.000 MNaOH solution to titrate both acidic protons in 40.00 mL of the tartaric acid solution. Calculate the molarity of the tartaric acid solution.

Online Text

 0.02262 M 0.04524 M 0.5655 M 1.131 M 0.2000 M 0.4000 M

## If 5.20 g of a salt are found in 2.500 L of a 0.500 Msolution, how may grams would be present in 2.50 L of a 1.50 M solution?Online Text

 5.20 g 10.4 g 15.6 g 1.73 g 7.8 g

## How many milliliters of 0.1000 MCa(OH)2 solution are needed to supply 0.05000 mol of Ca(OH)2? Online Text

 500.0 mL 250.0 mL 2000. mL 167.0 mL 1000. mL

## If 200. mL of a 2.50 MNaOH solution is diluted to 500. mL, what is the new concentration of NaOH?Online Text

 4.20 x 103 M 5.95 M 2.50 M 0.441 M 1.00 M

## What mass of ethanol, C2H5OH, is required to produce 300. mL of a 0.500 Msolution?Online Text

 46.1 g 23.0 g 6.91 g 92.1 g 13.8 g

## Indicate the concentration of ions present in 0.20 MCa(HCO3)2 solution.Online Text

 0.20 MCa2+, 0.20 MHCO3- 0.20 MCa2+, 0.10 MHCO3- 0.20 MCa(HCO3)2 0.20 MCa2+, 0.40 MHCO3- 0.20 MCa2+, 0.20 MCO3-

## Which of the following generates the most ions in dilute aqueous solution?Online Text

 C2H5OH MgCl2 NaCl NaHSO4 CaSO4

## Which of the following is a weak base?Online Text

 NaOH Ca(OH)2 NH3 RbOH Sr(OH)2

## Write the net ionic reaction for the neutralization of HF by NaOH.Online Text

 H+(aq) + OH-(aq) --> H2O HF(aq) + NaOH(aq) --> NaF(aq) + H2O HF(aq) + NaOH(aq) --> Na+(aq) + F-(aq) + H2O H+(aq) + NaOH(aq) --> Na+(aq) + H2O HF(aq) + OH-(aq) --> F-(aq) + H2O

## What is/are the spectator ion(s) when a BaCl2 solution is combined with an H2SO4 solution?Online Text

 Ba2+(aq), H+(aq) SO42-(aq), H+(aq) Cl-(aq) Cl-(aq), H+(aq) H+(aq)

## When NaCl is added to a solution of (i) AgNO3, (ii) Pb(NO3)2, or (iii) Ca(NO3)2, in which case(s) does a precipitate form?Online Text

 AgNO3 only Pb(NO3)2 only Ca(NO3)2 only in all three cases AgNO3 and Pb(NO3)2 only

Which of the following are soluble?

(i) BaSO4

(ii) AgBr

(iii) Sr3(NO3)2

(iv) PbS

(v) Na2CO3

Online Text

 all are soluble iii only iii and v v only i, iii, and iv only

## What is the net ionic equation for NaOH reacting with HClO4?Online Text

 HClO4(aq) + NaOH(aq) --> NaClO4(aq) + H2O HClO4(aq) + OH-(aq) --> ClO4-(aq) + H2O H+(aq) + NaOH(aq) --> Na+(aq) + H2O H+(aq) + OH-(aq) --> H2O

## Write a balanced molecular equation for the reaction of hydrofluoric acid and calcium.Online Text

 Ca(s) + 2HF(aq) --> CaF2(aq) + 2H+(aq) Ca(s) + HF(aq) --> CaF2(aq) + H2(g) Ca(s) + 2HF(aq) --> CaF2(aq) + H2(g) Ca(s) + 2HF(aq) --> CaF(aq) + H2(g)

## Based on the activity series (Table 4.4), which element will react with a solution of iron ions?Online Text

 Hg Ag Cu Sn Zn

Which of the following reactions will occur?

(i)Ni(s) + Zn2+(aq) -->

(ii)Pb(s) + Ag+(aq) -->

(iii)Zn(s) + Ca2+(aq) -->

(iv)Al(s) + Fe2+(aq) -->

Online Text

 i only ii only ii and iv only i and iii only iv only

## What volume of 0.125 MH2SO4 solution is required to neutralize 25.21 mL of 0.540 MNaOH? Online Text

 109 mL 54.4 mL 5.84 mL 11.7 mL 13.6 L

## What volume of 0.125 MH2SO4 is required to neutralize 2.50 g of Ca(OH)2?Online Text

 0.270 mL 0.135 mL 135 mL 270 mL 540 mL

## What volume of 0.125 MH2SO4 is required to completely precipitate all of the barium in 10.00 mL of a 0.150 Mbarium nitrate solution?Online Text

 12.0 mL 24.0 mL 6.00 mL 0.206 mL 8.33 mL

## What is the mass of the precipitate formed when 12.0 mL of 0.150 MNaCl is added to 25.00 mL of a 0.0500 MAgNO3 solution?Online Text

 258 g .258 g 179 g .179 g 36.0 g

## A solution is made of 25.0 mL of 0.250 Msulfuric acid and 15.0 mL of 0.500 Mhydrochloric acid all diluted to 250. mL. What is the resulting concentration of the hydrated proton?Online Text

 80.0 molar .0800 molar .0558 molar .0300 molar .0500 molar