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Practice Exercises



 This activity contains 40 questions.

Question 1.
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?

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Question 2.
How many milliliters of 1.50 MKOH solution are needed to supply 0.125 mol of KOH?

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Question 3.

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.

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Question 4.

Which of the following are nonelectrolytes in water?

(i) HF

(ii) ethanol, C2H5OH

(iii) CH3CH3

(iv) KClO3

(v) Cu(NO3)2

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Question 5.
Indicate the concentration of each ion or molecule present in a 0.14 MNaOH solution.

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Question 6.
Indicate the concentration of each ion or molecule present in a 0.25 MCaBr2 solution.

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Question 7.

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?

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Question 8.
Complete and balance the equation HBr (aq) + Ca(OH)2 (aq) -->

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Question 9.
Complete and balance the equation HClO4 (aq) + Cu(OH)2 (s) -->

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Question 10.

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)

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Question 11.

Which of the following are soluble?

(i) NiCl2

(ii) Ag2S

(iii) Cs3PO4

(iv) SrCO3

(v) (NH4)2SO4

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Question 12.
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)

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Question 13.
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).

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Question 14.
Write a balanced molecular equation for the reaction of hydrobromic acid with zinc.

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Question 15.

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) -->

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Question 16.
What volume of 0.115 MHClO4 solution is required to neutralize 50.00 mL of 0.0875 MNaOH?

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Question 17.
What volume of 0.128 MHCl is required to neutralize 2.87 g of Mg(OH)2?

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Question 18.

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?

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Question 19.
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?

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Question 20.

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.

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Question 21.
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?

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Question 22.
How many milliliters of 0.1000 MCa(OH)2 solution are needed to supply 0.05000 mol of Ca(OH)2?

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Question 23.
If 200. mL of a 2.50 MNaOH solution is diluted to 500. mL, what is the new concentration of NaOH?

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Question 24.
What mass of ethanol, C2H5OH, is required to produce 300. mL of a 0.500 Msolution?

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Question 25.
Indicate the concentration of ions present in 0.20 MCa(HCO3)2 solution.

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Question 26.
Which of the following generates the most ions in dilute aqueous solution?

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Question 27.
Which of the following is a weak base?

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Question 28.
Write the net ionic reaction for the neutralization of HF by NaOH.

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Question 29.
What is/are the spectator ion(s) when a BaCl2 solution is combined with an H2SO4 solution?

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Question 30.
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?

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Question 31.

Which of the following are soluble?

(i) BaSO4

(ii) AgBr

(iii) Sr3(NO3)2

(iv) PbS

(v) Na2CO3

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Question 32.
What is the net ionic equation for NaOH reacting with HClO4?

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Question 33.
Write a balanced molecular equation for the reaction of hydrofluoric acid and calcium.

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Question 34.
Based on the activity series (Table 4.4), which element will react with a solution of iron ions?

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Question 35.

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) -->

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Question 36.
What volume of 0.125 MH2SO4 solution is required to neutralize 25.21 mL of 0.540 MNaOH?

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Question 37.
What volume of 0.125 MH2SO4 is required to neutralize 2.50 g of Ca(OH)2?

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Question 38.
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?

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Question 39.
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?

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Question 40.
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?

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