Home Chapter 4: Aqueous Reactions and Solution Stoichiometry Quiz 1

# Quiz 1

This activity contains 12 questions.

## A 25.0-g sample of garden compost was analyzed for chloride content. The sample was dissolved in water, and the chloride was precipitated as silver chloride. 1.58 g of dried precipitate was obtained. Calculate the percent of chloride in the sample.

 3.1 percent. 4.8 percent 6.3 percent 62 percent 1.56 percent

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, or CH3COCH3?

 KClO2 H3PO3 HNO3 CH3COCH3 NH3 KOH

## An aqueous solution of nickel ions will oxidize each of the following metals except

 potassium. tin. aluminum. chromium. barium.

## Based on the activity series (Table 4.5), which element will react with a solution of iron ions?

 Ag Cu Zn Sn Hg

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

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

## Indicate the concentration of each ion or molecule present in a 0.25 M CaBr2 solution.

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

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 M H2SO4 was spilled, what is the minimum mass of NaHCO3 that must be added to the spill to neutralize the acid?

 35280 g 8.8 g 18 g 35 g 0.42 g

## The minerals chalcocite (Cu2S) and malachite (Cu2CO3(OH)2) are two primary sources of copper. What is the oxidation state of copper in each of these minerals?

 The oxidation state of copper in chalcocite is 2+, and in malachite it is 4+. The oxidation state of copper in chalcocite is 2+, and in malachite it is 2+. The oxidation state of copper in chalcocite is 2+, and in malachite it is 1+. The oxidation state of copper in chalcocite is 1+, and in malachite it is 2+. The oxidation state of copper in chalcocite is 1+, and in malachite it is 1+.

## 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?

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

## Which of the following reactions is an acid-base neutralization reaction?

 Ca(OH)2(aq) + 2HI(aq) ---> CaI2(aq) + 2H2O(l) S8(s) + 8O2(g) ---> 8SO2(g) Na3PO4(s) + (H2O) ---> 3Na+(aq) + PO43-(aq) AgNO3(aq) + NaI(aq) ---> AgI(s) + NaNO3(aq) 2Na(s) + 2H2O(l) ---> H2(g) + 2NaOH(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)

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

## 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).

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