Question 1

The reaction Sr(NO₃)₂(aq)+ Cs₂SO₄(aq)→ SrSO₄(s)+ 2 CsNO₃(aq)is best classified as a(n) A)acid-base neutralization reaction. B)oxidation-reduction reaction. C)precipitation reaction. D)single replacement reaction.

Accepted Answer

This is a precipitation reaction as it results in the formation of a solid (SrSO₄) from two aqueous solutions. There is no evidence of acid-base neutralization, oxidation-reduction, or single replacement reactions.

Question 2

What is the concentration of NO₃^- ions in a solution prepared by dissolving 20.0 g of Ca(NO₃)₂ in enough water to produce 300.mL of solution? A)0.203 M B)0.406 M C)0.537 M D)0.813 M

Accepted Answer

The answer of What is the concentration of NO₃^- ions...

Question 3

What is the concentration of an AlCl₃ solution if 150.mL of the solution contains 250.mg of Cl^- ion? A)1.57 × 10^-2 M B)3.75 × 10^-2 M C)4.70 × 10^-2 M D)1.41 × 10^-1 M

Accepted Answer

To find the concentration in moles per liter (M), first convert the mass of Cl^- ion to moles using its molar mass (35.45 g/mol). $250 \, \text{mg} = 0.250 \, \text{g}$, so moles of Cl^- = $0.250 \, \text{g} / 35.45 \, \text{g/mol} = 0.00705 \, \text{mol}$. Then, divide by the volume in liters (0.150 L) to find the concentration: $0.00705 \, \text{mol} / 0.150 \, \text{L} = 0.047 \, \text{M} = 4.7 \times 10^{-2} \, \text{M}$.

Question 4

A student dissolved 3.00 g of Co(NO₃)₂ in enough water to make 100.mL of stock solution.He took 4.00 mL of the stock solution and then diluted it with water to give 275.mL of a final solution.How many grams of NO₃^- ion are there in the final solution? A)0.0148 g B)0.0296 g C)0.0407 g D)0.0813 g

Accepted Answer

The answer of A student dissolved 3.00 g of Co(NO₃)₂...

Question 5

Write a balanced net ionic equation for the reaction of CaI₂(aq)with K₂S(aq). A)CaI₂(aq)+ K₂S(aq)→ CaS (aq)+ 2 KI(aq) B)Ca²⁺(aq)+ 2 I^-(aq)+ 2 K⁺(aq)+ S^2-(aq)→ CaS(s)+ 2 KI(aq) C)Ca²⁺(aq)+ S^2-(aq)→ CaS(s) D)Ca²⁺(aq)+ 2 I^-(aq)+ 2 K⁺(aq)+ S^2-(aq)→ CaS(s)+ 2 KI(s)

Accepted Answer

The correct net ionic equation involves the calcium ion reacting with the sulfide ion to form solid calcium sulfide, with spectator ions removed.

Question 6

The mixing of which pair of reactants will result in a precipitation reaction? A)CsI(aq)+ NaOH(aq) B)HCl(aq)+ Ca(OH)₂(aq) C)K₂SO₄(aq)+ Pb(NO₃)₂(aq) D)NaNO₃(aq)+ NH₄Cl(aq)

Accepted Answer

In Choice C, when KI(aq) is mixed with Pb(NO3)2(aq), a precipitation reaction occurs where PbI2(s) is formed. Choices A, B, and D do not involve the formation of an insoluble solid (precipitate), therefore they are not precipitation reactions.

Question 7

The reaction Ba(s)+ 2 AgNO₃(aq)→ Ba(NO₃)₂(aq)+ 2 Ag(s)is best classified as a(n) A)acid-base neutralization reaction. B)double replacement reaction. C)oxidation-reduction reaction. D)precipitation reaction.

Accepted Answer

This reaction is an oxidation-reduction (redox) reaction, as it involves the transfer of electrons between species. Barium (Ba) is oxidized, and silver (Ag) is reduced.

Question 8

If the reaction of phosphate ion with water is ignored,what is the total concentration of ions in a solution prepared by dissolving 7.00 g of K₃PO₄ in enough water to make 350.mL of solution? A)0.0236 M B)0.0943 M C)0.377 M D)0.754 M

Accepted Answer

The molar mass of K3PO4 is approximately 212.27 g/mol. Dissolving 7.00 g in 350 mL (0.350 L) gives a concentration of 0.0943 M for K3PO4. Since K3PO4 dissociates into 4 ions (3 K+ and 1 PO4^3-), the total ion concentration is 4 times 0.0943 M, which equals 0.377 M.

Question 9

What is the molar concentration of sulfate ions in a 0.450 M K₂SO₄ solution? A)0.225 M B)0.450 M C)0.900 M D)1.35 M

Accepted Answer

The formula given seems to represent a compound with one sulfate ion (SO4^2-) per formula unit. Therefore, the molar concentration of sulfate ions in the solution will be the same as the concentration of the compound itself, which is 0.450 M.

Question 10

Which pair of compounds is soluble in water? A)Hg₂Br₂ and Hg₂I₂ B)CuS and Na₂S C)LiI and Ca(NO₃)₂ D)KNO₃ and CaCO₃

Accepted Answer

LiI and Ca(NO3)2 are both soluble in water. LiI is soluble because lithium salts are generally soluble, and Ca(NO3)2 is soluble because nitrates are soluble in water.

Question 11

Write a balanced net ionic equation for the reaction of AgNO₃(aq)with LiCl(aq). A)AgNO₃(aq)+ LiCl(aq)→ AgCl(aq)+ LiNO₃(s) B)Ag⁺(aq)+ NO₃^-(aq)+ Li⁺(aq)+ Cl^-(aq)→ Ag⁺(aq)+ Cl^-(aq)+ LiNO₃(s) C)Ag⁺(aq)+ NO₃^-(aq)+ Li⁺(aq)+ Cl^-(aq)→ AgBr(s)+ Li⁺(aq)+ NO₃^-(aq) D)Ag⁺(aq)+ Br^-(aq)→ AgBr(s)

Accepted Answer

The correct net ionic equation for the reaction between AgNO3 (silver nitrate) and LiCl (lithium chloride) is Ag^+ (aq) + Cl^- (aq) → AgCl(s), which is not accurately represented by any of the provided choices due to a formatting error in the question. However, choice D seems to attempt to describe a reaction involving silver (Ag^+) and bromide (Br^-) ions to form silver bromide (AgBr), which is unrelated to the given reactants. The correct reaction should involve silver and chloride ions forming silver chloride as a precipitate.

Question 12

HBr,HCl,HClO₄,KBr,and NaCl are all classified as A)acids. B)nonelectrolytes. C)strong electrolytes. D)weak electrolytes.

Accepted Answer

All of the compounds listed are ionic compounds, which means that they dissociate in water to form ions. Strong electrolytes are compounds that dissociate almost completely in water, producing a large number of ions. For example, NaCl will dissociate almost completely in water to form Na+ and Cl- ions. Therefore, all of the compounds listed are strong electrolytes.

Question 13

Which one of the following compounds is soluble in water? A)Cu₃(PO₄)₂ B)FeS C)Hg(NO₃)₂ D)SrCO₃

Accepted Answer

Mercury(I) nitrate, Hg2(NO3)2, is soluble in water due to the general solubility rule that most nitrate (NO3-) salts are soluble in water.

Question 14

The reaction HNO₃(aq)+ KOH(aq)→ KNO₃(aq)+ H₂O(l)is best classified as a(n) A)acid-base neutralization reaction. B)oxidation-reduction reaction. C)precipitation reaction. D)single replacement reaction.

Accepted Answer

The reaction is a classic acid-base neutralization reaction where an acid (HNO₃) reacts with a base (KOH) to produce a salt (KNO₃) and water (H₂O).

Question 15

What is the molarity of chloride ions when 10.4 grams of MgCl₂ is dissolved in 753 mL of water? A)0.00 M B)0.145 M C)0.000290 M D)0.290 M3

Accepted Answer

The molar mass of MgCl2 is approximately 95.21 g/mol. Dissolving 10.4 g of MgCl2 gives 0.109 mol of MgCl2. Since each MgCl2 produces 2 moles of Cl- ions, the moles of Cl- ions are 0.218. The molarity is moles of solute per liter of solution, so 0.218 mol / 0.753 L = 0.290 M.

Question 16

What is the molar concentration of sodium ions in a 0.750 M Na₃PO₄ solution? A)0.250 M B)0.750 M C)2.25 M D)3.00 M

Accepted Answer

The answer of What is the molar concentration of sodium...

Question 17

Which one of the following compounds is insoluble in water? A)Na₂SO₄ B)KNO₃ C)BaSO₄ D)Li₂CO₃

Accepted Answer

BaSO4 (Barium sulfate) is insoluble in water, which is a well-known exception in the solubility rules for sulfates.

Question 18

How many mL of a 0.175 M FeCl₃solution are needed to make 550.mL of a solution that is 0.300 M in Cl^- ion? A)0.943 mL B)314 mL C)943 mL D)It is not possible to make a more concentrated solution from a less concentrated solution.

Accepted Answer

The answer of How many mL of a 0.175 M...

Question 19

Write a balanced net ionic equation for the reaction of Li₂CO₃(s)and HCl(aq). A)Li₂CO₃(s)+ 2 HCl(aq)→ 2 LiCl(aq)+ H₂O(l)+ CO₂(g) B)2Li⁺(aq)+ CO₃^2-(aq)+ 2H⁺(aq)+ 2Cl^-(aq)→ 2Li⁺(aq)+ 2Cl^-(aq)+ H₂O(l)+ CO₂(g) C)Li₂CO₃(s)+ 2 H⁺(aq)→ 2 Li⁺(aq)+ H₂O(l)+ CO₂(g) D)CO₃^2-(aq)+ 2 H⁺(aq)→ H₂O(l)+ CO₂(g)

Accepted Answer

The answer of Write a balanced net ionic equation for...

Question 20

How many mL of a 0.350 M AlI₃ solution are needed to make 700.mL of a solution that is 0.350 M in I^- ion? A)500 mL B)167 mL C)125 mL D)It is not possible to make a more concentrated solution from a less concentrated solution.

Accepted Answer

AlI3 dissociates into Al3+ and 3 I- ions. To get 0.350 M I- ions, you need 1/3 of the concentration of AlI3, so 700 mL * (1/3) = 233.33 mL of 0.350 M AlI3. However, since the solution is already 0.350 M in I-, you need 167 mL of AlI3 to achieve this concentration.

Quiz 4: Reactions in Aqueous Solutions

The reaction Sr(NO₃) ₂(aq) + Cs₂SO₄(aq) → SrSO₄(s) + 2 CsNO₃(aq) is best classified as a(n)

What is the concentration of NO₃^- ions in a solution prepared by dissolving 20.0 g of Ca(NO₃) ₂ in enough water to produce 300.mL of solution?

What is the concentration of an AlCl₃ solution if 150.mL of the solution contains 250.mg of Cl^- ion?

A student dissolved 3.00 g of Co(NO₃) ₂ in enough water to make 100.mL of stock solution.He took 4.00 mL of the stock solution and then diluted it with water to give 275.mL of a final solution.How many grams of NO₃^- ion are there in the final solution?

Write a balanced net ionic equation for the reaction of CaI₂(aq) with K₂S(aq) .

The mixing of which pair of reactants will result in a precipitation reaction?

The reaction Ba(s) + 2 AgNO₃(aq) → Ba(NO₃) ₂(aq) + 2 Ag(s) is best classified as a(n)

If the reaction of phosphate ion with water is ignored,what is the total concentration of ions in a solution prepared by dissolving 7.00 g of K₃PO₄ in enough water to make 350.mL of solution?

What is the molar concentration of sulfate ions in a 0.450 M K₂SO₄ solution?

Which pair of compounds is soluble in water?

Write a balanced net ionic equation for the reaction of AgNO₃(aq) with LiCl(aq) .

HBr,HCl,HClO₄,KBr,and NaCl are all classified as

Which one of the following compounds is soluble in water?

The reaction HNO₃(aq) + KOH(aq) → KNO₃(aq) + H₂O(l) is best classified as a(n)

What is the molarity of chloride ions when 10.4 grams of MgCl₂ is dissolved in 753 mL of water?

What is the molar concentration of sodium ions in a 0.750 M Na₃PO₄ solution?

Which one of the following compounds is insoluble in water?

How many mL of a 0.175 M FeCl₃solution are needed to make 550.mL of a solution that is 0.300 M in Cl^- ion?

Write a balanced net ionic equation for the reaction of Li₂CO₃(s) and HCl(aq) .

How many mL of a 0.350 M AlI₃ solution are needed to make 700.mL of a solution that is 0.350 M in I^- ion?

Quiz 4: Reactions in Aqueous Solutions

The reaction Sr(NO3) 2(aq) + Cs2SO4(aq) → SrSO4(s) + 2 CsNO3(aq) is best classified as a(n)

What is the concentration of NO3- ions in a solution prepared by dissolving 20.0 g of Ca(NO3) 2 in enough water to produce 300.mL of solution?

What is the concentration of an AlCl3 solution if 150.mL of the solution contains 250.mg of Cl- ion?

A student dissolved 3.00 g of Co(NO3) 2 in enough water to make 100.mL of stock solution.He took 4.00 mL of the stock solution and then diluted it with water to give 275.mL of a final solution.How many grams of NO3- ion are there in the final solution?

Write a balanced net ionic equation for the reaction of CaI2(aq) with K2S(aq) .

The mixing of which pair of reactants will result in a precipitation reaction?

The reaction Ba(s) + 2 AgNO3(aq) → Ba(NO3) 2(aq) + 2 Ag(s) is best classified as a(n)

If the reaction of phosphate ion with water is ignored,what is the total concentration of ions in a solution prepared by dissolving 7.00 g of K3PO4 in enough water to make 350.mL of solution?

What is the molar concentration of sulfate ions in a 0.450 M K2SO4 solution?