Deck 4: Chemical Reactions in Solution

Question 1

Using solubility guidelines, which of the following ionic compounds is not properly labeled with respect to solubility in water?

A) NiCl₂ is soluble.
B) Ag₂S is insoluble.
C) Cs₃PO₄ is insoluble.
D) SrCO₃ is insoluble.
E) (NH₄)₂SO₄ is soluble.

Answer 1

Cs₃PO₄ is insoluble.

Question 2

Which compound listed below is not soluble in water?

A) KCl
B) (NH₄)₂CO₃
C) AgNO₃
D) PbSO₄
E) none of these

Answer 2

PbSO₄

Question 3

Which of the following ionic compounds are expected to be soluble in water?
I. PbCl₂
II. Cu(NO₃)₂
III. BaSO₄

A) I only
B) II only
C) III only
D) I and II
E) All of these

Answer 3

II only

Question 4

Choose the correct net ionic equation for the reaction in water of CaCl₂ and Na₃PO₄.

A) 3 CaCl₂ (aq) + 2 Na₃PO₄ (aq)→ Ca₃(PO₄)₂ (s) + 6 NaCl (aq)
B) Ca²⁺ (aq) + PO₄^{3 -} (aq)→ Ca(PO₄) (s)
C) 3 Ca²⁺ (aq) + 2 PO₄^{3 -} (aq)→ Ca₃(PO₄)₂ (s)
D) Cl ^- (aq) + Na⁺ (aq)→ NaCl (aq)
E) none of these

Question 5

Exhibit 4-1 Consider the precipitation reaction below to answer the following problem(s):
AgNO₃ (aq) + K₃PO₄ (aq)→??
Refer to Exhibit 4-1. What two products are formed in this precipitation reaction?

A) Ag₃PO₄ and KNO₃
B) AgPO₄ and K₃NO₃
C) Ag₃N and K₃P and O₂
D) Ag₃P and K₃N and O₂
E) AgK₃ and NO₃PO₄

Question 6

A chemist places AgNO₃ in one flask and NaBr in another. Water is added to both flasks and the mixture in the first flask is added to the second. Which choice below describes correctly the results of this experiment?

A) Both of the compounds in the flasks dissolve when water is added and AgBr precipitates when the contents of the flasks are mixed.
B) Both of the compounds in the flasks dissolve when water is added and NaNO₃ precipitates when the contents of the flasks are mixed.
C) Both of the compounds in the flasks dissolve when water is added and there is no precipitate when the contents of the flasks are mixed.
D) The AgNO₃ does not dissolve in water, but the NaBr does dissolve. There is no change upon mixing the contents of the flasks.
E) none of these

Question 7

Choose the correct net ionic equation for the reaction of HCl and NaOH taking place in H₂O.

A) 2 H⁺ (aq) + OH ^- (aq)→ H₃O⁺ (aq)
B) H + (aq) + OH - (aq) H₂ O ( )
C) 2 Na⁺ (aq) + 2 Cl ^- (aq)→ 2 NaCl (aq)
D) 2 H + (aq) + 2 Cl - (aq) + 2 Na + (aq) + 2 OH - (aq) 2 H₂ O ( ) + 2 NaCl (aq)
E) none of these

Question 8

Which compound listed below is soluble in water?

A) BaSO₄
B) AgCl
C) MgCO₃
D) Na₂CO₃
E) none of these

Question 9

What products are expected and what are the coefficients for these products in a precipitation reaction when the following aqueous solutions are mixed?
3 AgNO₃ (aq) + Cs₃PO₄ (aq)→??

A) AgPO₄ (s) + Cs₃NO₃ (aq)
B) Ag₂PO₄ (s) + 3 Cs(NO₃)₂
C) Ag₃PO₄ (s) + 3 CsNO₃ (aq)
D) AgPO₄ (s) + 3 CsNO₃ (aq)
E) 2 Ag₃N (s) + 2 Cs₃P + 11 O₂

Question 10

Which compound listed below is not soluble in water?

A) BaCO₃
B) BaCl₂
C) Na₂CO₃
D) Na₂SO₄
E) none of these

Question 11

Which compound listed below is soluble in water?

A) BaCl₂
B) AgBr
C) PbSO₄
D) Be(OH)₂
E) none of these

Question 12

Exhibit 4-1 Consider the precipitation reaction below to answer the following problem(s):
AgNO₃ (aq) + K₃PO₄ (aq)→??
Refer to Exhibit 4-1. What is the correct formula for the compound that would precipitate as an insoluble solid from the precipitation reaction above?

A) Ag₃PO₄
B) KNO₃
C) AgPO₄
D) Ag₃N
E) AgK₃

Question 13

Which compound listed below is not soluble in water?

A) NH₄Cl
B) CaCl₂
C) NaOH
D) PbCl₂
E) none of these

Question 14

Which compound listed below is soluble in water?

A) PbCl₂
B) AgNO₃
C) Fe(OH)₃
D) CaCO₃
E) none of these

Question 15

A chemist places Ba(NO₃)₂ in one flask and Na₂SO₄ in another. Water is added to both flasks and the mixture in the first flask is added to the second. Which choice below describes correctly the results of this experiment?

A) Both of the compounds in the flasks dissolve when water is added and NaNO₃ precipitates when the contents of the flasks are mixed.
B) Both of the compounds in the flasks dissolve when water is added and BaSO₄ precipitates when the contents of the flasks are mixed.
C) Both of the compounds in the flasks dissolve when water is added and there is no precipitate when the contents of the flasks are mixed.
D) The Ba(NO₃)₂ does not dissolve in water, but the Na₂SO₄ does dissolve. There is no change upon mixing the contents of the flasks.
E) none of these

Question 16

Which compound listed below is not soluble in water?

A) Na₂CO₃
B) CuCl₂
C) Fe(NO₃)₃
D) BaSO₄
E) NH₄OH

Question 17

Choose the correct net ionic equation for the reaction in water of AgNO₃ and BaCl₂.

A) 2 AgNO₃ (aq) + BaCl₂ (aq)→ 2 AgCl (s) + Ba(NO₃)₂ (aq)
B) Ag²⁺ (aq) + 2 Cl ^- (aq)→ AgCl₂ (s)
C) Ag⁺ (aq) + Cl ^- (aq)→ AgCl (s)
D) Ba²⁺ (aq) + 2 NO₃ ^- (aq)→ Ba(NO₃)₂ (aq)
E) none of these

Question 18

A chemist places CaCO₃ in one flask and KBr in another. Water is added to both flasks and the mixture in the first flask is added to the second. Which choice below describes correctly the results of this experiment?

A) Both of the compounds in the flasks dissolve when water is added and CaBr₂ precipitates when the contents of the flasks are mixed.
B) Both of the compounds in the flasks dissolve when water is added and K₂CO₃ precipitates when the contents of the flasks are mixed.
C) Both of the compounds in the flasks dissolve when water is added and there is no precipitate when the contents of the flasks are mixed.
D) The CaCO₃ does not dissolve in water, but the KBr does dissolve. There is no change upon mixing the contents of the two flasks.
E) none of these

Question 19

Which of the following ionic compounds is considered insoluble in water?

A) (NH₄)₃PO₄
B) Mg(OH)₂
C) Na₂SO₄
D) Pb(NO₃)₂
E) Mg(C₂H₃O₂)₂

Question 20

A chemist places (NH₄)₂SO₄ in one flask and NaI in another. Water is added to both flasks and the mixture in the first flask is added to the second. Which choice below describes correctly the results of this experiment?

A) Both of the compounds in the flasks dissolve when water is added and NH₄I precipitates when the contents of the flasks are mixed.
B) Both of the compounds in the flasks dissolve when water is added and Na₂SO₄ precipitates when the contents of the flasks are mixed.
C) Both of the compounds in the flasks dissolve when water is added and there is no precipitate when the contents of the flasks are mixed.
D) The (NH₄)₂SO₄ does not dissolve in water, but the NaI does dissolve. There is no change upon mixing the contents of flasks
E) none of these

Question 21

What mass of NaOH is needed to make 450 mL of a 2.0 molar solution?

A) 18 g
B) 42 g
C) 36 g
D) 24 g
E) none of these

Question 22

What is the definition for Molarity ?

A) Grams of solute per moles of solute
B) Moles of solute per grams of solution
C) Moles of solute per Liter of solvent
D) Grams of solute per Liter of solution
E) Moles of solute per Liter of solution

Question 23

Exhibit 4-2 Consider mixing an aqueous solution of FeCl₃ with an aqueous solution of KOH:
FeCl₃ (aq) + KOH (aq)→??
Refer to Exhibit 4-2. What is the net ionic equation for this precipitation reaction?

A) Fe³⁺ (aq) + 3 OH ^- (aq)→ Fe(OH)₃ (s)
B) Fe³⁺ (aq) + 3 Cl ^- (aq)→ FeCl₃ (s)
C) Fe³⁺ (aq) + 3 OH ^- (aq)→ FeOH₃ (s)
D) 3 K⁺ (aq) + 3 Cl ^- (aq)→ 3 KCl (s)
E) K⁺ (aq) + Cl₃ (aq)→ KCl₃ (s)

Question 24

Which equation is the net ionic equation for the reaction in water of BeCl₂ and K₂CO₃?

A) BeCl₂ (aq) + K₂CO₃ (aq)→ BeCO₃ (s) + 2 KCl (aq)
B) BeCl₂ (s)→ Be²⁺ (aq) + 2 Cl ^- (aq)
C) K⁺ (aq) + Cl ^- (aq)→ KCl (s)
D) Be²⁺ (aq) + CO₃^{2 -} (aq)→ BeCO₃ (s)
E) none of these

Question 25

What is the molarity of a solution if 0.50 mole of CaCl₂ is dissolved to make 2.00 L of solution?

A) 1.0 molar
B) 2.0 molar
C) 0.50 molar
D) 0.25 molar
E) none of these

Question 26

Which ions are considered spectators in the reaction between aqueous solutions of (NH₄)₃PO₄ and CaCl₂?

A) 3 Ca²⁺ (aq) and 2 PO₄^{3 -} (aq)
B) 6 N^{3 -} , 24 H⁺ (aq) and 6 Cl ^- (aq)
C) 6 NH₄⁺ (aq) and 6 Cl ^- (aq)
D) 3 Ca²⁺ (aq) and 6 Cl ^- (aq)
E) 6 NH₄⁺ (aq) and 2 PO₄^{3 -} (aq)

Question 27

Exhibit 4-2 Consider mixing an aqueous solution of FeCl₃ with an aqueous solution of KOH:
FeCl₃ (aq) + KOH (aq)→??
Refer to Exhibit 4-2. What is the overall equation for the precipitation reaction that ensues?

A) FeCl₃ (aq) + KOH (aq)→ FeOH (s) + KCl₃ (aq)
B) FeCl₃ (aq) + 3 KOH (aq)→ FeOH₃ (s) + 3 KCl₃ (aq)
C) FeCl₃ (aq) + 3 KOH (aq)→ Fe(OH)₃ (s) + 3 KCl (aq)
D) FeCl₃ (aq) + KOH (aq)→ FeK (s) + Cl₃OH (aq)
E) FeCl₃ (aq) + KOH (aq)→ FeCl₃ (aq) + KOH (aq)

Question 28

What is the balanced net ionic equation for the result when the following two aqueous solutions are mixed?
CaCl₂ (aq) and Cs₃PO₄ (aq)

A) Ca²⁺ (aq) + 2 Cl ^- (aq)→ CaCl₂ (s)
B) Ca²⁺ (aq) + PO₄^{3 -} (aq)→ CaPO₄ (s)
C) Cs⁺ (aq) + Cl ^- (aq)→ CsCl (s)
D) 2 Ca²⁺ (aq) + 3 PO₄^{3 -} (aq)→ Ca₂(PO₄)₃ (s)
E) 3 Ca²⁺ (aq) + 2 PO₄^{3 -} (aq)→ Ca₃(PO₄)₂ (s)

Question 29

What mass of KOH is needed to prepare 0.50 L of a 0.100 molar solution?

A) 0.22 g
B) 4.3 g
C) 1.1 g
D) 2.8 g
E) none of these

Question 30

Which equation shown below represents the total ionic equation for the reaction between aqueous solutions of (NH₄)₃PO₄ and CaCl₂?

A) 6 NH₃ (g) + 6 H⁺ (aq) + 2 PO₄^{3 -} (aq) + 3 Ca²⁺ (aq) + 3 Cl₂^{2 -} (aq)→ 3 Ca²⁺ (aq) + 2 PO₄^{3 -} (aq) + 3 (NH₄)₂Cl₂ (s)
B) 6 N^{3 -} (aq) + 24 H⁺ (aq) + 2 P^{3 -} (aq) + 8 O^{2 -} (aq) + 3 Ca²⁺ (aq) + 6 Cl ^- (aq)→ Ca₃(PO₄)₂ (s) + 6 N^{3 -} (aq) + 24 H⁺ (aq) + 6 Cl ^- (aq)
C) 3 NH₄⁺ (aq) + PO₄^{3 -} (aq) + Ca²⁺ (aq) + 2 Cl ^- (aq)→ CaPO₄ (s) + 3 NH₄⁺ (aq) + 2 Cl ^- (aq)
D) 6 NH₄⁺ (aq) + 2 PO₄^{3 -} (aq) + 3 Ca²⁺ (aq) + 6 Cl ^- (aq)→ 3 Ca²⁺ (aq) + 2 PO₄^{3 -} (aq) + 6 NH₄Cl (s)
E) 6 NH₄⁺ (aq) + 2 PO₄^{3 -} (aq) + 3 Ca²⁺ (aq) + 6 Cl ^- (aq)→ Ca₃(PO₄)₂ (s) + 6 NH₄⁺ (aq) + 6 Cl ^- (aq)

Question 31

Which equation is the net ionic equation for the reaction in water of Pb(NO₃)₂ and CsI?

A) Pb(NO₃)₂ (aq) + CsI (aq)→ PbI₂ (s) + 2 CsNO₃ (aq)
B) Pb(NO₃)₂ (s)→ Pb²⁺ (aq) + 2 NO₃ ^- (aq)
C) Cs⁺ (aq) + NO₃ ^- (aq)→ CsNO₃ (s)
D) Pb²⁺ (aq) + 2 I ^- (aq)→ PbI₂ (s)
E) none of these

Question 32

What is the molarity of a solution containing 17.0 grams of NH₃ in 1.20 liters of solution?

A) 0.0706 M
B) 0.833 M
C) 1.20 M
D) 14.2 M
E) None of these

Question 33

What is the molarity of an aqueous solution prepared by dissolving 25.0 grams of Na₂SO₄ in enough water to form 500 mL of solution?
Molar Mass(Na₂SO₄) = 142.0 g/mol

A) 3.52×10 ^{- 4} M Na₂SO₄
B) 0.0500 M Na₂SO₄
C) 0.176 M Na₂SO₄
D) 0.352 M Na₂SO₄
E) 500 M Na₂SO₄

Question 34

What is the molarity of a solution prepared by dissolving 3.4 g of NH₃ in 500 mL of solution?

A) 4.0×10 ^{- 4} M
B) 6.8×10 ^{- 3} M
C) 4.0×10 ^{- 1} M
D) 6.8 M
E) none of these

Question 35

Which equation is the net ionic equation for the reaction in water of BaCl₂ and Na₂SO₄?

A) BaCl₂ (aq) + Na₂SO₄ (aq)→ BaSO₄ (s) + 2 NaCl (aq)
B) BaCl₂ (s)→ Ba²⁺ (aq) + 2 Cl ^- (aq)
C) Ba²⁺ (aq) + SO₄^{2 -} (aq)→ BaSO₄ (s)
D) Na⁺ (aq) + Cl ^- (aq)→ NaCl (s)
E) none of these

Question 36

Exhibit 4-2 Consider mixing an aqueous solution of FeCl₃ with an aqueous solution of KOH:
FeCl₃ (aq) + KOH (aq)→??
Refer to Exhibit 4-2. What spectator ions are present in this precipitation reaction?

A) Fe⁺ (aq) and 3 Cl ^- (aq)
B) K⁺ (aq) and OH ^- (aq)
C) Fe³⁺ (aq) and 3 OH ^- (aq)
D) 3 K⁺ and 3 Cl ^- (aq)
E) K₃⁺ (aq) and Cl₃ ^- (aq)

Question 37

What is the molarity of a solution containing 29.2 grams of NaCl in 0.60 liters of solution?
MM(NaCl) = 58.4 g/mol

A) 0.300 M
B) 0.833 M
C) 3.33 M
D) 48.7 M
E) 1.20 M

Question 38

What mass of I₂ is needed to prepare 50.0 mL of 1.00 M solution?

A) 6.42 g
B) 12.7 g
C) 14.3 g
D) 9.86 g
E) none of these

Question 39

What is the molarity of a solution prepared by dissolving 47 g of KCl in enough water to give 375 mL of solution?
Molar Mass(KCl) = 74.55 g/mol

A) 0.236 M
B) 0.595 M
C) 1.68 M
D) 4.23 M
E) 9.34 M

Question 40

What are the spectator ions and what is the net ionic equation for the following double-replacement, precipitation reaction?
Na₂S (aq) + ZnSO₄ (aq)→Spectator Ions Net reaction
I. Zn²⁺ and S^{2 -} 2 Na⁺ (aq) + SO₄^{2 -} (aq)→Na₂SO₄ (aq)
II. Na⁺ and SO₄^{2 -} Zn²⁺ (aq) + S^{2 -} (aq)→ZnS (s)
III. Na⁺ and Zn²⁺ S^{2 -} (aq) + SO₄^{2 -} (aq)→ S₂O₄^{4 -} (aq)
IV. S^{2 -} and SO₄^{2 -} Na⁺ (aq) + Zn²⁺ (aq)→NaZn³⁺ (aq)
V. Na⁺ and S^{2 -} Zn²⁺ (aq) + SO₄^{2 -} (aq)→ZnSO₄ (s)

A) I
B) II
C) III
D) IV
E) V

Question 41

How many grams of NaCl are required to prepare 500. mL of an aqueous 0.500 M NaCl solution?
MM(NaCl) = 58.44 g/mol

A) 4.28 g NaCl
B) 14.6 g NaCl
C) 58.4 g NaCl
D) 62.8 g NaCl
E) 232 g NaCl

Question 42

How many moles of H₂SO₄ are present in 211 mL of a 4.36 molar solution?

A) 1.12 mol
B) 0.342 mol
C) 0.920 mol
D) 1.42 mol
E) none of these

Question 43

How many grams of NH₃ are present in 2.50 L of 3.00 M NH₃ solution?
Molar Mass(NH₃) = 17.03 g/mol

A) 0.0705 g NH₃
B) 7.50 g NH₃
C) 14.2 g NH₃
D) 20.4 g NH₃
E) 128 g NH₃

Question 44

How many grams of HCl are present in 2.50 L of 3.00 M HCl solution?
Molar Mass(HCl) = 36.46 g/mol

A) 0.0228 g HCl
B) 0.206 g HCl
C) 30.4 g HCl
D) 273 g HCl
E) None of these

Question 45

How many milliliters of 1.50 M KOH solution are needed to provide 0.125 moles of KOH?

A) 0.0833 mL
B) 12.0 mL
C) 83.3 mL
D) 188 mL
E) 1.20×10⁴ mL

Question 46

What volume in milliliters of a 0.200 M NaCl solution is required to provide 1.00 grams of NaCl?
Molar Mass(NaCl) = 58.44 g/mol

A) 3.42 mL of 0.200 M NaCl
B) 11.7 mL of 0.200 M NaCl
C) 85.6 mL of 0.200 M NaCl
D) 292 mL of 0.200 M NaCl
E) 5000 mL of 0.200 M NaCl

Question 47

How many moles of KNO₃ are present in 45.6 mL of a 3.11 molar solution?

A) 0.142 mol
B) 14.3 mol
C) 3.11 mol
D) 142 mol
E) none of these

Question 48

How many grams of NaF are needed to make 250 mL of a 0.22 molar solution?

A) 7.2 g
B) 1.2 g
C) 2.3 g
D) 4.6 g
E) none of these

Question 49

How many grams of KCl is required to prepared 500 mL of a 2.50 M aqueous solution of KCl?
Molar Mass(KCl) = 74.55 g/mol

A) 0.0168 g KCl
B) 0.0671 g KCl
C) 14.9 g KCl
D) 93.2 g KCl
E) 373 g KCl

Question 50

How many grams of H₂SO₄ are present in 75.0 mL of 12.0 M H₂SO₄?
Molar Mass (H₂SO₄) = 98.09 g/mol

A) 1.63 g H₂SO₄
B) 9.18 g H₂SO₄
C) 15.7 g H₂SO₄
D) 88.3 g H₂SO₄
E) 613 g H₂SO₄

Question 51

How many moles of OH ^- ions are present in 422 mL of a 1.21 molar solution of Ba(OH)₂?

A) 2.22 mol
B) 0.312 mol
C) 0.511 mol
D) 1.02 mol
E) none of these

Question 52

How many moles of NO₃ ^- ions are present in 533 mL of a 0.111 molar solution of Ca(NO₃)₂?

A) 0.0300 mol
B) 0.118 mol
C) 0.0592 mol
D) 1.22 mol
E) none of these

Question 53

How many grams of AgNO₃ are present in 50.0 mL of a 12.0 M AgNO₃ solution?
Molar Mass(AgNO₃) = 169.88 g/mol

A) 3.53 g of AgNO₃
B) 40.8 g of AgNO₃
C) 102 g of AgNO₃
D) 283 g of AgNO₃
E) 708 g of AgNO₃

Question 54

How many grams of sodium chloride are needed to prepare 1.4 L of a 1.0 molar solution of sodium chloride?

A) 82 g
B) 44 g
C) 37 g
D) 2.4 g
E) none of these

Question 55

How many moles of Na₃PO₄ are present in 5.00 mL of a 0.226 molar solution?

A) 1.13×10 ^{- 3} mol
B) 1.67×10 ^{- 3} mol
C) 3.33×10 ^{- 3} mol
D) 0.00224 mol
E) none of these

Question 56

How many moles of Ca²⁺ ions are present in 15.6 mL of a 1.21 molar solution of CaCl₂?

A) 0.0189 mol
B) 0.0112 mol
C) 0.102 mol
D) 0.00332 mol
E) none of these

Question 57

How many grams of potassium sulfate are needed to prepare 2.44 L of a 0.0333 molar solution of potassium sulfate?

A) 8.72 g
B) 4.04 g
C) 7.22 g
D) 14.2 g
E) none of these

Question 58

How many grams of solute is present in 164.1 mL of 0.207 M calcium acetate, Ca(C₂H₃O₂)₂?
Molar Mass(Ca(C₂H₃O₂)₂) = 158.17 g/mol

A) 0.200 g Ca(C₂H₃O₂)₂
B) 0.215 g Ca(C₂H₃O₂)₂
C) 4.66 g Ca(C₂H₃O₂)₂
D) 5.01 g Ca(C₂H₃O₂)₂
E) 5.37 g Ca(C₂H₃O₂)₂

Question 59

How many moles of K⁺ ions are present in 2.00 L of a 0.211 molar solution of K₂SO₄?

A) 0.422 mol
B) 0.844 mol
C) 0.211 mol
D) 0.522 mol
E) none of these

Question 60

How many grams of silver nitrate (AgNO₃) are present in 255 mL of 2.50 M silver nitrate solution?
Molar Mass(AgNO₃) = 169.87 g/mol

A) 5.77×10 ^{- 2} g AgNO₃
B) 17.3 g AgNO₃
C) 108 g AgNO₃
D) 266 g AgNO₃
E) 1.67×10³ g AgNO₃

Question 61

What mass of BaSO₄ precipitates from mixing 2.44 L of 0.212 molar BaCl₂ with excess H₂SO₄?

A) 121 g
B) 50.3 g
C) 241 g
D) 101 g
E) none of these

Question 62

What is the final concentration of a NaCl aqueous solution prepared by mixing 20.0 mL of water witH₆0.0 mL of 2.00 M NaCl solution?

A) 0.667 M
B) 1.50 M
C) 2.67 M
D) 3.00 M
E) 6.00 M

Question 63

Concentrated sulfuric acid, H₂SO₄, is 18.0 M. How many milliliters of concentrated sulfuric acid are required to prepare 500 mL of 3.60 M H₂SO₄?

A) 0.400 mL
B) 10.0 mL
C) 100 mL
D) 400 mL
E) 2500 mL

Question 64

How many mL of 10. molar HCl is needed to make up a 200 mL solution oF₄.0 molar HCl?

A) 160 mL
B) 40 mL
C) 80 mL
D) 20 mL
E) none of these

Question 65

What volume of a 2.00 molar standard solution of NaOH is needed to prepare 1.00 L of a 0.0250 molar solution?

A) 12.5 mL
B) 25.0 mL
C) 6.25 mL
D) 18.2 mL
E) none of these

Question 66

What is the final concentration of a NaCl solution prepared by adding 20.0 mL of water to 30.0 mL of 5.0 M NaCl solution?

A) 2.00 M NaCl
B) 3.00 M NaCl
C) 3.33 M NaCl
D) 5.00 M NaCl
E) 7.50 M NaCl

Question 67

What volume of 1.1 M HCl is needed to prepare 100 mL of a 0.20 M HCl solution?

A) 9.0 mL
B) 18 mL
C) 32 mL
D) 36 mL
E) none of these

Question 68

How many milliliters of water must be added to 75.0 mL of 0.150 M AgNO₃ in order to prepare a 0.100 M solution?
(Assume volumes are additive.)

A) 25.0 mL of H₂O
B) 38.0 mL of H₂O
C) 50.0 mL of H₂O
D) 113 mL of H₂O
E) 188 mL of H₂O

Question 69

What mass of AgCl can be formed from the reaction of excess AgNO₃ witH₂ 00 mL of 0.500 M CaCl₂?

A) 28.7 g
B) 14.4 g
C) 57.4 g
D) 20.2 g
E) none of these

Question 70

How many milliliters of water should be added to 25.0 mL of 1.00 M AgNO₃ in order to provide a 0.125 M AgNO₃ solution?

A) 3.13 mL of water
B) 28.1 mL of water
C) 175 mL of water
D) 200 mL of water
E) 225 mL of water

Question 71

How many milliliters of concentrated, 18.0 M H₂SO₄ are required to prepare 250 mL of 3.00 M H₂SO₄?

A) 0.667 mL
B) 24.0 mL
C) 41.7 mL
D) 1500 mL
E) None of these

Question 72

What is the molarity of a solution of H₂SO₄ that is prepared by the dilution of 150 mL of 5.00 molar HCl to 2.00L?

A) 0.500 molar
B) 0.375 molar
C) 0.750 molar
D) 0.150 molar
E) none of these

Question 73

What mass of AgCl is produced by mixing 2.4 g of CaCl₂ with 30 mL of a 2.4 M AgNO₃ solution?

A) 10 g
B) 6.2 g
C) 3.1 g
D) 5.0 g
E) none of these

Question 74

What is the molarity of a solution prepared by diluting 50.0 mL of 0.110 M HCl to a final volume of 75 mL?

A) 0.044 M
B) 0.066 M
C) 0.0733 M
D) 0.165 M
E) None of these

Question 75

What is the molarity of a solution prepared by diluting 25.0 mL of 0.220 M NaCl to a final volume of 75.0 mL?

A) 0.0733 M NaCl
B) 0.220 M NaCl
C) 0.660 M NaCl
D) 1.52 M NaCl
E) 13.6 M NaCl

Question 76

What mass of AgCl forms from the reaction of excess AgNO₃ witH₅0 mL of 0.20 M solution of BaCl₂?

A) 1.4 g
B) 2.9 g
C) 0.70 g
D) 3.4 g
E) none of these

Question 77

What mass of Al(OH)₃ is formed from mixing 1.24 L of 0.332 molar AlCl₃ with excess NaOH?

A) 12.1 g
B) 40.3 g
C) 24.1 g
D) 32.1 g
E) none of these

Question 78

What is the molarity of a solution prepared by diluting 25 mL of 1.2 molar H₂SO₄ to 1.0 L?

A) 0.015 molar
B) 0.060 molar
C) 0.030 molar
D) 0.040 molar
E) none of these

Question 79

What is the molarity of a solution of HCl that is prepared by the dilution of 10 mL of 2.00 molar HCl to 1.00L?

A) 0.500 molar
B) 0.0350 molar
C) 0.0200 molar
D) 0.100 molar
E) none of these

Question 80

What is the molarity of a solution prepared by diluting 75 mL of 2.35 M Na₂SO₄ solution to a final volume of 250 mL?

A) 0.0441 M
B) 0.128 M
C) 0.705 M
D) 1.42 M
E) 7.83 M