Question 1

What is the molarity of a potassium triiodide solution,KI₃(aq),if 30.00 mL of the solution is required to completely react with 25.00 mL of a 0.500 M thiosulfate solution,K₂S₂O₃(aq)? The chemical equation for the reaction is 2 S₂O₃^2-(aq)+ I₃^-(aq)→ S₄O₆^2-(aq)+ 3 I^-(aq).

Accepted Answer

The answer of What is the molarity of a potassium...

Question 2

How many milliliters of 0.200 M FeCl₃ are needed to react with an excess of Na₂S to produce 0.690 g of Fe₂S₃ if the percent yield for the reaction is 65.0%? 3 Na₂S(aq)+ 2 FeCl₃(aq)→ Fe₂S₃(s)+ 6 NaCl(aq)

Accepted Answer

The answer of How many milliliters of 0.200 M FeCl₃...

Question 3

According to the balanced equation shown below,3.00 moles of oxalic acid,H₂C₂O₄,react with ________ moles of permanganate,MnO₄^-. 5 H₂C₂O₄(aq)+ 2 MnO₄^-(aq)+ 6 H⁺^aq)→ 10 CO₂(g)+ Mn²⁺(aq)+ 8 H₂O(l)

Accepted Answer

According to the balanced equation, 5 moles of oxalic acid react with 2 moles of permanganate. Therefore, 3.00 moles of oxalic acid would react with (2/5) * 3.00 = 1.20 moles of permanganate.

Question 4

There are ________ mol of bromide ions in 0.300 L of a 0.150M solution of AlBr₃.

Accepted Answer

The answer of There are ________ mol of bromide ions...

Question 5

If 100.mL of 0.100 M Na₂SO₄ is added to 200.mL of 0.150 M NaCl,what is the concentration of Na⁺ ions in the final solution? Assume that the volumes are additive.

Accepted Answer

The answer of If 100.mL of 0.100 M Na₂SO₄ is...

Question 6

What is the molar concentration of lithium ions in a 0.550 M Li₃PO₄ solution?

Accepted Answer

Li3PO4 dissociates into 3 Li+ ions and 1 PO4^3- ion. Therefore, the concentration of Li+ ions is 3 times the concentration of Li3PO4, which is 0.550 M x 3 = 1.65 M.

Question 7

Calculate the concentration (M)of sodium ions in a solution made by diluting 60.0 mL of a 0.374 M solution of sodium sulfide to a total volume of 350 mL.

Accepted Answer

The initial moles of sodium sulfide are 0.374 M * 0.060 L = 0.02244 moles. Sodium sulfide (Na2S) dissociates into 2 Na+ ions, so moles of Na+ = 2 * 0.02244 = 0.04488 moles. The final concentration of Na+ is 0.04488 moles / 0.350 L = 0.128 M.

Question 8

How many milliliters of 0.550 M hydriodic acid are needed to react with 25.00 mL of 0.217 M CsOH? HI(aq)+ CsOH(aq)→ CsI(aq)+ H₂O(l)

Accepted Answer

First, we need to write out the balanced equation:

HI(aq) + CsOH(aq) → CsI(aq) + H2O(l)

Next, we can use stoichiometry to determine the moles of HI required to react with the 25.00 mL of CsOH solution:

0.217 M CsOH × 0.02500 L = 0.005425 mol CsOH

From the balanced equation, we can see that 1 mole of HI reacts with 1 mole of CsOH. Therefore, we need 0.005425 moles of HI to react with the CsOH.

Now we can use the concentration of the HI solution to determine the volume required:

0.005425 mol HI × (1 L/0.550 mol) × (1000 mL/1 L) = 9.86 mL

Therefore, the answer is C, 9.86 mL.

Question 9

Based on the balanced chemical equation shown below,determine the mass percent of Fe³⁺ in a sample of iron ore,if 22.40 mL of a 0.1000 M stannous chloride,SnCl₂(aq),solution is required to completely react with theFe³⁺ present in the ore sample.The chemical equation for the reaction is 2 Fe³⁺(aq)+ Sn²⁺(aq)→ 2 Fe²⁺(aq)+ Sn⁴⁺(aq).

Accepted Answer

The answer of Based on the balanced chemical equation shown...

Question 10

Based on the balanced chemical equation shown below,determine the molarity of a solution containing Fe²⁺(aq),if 40.00 mL of the Fe²⁺(aq)solution is required to completely react with 30.00 mL of a 0.125 M potassium bromate,KBrO₃(aq),solution.The chemical equation for the reaction is 6 Fe²⁺(aq)+ BrO₃^-(aq)+ 6 H⁺(aq)→ 6 Fe³⁺(aq)+ Br^-(aq)+ 3 H₂O(l).

Accepted Answer

The answer of Based on the balanced chemical equation shown...

Question 11

How many moles of Co²⁺ are present in 0.500 L of a 0.450 M solution of CoI₂?

Accepted Answer

The number of moles of a substance in a solution can be calculated using the formula: moles = molarity × volume (in liters). For a 0.450 M solution with a volume of 0.500 L, the calculation is 0.450 moles/L × 0.500 L = 0.225 moles.

Question 12

When 15.6 mL of 0.500 M AgNO₃ is added to 12.5 mL of 0.300 M NH₄Cl,how many grams of AgCl are formed? AgNO₃(aq)+ NH₄Cl(aq)→ AgCl(s)+ NH₄NO₃(aq)

Accepted Answer

First, correct the chemical formulas: AgNO3 + NH4Cl → AgCl + NH4NO3. To find the mass of AgCl formed, first determine the limiting reactant. Moles of AgNO3 = 15.6 mL * 0.500 M = 0.0078 mol. Moles of NH4Cl = 12.5 mL * 0.300 M = 0.00375 mol. NH4Cl is the limiting reactant. Moles of AgCl formed = moles of NH4Cl = 0.00375 mol. Mass of AgCl = moles * molar mass = 0.00375 mol * 143.32 g/mol = 0.537 g.

Question 13

What is the molar concentration of phosphate ions in a 0.350 M Li₃PO₄ solution?

Accepted Answer

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

Question 14

How many grams of CaCl₂ are formed when 30.00 mL of 0.00237 M Ca(OH)₂ reacts with excess Cl₂ gas? 2 Ca(OH)₂(aq)+ 2 Cl₂(g)→ Ca(OCl)₂(aq)+ CaCl₂(s)+ 2 H₂O(l)

Accepted Answer

First, calculate moles of Ca(OH)₂: 0.00237 M * 0.030 L = 7.11 x 10⁻⁵ moles. From the balanced equation, 1 mole of Ca(OH)₂ produces 1 mole of CaCl₂. Therefore, 7.11 x 10⁻⁵ moles of CaCl₂ are formed. The molar mass of CaCl₂ is approximately 110.98 g/mol. Thus, mass = 7.11 x 10⁻⁵ moles * 110.98 g/mol = 0.00789 g.

Question 15

How many milliliters of 0.260 M Na₂S are needed to react with 35.00 mL of 0.315 M AgNO₃? Na₂S(aq)+ 2 AgNO₃(aq)→ 2 NaNO₃(aq)+ Ag₂S(s)

Accepted Answer

The balanced chemical equation is:Na₂S(aq) + 2 AgNO₃(aq) → 2 NaNO₃(aq) + Ag₂S(s)From the balanced chemical equation, we can see that 1 mole of Na₂S reacts with 2 moles of AgNO₃. Therefore, the number of moles of Na₂S needed to react with 35.00 mL of 0.315 M AgNO₃ is:(35.00 mL AgNO₃) x (1 L/1000 mL) x (0.315 mol AgNO₃/L) x (1 mol Na₂S/2 mol AgNO₃) = 5.58 x 10^-3 mol Na₂SThe volume of 0.260 M Na₂S needed to provide 5.58 x 10^-3 mol Na₂S is:(5.58 x 10^-3 mol Na₂S) x (1 L/0.260 mol Na₂S) x (1000 mL/L) = 21.2 mL Na₂STherefore, the correct answer is A) 21.2 mL.

Question 16

Based on the balanced chemical equation shown below,what volume of 0.250 M K₂S₂O₃(aq),is needed to completely react with 12.44 mL of 0.125 M KI₃(aq),according to the following chemical equation. 2 S₂O₃^2-(aq)+ I₃^-(aq)→ S₄O₆^2-(aq)+ 3 I^-(aq)

Accepted Answer

The answer of Based on the balanced chemical equation shown...

Question 17

A student dissolved 5.00 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 in the final solution?

Accepted Answer

The answer of A student dissolved 5.00 g of Co(NO₃)₂...

Question 18

Balance the chemical equation given below,and determine the number of milliliters of 0.00300 M phosphoric acid required to neutralize 35.00 mL of 0.00150 M calcium hydroxide. _____ Ca(OH)₂(aq)+ _____ H₃PO₄(aq)→ _____ Ca₃(PO₄)₂(aq)+ _____ H₂O(l)

Accepted Answer

The balanced chemical equation is:

3 Ca(OH)2(aq) + 2 H3PO4(aq) → Ca3(PO4)2(s) + 6 H2O(l)

According to the equation, 3 moles of calcium hydroxide react with 2 moles of phosphoric acid. Therefore, the number of moles of phosphoric acid required to neutralize 35.00 mL of 0.00150 M calcium hydroxide is:

(35.00 mL) x (0.00150 mol/L) = 0.0525 mmol Ca(OH)2

(0.0525 mmol Ca(OH)2) x (2 mmol H3PO4/3 mmol Ca(OH)2) = 0.0350 mmol H3PO4

To calculate the volume of 0.00300 M phosphoric acid required to provide 0.0350 mmol H3PO4, we can use the equation:

Molarity = moles of solute / volume of solution (in L)

Volume of solution (in L) = moles of solute / molarity

Volume of solution (in L) = 0.0350 mmol / (0.00300 mol/L) = 11.7 mL

Therefore, the answer is B, 11.7 mL.

Question 19

How many sodium ions are present in 30.0 mL of 0.600 M Na₂CO₃ solution?

Accepted Answer

To find the number of sodium ions, first calculate the moles of Na₂CO in 30.0 mL (0.030 L) of a 0.600 M solution using the formula moles = concentration × volume. This gives 0.600 mol/L × 0.030 L = 0.018 mol. Since each formula unit of Na₂CO contains one sodium ion, there are also 0.018 mol of sodium ions. To find the number of ions, multiply the moles by Avogadro's number (6.022 × 10^23 ions/mol), resulting in 0.018 mol × 6.022 × 10^23 ions/mol = 1.08 × 10^22 ions, which matches choice B.

Question 20

How many carbonate ions are present in 30.0 mL of 0.600 M Li₂CO₃ solution?

Accepted Answer

The answer of How many carbonate ions are present in...

Quiz 4: Chemical Quantities and Aqueous Reactions

What is the molarity of a potassium triiodide solution,KI₃(aq) ,if 30.00 mL of the solution is required to completely react with 25.00 mL of a 0.500 M thiosulfate solution,K₂S₂O₃(aq) ? The chemical equation for the reaction is 2 S₂O₃^2-(aq) + I₃^-(aq) → S₄O₆^2-(aq) + 3 I^-(aq) .

How many milliliters of 0.200 M FeCl₃ are needed to react with an excess of Na₂S to produce 0.690 g of Fe₂S₃ if the percent yield for the reaction is 65.0%? 3 Na₂S(aq) + 2 FeCl₃(aq) → Fe₂S₃(s) + 6 NaCl(aq)

According to the balanced equation shown below,3.00 moles of oxalic acid,H₂C₂O₄,react with ________ moles of permanganate,MnO₄^-. 5 H₂C₂O₄(aq) + 2 MnO₄^-(aq) + 6 H⁺^aq) → 10 CO₂(g) + Mn²⁺(aq) + 8 H₂O(l)

There are ________ mol of bromide ions in 0.300 L of a 0.150M solution of AlBr₃.

If 100.mL of 0.100 M Na₂SO₄ is added to 200.mL of 0.150 M NaCl,what is the concentration of Na⁺ ions in the final solution? Assume that the volumes are additive.

What is the molar concentration of lithium ions in a 0.550 M Li₃PO₄ solution?

Calculate the concentration (M) of sodium ions in a solution made by diluting 60.0 mL of a 0.374 M solution of sodium sulfide to a total volume of 350 mL.

How many milliliters of 0.550 M hydriodic acid are needed to react with 25.00 mL of 0.217 M CsOH? HI(aq) + CsOH(aq) → CsI(aq) + H₂O(l)

How many moles of Co²⁺ are present in 0.500 L of a 0.450 M solution of CoI₂?

When 15.6 mL of 0.500 M AgNO₃ is added to 12.5 mL of 0.300 M NH₄Cl,how many grams of AgCl are formed? AgNO₃(aq) + NH₄Cl(aq) → AgCl(s) + NH₄NO₃(aq)

What is the molar concentration of phosphate ions in a 0.350 M Li₃PO₄ solution?

How many grams of CaCl₂ are formed when 30.00 mL of 0.00237 M Ca(OH) ₂ reacts with excess Cl₂ gas? 2 Ca(OH) ₂(aq) + 2 Cl₂(g) → Ca(OCl) ₂(aq) + CaCl₂(s) + 2 H₂O(l)

How many milliliters of 0.260 M Na₂S are needed to react with 35.00 mL of 0.315 M AgNO₃? Na₂S(aq) + 2 AgNO₃(aq) → 2 NaNO₃(aq) + Ag₂S(s)

Based on the balanced chemical equation shown below,what volume of 0.250 M K₂S₂O₃(aq) ,is needed to completely react with 12.44 mL of 0.125 M KI₃(aq) ,according to the following chemical equation. 2 S₂O₃^2-(aq) + I₃^-(aq) → S₄O₆^2-(aq) + 3 I^-(aq)

A student dissolved 5.00 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 in the final solution?

Balance the chemical equation given below,and determine the number of milliliters of 0.00300 M phosphoric acid required to neutralize 35.00 mL of 0.00150 M calcium hydroxide. ___ Ca(OH) ₂(aq) + _ H₃PO₄(aq) → _ Ca₃(PO₄) ₂(aq) + ___ H₂O(l)

How many sodium ions are present in 30.0 mL of 0.600 M Na₂CO₃ solution?

How many carbonate ions are present in 30.0 mL of 0.600 M Li₂CO₃ solution?

Quiz 4: Chemical Quantities and Aqueous Reactions

What is the molarity of a potassium triiodide solution,KI3(aq) ,if 30.00 mL of the solution is required to completely react with 25.00 mL of a 0.500 M thiosulfate solution,K2S2O3(aq) ? The chemical equation for the reaction is 2 S2O32-(aq) + I3-(aq) → S4O62-(aq) + 3 I-(aq) .

How many milliliters of 0.200 M FeCl3 are needed to react with an excess of Na2S to produce 0.690 g of Fe2S3 if the percent yield for the reaction is 65.0%? 3 Na2S(aq) + 2 FeCl3(aq) → Fe2S3(s) + 6 NaCl(aq)

According to the balanced equation shown below,3.00 moles of oxalic acid,H2C2O4,react with ________ moles of permanganate,MnO4-. 5 H2C2O4(aq) + 2 MnO4-(aq) + 6 H+aq) → 10 CO2(g) + Mn2+(aq) + 8 H2O(l)

There are ________ mol of bromide ions in 0.300 L of a 0.150M solution of AlBr3.

If 100.mL of 0.100 M Na2SO4 is added to 200.mL of 0.150 M NaCl,what is the concentration of Na+ ions in the final solution? Assume that the volumes are additive.

What is the molar concentration of lithium ions in a 0.550 M Li3PO4 solution?

Calculate the concentration (M) of sodium ions in a solution made by diluting 60.0 mL of a 0.374 M solution of sodium sulfide to a total volume of 350 mL.

How many milliliters of 0.550 M hydriodic acid are needed to react with 25.00 mL of 0.217 M CsOH? HI(aq) + CsOH(aq) → CsI(aq) + H2O(l)

How many moles of Co2+ are present in 0.500 L of a 0.450 M solution of CoI2?

When 15.6 mL of 0.500 M AgNO3 is added to 12.5 mL of 0.300 M NH4Cl,how many grams of AgCl are formed? AgNO3(aq) + NH4Cl(aq) → AgCl(s) + NH4NO3(aq)

What is the molar concentration of phosphate ions in a 0.350 M Li3PO4 solution?

How many grams of CaCl2 are formed when 30.00 mL of 0.00237 M Ca(OH) 2 reacts with excess Cl2 gas? 2 Ca(OH) 2(aq) + 2 Cl2(g) → Ca(OCl) 2(aq) + CaCl2(s) + 2 H2O(l)

How many milliliters of 0.260 M Na2S are needed to react with 35.00 mL of 0.315 M AgNO3? Na2S(aq) + 2 AgNO3(aq) → 2 NaNO3(aq) + Ag2S(s)

Based on the balanced chemical equation shown below,what volume of 0.250 M K2S2O3(aq) ,is needed to completely react with 12.44 mL of 0.125 M KI3(aq) ,according to the following chemical equation. 2 S2O32-(aq) + I3-(aq) → S4O62-(aq) + 3 I-(aq)

A student dissolved 5.00 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 in the final solution?

Balance the chemical equation given below,and determine the number of milliliters of 0.00300 M phosphoric acid required to neutralize 35.00 mL of 0.00150 M calcium hydroxide. _____ Ca(OH) 2(aq) + _____ H3PO4(aq) → _____ Ca3(PO4) 2(aq) + _____ H2O(l)

How many sodium ions are present in 30.0 mL of 0.600 M Na2CO3 solution?

How many carbonate ions are present in 30.0 mL of 0.600 M Li2CO3 solution?

What is the molarity of a potassium triiodide solution,KI₃(aq) ,if 30.00 mL of the solution is required to completely react with 25.00 mL of a 0.500 M thiosulfate solution,K₂S₂O₃(aq) ? The chemical equation for the reaction is 2 S₂O₃^2-(aq) + I₃^-(aq) → S₄O₆^2-(aq) + 3 I^-(aq) .

How many milliliters of 0.200 M FeCl₃ are needed to react with an excess of Na₂S to produce 0.690 g of Fe₂S₃ if the percent yield for the reaction is 65.0%? 3 Na₂S(aq) + 2 FeCl₃(aq) → Fe₂S₃(s) + 6 NaCl(aq)

According to the balanced equation shown below,3.00 moles of oxalic acid,H₂C₂O₄,react with ________ moles of permanganate,MnO₄^-. 5 H₂C₂O₄(aq) + 2 MnO₄^-(aq) + 6 H⁺^aq) → 10 CO₂(g) + Mn²⁺(aq) + 8 H₂O(l)

There are ________ mol of bromide ions in 0.300 L of a 0.150M solution of AlBr₃.

If 100.mL of 0.100 M Na₂SO₄ is added to 200.mL of 0.150 M NaCl,what is the concentration of Na⁺ ions in the final solution? Assume that the volumes are additive.

What is the molar concentration of lithium ions in a 0.550 M Li₃PO₄ solution?

How many milliliters of 0.550 M hydriodic acid are needed to react with 25.00 mL of 0.217 M CsOH? HI(aq) + CsOH(aq) → CsI(aq) + H₂O(l)

How many moles of Co²⁺ are present in 0.500 L of a 0.450 M solution of CoI₂?

When 15.6 mL of 0.500 M AgNO₃ is added to 12.5 mL of 0.300 M NH₄Cl,how many grams of AgCl are formed? AgNO₃(aq) + NH₄Cl(aq) → AgCl(s) + NH₄NO₃(aq)

What is the molar concentration of phosphate ions in a 0.350 M Li₃PO₄ solution?

How many grams of CaCl₂ are formed when 30.00 mL of 0.00237 M Ca(OH) ₂ reacts with excess Cl₂ gas? 2 Ca(OH) ₂(aq) + 2 Cl₂(g) → Ca(OCl) ₂(aq) + CaCl₂(s) + 2 H₂O(l)

How many milliliters of 0.260 M Na₂S are needed to react with 35.00 mL of 0.315 M AgNO₃? Na₂S(aq) + 2 AgNO₃(aq) → 2 NaNO₃(aq) + Ag₂S(s)

Based on the balanced chemical equation shown below,what volume of 0.250 M K₂S₂O₃(aq) ,is needed to completely react with 12.44 mL of 0.125 M KI₃(aq) ,according to the following chemical equation. 2 S₂O₃^2-(aq) + I₃^-(aq) → S₄O₆^2-(aq) + 3 I^-(aq)

A student dissolved 5.00 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 in the final solution?

Balance the chemical equation given below,and determine the number of milliliters of 0.00300 M phosphoric acid required to neutralize 35.00 mL of 0.00150 M calcium hydroxide. ___ Ca(OH) ₂(aq) + _ H₃PO₄(aq) → _ Ca₃(PO₄) ₂(aq) + ___ H₂O(l)

How many sodium ions are present in 30.0 mL of 0.600 M Na₂CO₃ solution?

How many carbonate ions are present in 30.0 mL of 0.600 M Li₂CO₃ solution?