How do aqueous solutions of ionic and molecular compounds differ?

Balance these equations for reactions occurring in an acidic solution:

(a) NO₃^–  + Zn --> NH₄⁺ + Zn²⁺

(b) Cr³⁺ + BiO₃^– --> Cr₂O₇^2– + Bi³⁺

(c) I₂ + OCl^– --> IO₃^–  + Cl^–

(d) Mn²⁺ + BiO₃^– --> MnO₄^– + Bi³⁺

What mass (in grams) of nitrogen must be added to 8.34 g of argon at 24.17oC, and in a 126.1 L contain for a final pressure of 895 mmHg?

What is the mole fraction of O2 in a mixture of 15.1 g of O2, 8.19 g of N2, and 2.47 g of H2?

What is the mole fraction of N2 in a mixture of 15.1 g of O2, 8.19 g of N2, and 2.47 g of H2?

What is the mole fraction of H2 in a mixture of 15.1 g of O2, 8.19 g of N2, and 2.47 g of H2?

What is the partial pressure in atm of O2 of this mixture if it is held in a 15.20 −L vessel at 15 ∘C?

Which of the following would result as a buffer if any when 1 L of each is mixed together:

a) 0.1 M KOH and 0.2 NH₄Cl

b) 0.2 M HNO₃ and 0.6 M NaNO₃

Please Explain!

The average human body contains 5.70 L of blood with a Fe2+ concentration of 3.20×10−5 M . If a person ingests 7.00 mL of 24.0 mM NaCN, what percentage of iron(II) in the blood would be sequestered by the cyanide ion?

The formation constant* of [M(CN)2]– is 5.30 × 1018, where M is a generic metal. A 0.150-mole quantity of M(NO3) is added to a liter of 0.610 M NaCN solution. What is the concentration of M ions at equilibrium?

An ethylene glycol solution contains 21.2 g of ethylene glycol (C₂H₆O₂) in 89.4 mL of water. (Assume a density of 1.00 g/mL for water.)

Determine the boiling and freezing point of the solution. Express you answer in degrees Celsius.

1. A mole of X reacts at a constant pressure of 43.0 atm via the reaction

X(g)+4Y(g)→2Z(g),      ΔH∘=−75.0 kJ

Before the reaction, the volume of the gaseous mixture was 5.00 L. After the reaction, the volume was 2.00 L. Calculate the value of the total energy change, ΔE, in kilojoules.

2. A 1.2 kg block of iron at 27 ∘C is rapidly heated by a torch such that 15 kJ is transferred to it. What temperature would the block of iron reach assuming the complete transfer of heat and no loss to the surroundings? If the same amount of heat was quickly transferred to a 880 g pellet of copper at 30 ∘C, what temperature would it reach before losing heat to the surroundings? qcs, Fe(s)cs, Cu(s)===mcsΔT0.450 J/g⋅∘C0.385 J/g⋅∘C

3.To determine whether a shiny gold-colored rock is actually gold, a chemistry student decides to measure its heat capacity. She first weighs the rock and finds that it has a mass of 4.7 g. She then finds that, upon absorption of 52.7 J of heat, the rock undergoes a rise in temperature from 25 ∘C to 57 ∘C. Find the specific heat capacity of the substance comprising the rock.

4. A 55.0-g aluminum block initially at 27.5 ∘C absorbs 725 J of heat. What is the final temperature of the aluminum?

Draw the structure of a compound with molecular formula C₅H₁₂ that exhibits only one kind of proton

10B When you need to produce a variety of diluted solutions of a solute, you can dilute a series of stock solutions. A stock solution has a significantly higher concentration of the given solute (typically 101 to 104 times higher than those of the diluted solutions). The high concentration allows many diluted solutions to be prepared using minimal amounts of the stock solution.

What volume of a 6.31  M stock solution do you need to prepare 100.  mL of a 0.2227  M solution of HNO3?

Express the volume to three significant figures with the appropriate units.

10C The absorbance of a cationic iron(II) sample solution was measured in a spectrophotometer, but the instrument returned an error because the absorbance was too high. The sample was then diluted by using a pipette to take 100.0 μL of the sample and injecting it into a cuvette already containing 2.00 mL of water (total volume is 2.00 mL + 100.0 μL). The absorbance value of the diluted solution corresponded to a concentration of 5.92×10⁻⁶  M . What was the concentration of the original solution?

Express the concentration to three significant figures with the appropriate units.

11A The absorbance of a cationic iron(II) sample solution was measured in a spectrophotometer, but the instrument returned an error because the absorbance was too high. The sample was then diluted by using a pipette to take 100.0 μL of the sample and injecting it into a cuvette already containing 2.00 mL of water (total volume is 2.00 mL + 100.0 μL). The absorbance value of the diluted solution corresponded to a concentration of 5.92×10⁻⁶  M . What was the concentration of the original solution?

Express the concentration to three significant figures with the appropriate units.

11B A 429-mL sample of unknown HCl solution reacts completely with Na2CO3 to form 18.1 g CO2. What was the concentration of the HCl solution?

Balance the following electrochemical reaction in an acidic solution:

CrO4^- +S^2- > Cr^3 +(SO4)^2-

Explain or define the following terms:

a) molar absorptivity

b) path length

c) ligand

Ammonia gas, NH3 (g) can be synthesized via the reaction:

2 NO (g) + 5 H₂ (g) -> 2 NH₃ (g) + 2 H₂O (g)

Suppose you start with a 45.8 g of NO and 12.4 g of H₂. Determine the limiting reactant and give the theoretical yield of ammonia, in grams. The molar mass of NO is 30.01 g/mol, and the molar mass of H₂ is 2.02 g/mol.