Complete and balance the following equation:

S(s)+HNO3(aq)→H2SO3(aq)+N2O(g)(acidic solution)

Express your answer as a net chemical equation including phases.

Complete and balance the following equation:

BrO3−(aq)+N2H4(aq)→Br2(l)+N2(g)(acidic solution)

Express your answer as a net chemical equation including phases.

Complete and balance the following equation:

H2O2(aq)+ClO2(aq)→ClO2−(aq)+O2(g)(basic solution)

Determine the pH of a 0.046 M iodous acid (HIO2) solution. Iodous acid is a weak acid (Ka = 3.2 ✕ 10−5 M).

Calculate [OH ^-] and pH for each of the following solutions.



(a) 0.0043 M KOH

(b) 0.0341 g of CsOH in 540.0 mL of solution

(c) 28.1 mL of 0.00187 M Ca(OH)₂ diluted to 800 mL

(d) A solution formed by mixing 71.0 mL of 0.000480 M Ca(OH)₂ with 24.0 mL of 1.3 x 10^-3 M KOH

How do you find the lattice energy of ionic compounds?

1. a) What is the net ionic equation for ZnSO₄ + H₂O?

b) Is the solution acidic or basic?

c) Which ion, Zn²⁺ or SO₄^2-, is causing the observed acidity or basicity?

2. What is the net ionic equation for Na₂CO₃ + H₂O?

3. What is the net ionic equation for NaHSO₄ + H₂O?

a) How many grams of hydrogen gas (H2) is produced by the decomposition of 43.7g of ammonia gas (NH3)?

b) If 12.0 moles of H2 were produced, how many grams of NH3 was decomposed?

c) If 12.0 moles of H2 were produced, how many moles of N2 were produced?

2. Describe how you would prepare 100ml of 0.08 M sulfuric acid [H2SO4] from an 18 M concentrated sulfuric acid stock solution.

3. Describe how you would prepare 50 ml of 0.2 M potassium iodate [KIO3] dissolved in the 0.08 M sulfuric acid [H2SO4] that you have prepared above.

4. Describe how you would prepare 25 ml of 3.6 M hydrogen peroxide [h2O2] from a 30% (w/w) stock H2O2 solution (

5. Describe how you would prepare 50 ml of a 3% (w/v) soluble starch solution in water.

Molecular weights:

Malonic acid: 104.6

Manganese sulfate: 169.01

Potassium iodate: 214

Hydrogen peroxide: 34.01

1). Why do some oxygen containing hydrocarbons form hydrogen bonds and others do not?

2). A functional group R would attatch itself to which carbon of an n-propyl group?

What is the pH of a solution formed when 42.0mL of 0.120 M NaOH is added to 50.0mL of 0.120 M CH3COOH? (Ka= 1.8x10^-5)

9.537 g of a non-volatile solute is dissolved in 220.0 g of water.  
The solute does not react with water nor dissociate in solution.  
Assume that the resulting solution displays ideal Raoult's law behaviour.  
At 25°C the vapour pressure of the solution is 23.498 torr.  
The vapour pressure of pure water at 25°C is 23.756 torr.  
Calculate the molar mass of the solute (g/mol).

71.1 g/mol

Now suppose, instead, that 9.537 g of a volatile solute is dissolved in 220.0 g of water.  
This solute also does not react with water nor dissociate in solution.  
The pure solute displays, at 25°C, a vapour pressure of 2.376 torr.  
Again, assume an ideal solution.  
If, at 25°C the vapour pressure of this solution is also 23.498 torr.  
Calculate the molar mass of this volatile solute.

Consider the following equilibrium: Fe(OH)₃(s) D Fe³⁺(aq) + 3OH^–(aq) with K_sp = 1.6 x 10^-39. The activity coefficients for Fe³⁺(aq) and 3OH^–(aq) are 0.445 and 0.900 in a solution with an ionic strength of 0.01M. The pH of the solution was 11.

a. Calculate [OH^–] in the solution.

b. Use the activity coefficients in order to calculate [Fe³⁺] in the solution.

Hydrogen gas can be produced by the reaction of iron metal with steam, as shown in the equation below:

3 Fe (s) + 4 H2O (g) à Fe3O4 (s) + 4 H2 (g)

If 40.00 g of iron are combined with 40.00 g of steam and reacted, calculate (i) how many grams of hydrogen gas will be formed and (ii) how many grams of the excess reagent will remain after the end of the reaction.

Mix the watery environment of Elodea with a pH indicator called phenol red. In the presence of an acid, phenol red will appear yellow. In the presence of a strong base, phenol red will appear purple. Intermediate colors correspond with intermediate pH values. Recall that plants use CO₂ for photosynthesis; the concentration of CO₂ will determine the pH of a solution. Plants also produce CO₂ as a byproduct of cellular respiration.

1. Will a solution with a high concentration of CO₂ be acidic or basic? Why? (search on the internet)
2. As Elodea uses CO₂ during photosynthesis, will the solution become more acidic or basic? If the solution is also mixed with phenol red, what color should it become over time?
3. Will the concentration of CO₂ increase or decrease for Elodea in darkness? What color will the phenol red indicator show over time?
4. Which colors of visible light are used by chlorophyll for photosynthesis? Which are not?
5. Write a hypothesis for how the intensity of light would affect the photosynthetic rate in Elodea.

Isolation of Nicotine from Tobacco

1. Why did you add 5 mL of 3 M NaOH to the mixture prior to the steam distillation?

2. How can you tell when steam distillation is complete when a large quantity of an organic compound is steam distilled?

3. Is the nicotine you isolated pure? Provide experimental evidence to support your answer.

calculate the mean ionic activity of a 0.0350 m Na3PO4 solution for which the mean activity coeffiecient is 0.685.

Answer should be: 0.0547

Please show me how to get there. Thank you