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If an acid has a normality of 1N, it means the acid concentration is equivalent to one mole of H+/liter of solution. Thus a 1 molar (1M) concentration of sulfuric acid will have a normality of 2N, but a 1M solution of HCl will be only 1N. If you mix 7 liters of a sulfuric acid solution (with a concentration of 3N) with 3 liters of a sodium sulfate solution (2 molar concentration), calculate the molarity of the sulfate in the final solution. (i.e. moles of sulfate/liter solution).

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Trinidad TremblayLv2
28 Sep 2019
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Related questions

I know its a lot of questions but anything helps! please help me im so lost!

1. Using the Beer’s law equation, A=εbc, where A - the unit-less absorbance, c - the molarity of the solution, and b - the path length in centimeters, find the units for the molar extinction coefficient, ε. Show your work. Don’t include numbers. (10 pts)

2. Given the following data for a colored solution, find the concentration of the unknown sample given. You will need to print a graph of absorbance vs. concentration as discussed in the experiment to do this. This cannot be done by hand for credit. Please remember to include the graph with your prelab and label each axis. A title should be given to all graphs. (10 pts)

Trial

Concentration,

(moles/liter)

Absorbance

(unit-less values)

1

0.080

0.399

2

0.16

0.715

3

0.24

0.950

4

0.32

1.136

5

0.40

1.429

Unknown Solution A

X

1.337

The concentration of unknown solution A is (moles/liter) ________________________

Show your calculation with units here:

3. Determine the total amount of the stock solution you will need for this experiment. Record that volume here and then in the procedure where there’s a blank for it: ________________________________mL of stock solution is needed for this experiment. (10 pts)

4. This multiple part question deals with concentrations.(10 pts)

A) What is the final concentration of iron(III) sulfate made if 17.804 grams of the solid is added to a 100.00 mL volumetric flask and then distilled water is added to the graduation. Assume the solid is anhydrous iron sulfate.

B) What is the concentration of sulfate ion in the solution?

C) What is the concentration of Fe3+ in the solution? Show your work.

5. You need 0.5000 M copper(II) sulfate solution for this experiment. Remember that copper(II) sulfate exists as a pentahydrate. (10 pts)

A) What is a hydrate?

B) What is the formula for copper (II) sulfate pentahydrate? What is the formula mass of this compound?

C) How would you, exactly, make 50.00 mL of a 0.515 M copper (II) sulfate solution?

D) Tell the exact mass of the solid needed.

Q. When a pink aqueous solution of potassium permanganate, faintly acidified with dilute sulfuric acid was treated with 10% aq. hydrogen peroxide, the reaction took place with the evolution of gas bubbles, and the pink solution was turned colorless. Further chemical analysis revealed that the evolved gas was oxygen, and the resulting solution contains potassium sulfate and manganese (II) sulfate; water was also formed during the same reaction. Please answer the followings:
1) Write down the balanced chemical equation for this reaction.

2) Define the type/types of the reaction; assign the oxidation number of Manganese in potassium permanganate and manganese (II) sulfate. Also, offer an explanation for the color change.


3) Write down the ions present in the solution before & after the reaction. If 100 mL 0.5 M potassium permanganate was mixed with 50 mL 2 M sulfuric acid, what will be the final pH (>7 or <7) of the solution?


4) After the completion of reaction, when evolution of gas-bubbles ceased, what will happen if an aqueous solution of sodium carbonate was added to the reaction mixture? Please write down the net ionic equation.


5) If initially 5.65 g of potassium permanganate was taken for the reaction, calculate the total mass of manganese (II) sulfate present in the solution after the completion of the reaction. What is the Manganese ion concentration of the solution (assume that the total volume of the final reaction mixture is 500 mL)?


Useful hints: hydrogen peroxide is a strong oxidizing agent and considered to be a molecular compound

Can I get all of the question answered in a way that I know under which sub question the answer goes please.

Can I get all of the questions answered in a way that I know how it fits in the question. Some parts are explanations. Thank you.

Q. When a pink aqueous solution of potassium permanganate, faintly acidified with dilute sulfuric acid was treated with 10% aq. hydrogen peroxide, the reaction took place with the evolution of gas bubbles, and the pink solution was turned colorless. Further chemical analysis revealed that the evolved gas was oxygen, and the resulting solution contains potassium sulfate and manganese (II) sulfate; water was also formed during the same reaction. Please answer the followings:

1) Write down the balanced chemical equation for this reaction.

2) Define the type/types of the reaction; assign the oxidation number of Manganese in potassium permanganate and manganese (II) sulfate. Also, offer an explanation for the color change.

3) Write down the ions present in the solution before & after the reaction. If 100 mL 0.5 M potassium permanganate was mixed with 50 mL 2 M sulfuric acid, what will be the final pH (>7 or <7) of the solution?

4) After the completion of reaction, when evolution of gas-bubbles ceased, what will happen if an aqueous solution of sodium carbonate was added to the reaction mixture? Please write down the net ionic equation.

5) If initially 5.65 g of potassium permanganate was taken for the reaction, calculate the total mass of manganese (II) sulfate present in the solution after the completion of the reaction. What is the Manganese ion concentration of the solution (assume that the total volume of the final reaction mixture is 500 mL)?

Useful hints: hydrogen peroxide is a strong oxidizing agent and considered to be a molecular compound.

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