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Dahasolnce [82]
3 years ago
11

You are required to prepare 500 ml of a 6.00 M solution of HNO3 from a stock solution of 12.0 M. Describe in detail how you woul

d go about preparing this solution. Clearly state the volume of stock solution used, the glassware's used and the procedure. ​
Chemistry
1 answer:
andriy [413]3 years ago
8 0

Answer: 250 ml of stock solution with molarity of 12.0 M is measured using a pipette and 250 ml of water is added to volumetric flask of 500 ml to make the final volume of 500 ml.

Explanation:

According to the dilution law,

C_1V_1=C_2V_2

where,

C_1 = concentration of stock solution = 12.0 M

V_1 = volume of stock solution = ?

C_2 = concentration of diluted solution= 6.00 M

V_2 = volume of diluted acid solution = 500 ml

Putting in the values we get:

12.0\times V_1=6.00\times 500

V_1=250ml

Thus 250 ml of stock solution with molarity of 12.0 M is measured using a pipette and 250 ml of water is added to volumetric flask of 500 ml to make the final volume of 500 ml.

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2 years ago
How many grams of ammonia (NH3) can be produced by the synthesis of excess hydrogen gas (H2) and 253.8 grams of nitrogen gas (N2
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Answer:

308.2 g of NH₃.

Explanation:

We'll begin by writing the balanced equation for the reaction. This is illustrated below:

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Next, we shall determine the mass of N₂ that reacted and the mass of NH₃ produced from the balanced equation. This can be obtained as follow:

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Summary:

From the balanced equation above,

28 g of N₂ reacted to produce 34 g of NH₃.

Finally, we shall determine the mass of NH₃ produced by the reaction of 253.8 g of N₂. This can be obtained as illustrated below:

From the balanced equation above,

28 g of N₂ reacted to produce 34 g of NH₃.

Therefore, 253.8 g of N₂ will react to produce = (253.8 × 34)/28 = 308.2 g of NH₃.

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