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sveta [45]
3 years ago
11

In the following balanced reaction, what volume of a 3.0 M H2SO4 is required to completely neutralize 200.0 ml of a 2.5 M NaOH?

Chemistry
2 answers:
cupoosta [38]3 years ago
7 0

Answer:

B Plato

Explanation:

insens350 [35]3 years ago
4 0

B) 83 mL

Find the moles of NaOH by using Molarity=moles/volume(L) so Moles = molarity x volume.

Then use the mol ratio to go from moles of NaOH to moles of H2SO4 by dividing the moles of NaOH by 2. Now you're in moles of H2SO4 so again use M = moles/Volume to find the volume. Volume = moles/M.

(The volume is in Liters in the equation but you can use the mL on this problem because your conversions cancel each other out.)

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What volume of 0.08892 M HNO3 is required to react completetly with 0.2352 g of potassium hydrogen phosphate?
galina1969 [7]

Answer:

0.0303 Liters

Explanation:

Given:

Mass of the potassium hydrogen phosphate = 0.2352

Molarity of the HNO₃ Solution = 0.08892 M

Now,

From the reaction it can be observed that 1 mol of potassium hydrogen phosphate reacts with 2 mol of HNO₃

The number of moles of 0.2352 g of potassium hydrogen phosphate

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also,

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Number of moles = 0.2352 / 174.15 = 0.00135 moles

thus,

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Now,

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thus,

for 0.0027 mol of HNO₃, we have

0.08892 = 0.0027 / Volume

or

Volume =  0.0303 Liters

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3 years ago
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