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13 Dec 2019

A flask contains 250.0 mL of nitric acid (HNO3) at an unknown

concentration. Nitric acid is a strong acid and dissociates completely

into its ions when mixed with water.

o 10.0 mL of the original solution is diluted up to 100 mL to give solution

#2.

o 15.0 mL of solution #2 is diluted up to 100.0 mL to form solution #3.

o 5.00 mL of solution #3 is diluted up to 100.0 mL to form solution #4.

o 25.0 mL of solution #4 has a pOH of 10.18.

a. What is the concentration of nitric acid, or [HNO3], in the original

solution?

b. What is the pH of the original solution of nitric acid?

c. What is the pH of solution #2?

d. What is the pOH of solution #3?

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PHOSPHATE STANDARD CALCULATION HELP

Have one correct answer, stuck on where to go from ther. Urgent request, please help

1) Diluting Concentrated Nitric Acid
Calculate the volume of 15 M Nitric acid required to make 300 mL of 1.1 M nitric acid.

a) Volume of 15 M Nitric acid required _____22.0_________ mL

2) Making the Original Phosphate Solution
You weigh out pure NaH2PO4.

Weight of Sodium Dihydrogen phosphate used 0.4567 g

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10 mL of this is pipetted and again diluted to 100.00 mL to make the original phosphate standard.
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4) Measuring the Absorbance of the Standard
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% T of solution 48.0 %
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A 25.00 ml aliquot of a nitric acid solution of unknownconcentration is pipette into a 125ml Erlenmeyer flask and 2 dropsof phenolphthalein are added.
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