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bija089 [108]
3 years ago
9

Calculate the molarity of a 10.0% (by mass) aqueous solution of hydrochloric acid.

Chemistry
1 answer:
olga2289 [7]3 years ago
6 0

The question is incomplete,the complete question :

Calculate the molality of a 10.0% (by mass) aqueous solution of hydrochloric acid:

a) 0.274 m

b) 2.74 m

c) 3.05 m

d) 4.33 m

e) the density of the solution is needed to solve the problem

Answer:

The molality of a 10.0% (by mass) aqueous solution of hydrochloric acid is 3.05 mol/kg.

Explanation:

10.0% (by mass) aqueous solution of hydrochloric acid.

10 grams of HCl is present in 100 g of solution.

Mass of HCl = 10 g

Mass of solution = 100 g

Mass of solution = Mass of solute + Mass of water

Mass of water = 100 g - 10 g = 90 g

Moles of HCl = \frac{10 g}{36.5 g/mol}=0.2740 mol

Mass of water in kilograms = 0.090 kg

Molality = \frac{0.2740 mol}{0.090 kg}=3.05 mol/kg

The molality of a 10.0% (by mass) aqueous solution of hydrochloric acid is 3.05 mol/kg.

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a) The relationship at equivalence is that 1 mole of phosphoric acid will need three moles of sodium hydroxide.

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Phosphoric acid is tripotic because it has 3 acidic hydrogen atom surrounding it.

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b)  if 10.00 mL of a phosphoric acid solution required the addition of 17.50 mL of a 0.200 M NaOH(aq) to reach the endpoint; Then the molarity of the solution is calculated as follows

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= 0.0035 \ mole \ of NaOH* \frac{1 mole of H_3PO_4}{3 \ mole \ of \ NaOH}

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Using the molarity equation to determine the molar concentration of phosphoric acid in the original stock solution; we have:

Molar Concentration =  \frac{mole \ \ of \ soulte }{ Volume \ of \ solution }

Molar Concentration = \frac{0.00166 \ mole \ of \  H_3PO_4 }{10}*1000

Molar Concentration = 0.166 M

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