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3 years ago

what is the molarity of an HCI solution if 25.0 ml of 0.185 M NaOH is required to neutralize 0.0200 L of HCI?

Chemistry

1 answer:

tekilochka [14]3 years ago

3 0

Answer:

0.231 M.

Explanation:

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

HCl + NaOH —> NaCl + H2O

From the balanced equation above, we obtained the following data:

Mole ratio of the acid, HCl (nA) = 1

Mole ratio of the base, NaOH (nB) = 1

Next, the data obtained from the question:

Volume of base, NaOH (Vb) = 25 mL

Molarity of base, NaOH (Mb) = 0.185 M

Volume of acid, HCl (Va) = 0.0200 L

Molarity of acid, HCl (Ma) =?

Next, we shall convert 0.0200 L to mL

This can be obtained as follow:

1 L = 1000 mL

Therefore,

0.0200 L = 0.0200 L × 1000 mL /1 L

0.0200 L = 20 mL

Thus, 0.0200 L is equivalent to 20 mL.

Finally, we shall determine the molarity of the acid solution as follow:

Mole ratio of the acid, HCl (nA) = 1

Mole ratio of the base, NaOH (nB) = 1

Volume of base, NaOH (Vb) = 25 mL

Molarity of base, NaOH (Mb) = 0.185 M

Volume of acid, HCl (Va) = 20 mL

Molarity of acid, HCl (Ma) =?

MaVa / MbVb = nA/nB

Ma × 20 / 0.185 × 25 = 1

Ma × 20 / 4.625 = 1

Cross multiply

Ma × 20 = 4.625 × 1

Ma × 20 = 4.625

Divide both side by 20

Ma = 4.625 / 20

Ma = 0.231 M

Thus, the molarity of the acid solution is 0.231 M.

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Answer:

36.92 mg of oxygen required for bio-degradation.

Explanation:

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2 years ago

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3 years ago

• We obtained the above 10.00-mL solution by diluting a stock solution using a 1.00-mL aliquot and placing it into a 25.00-mL vo

garik1379 [7]

Answer:

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

b) 0.0035 mole

c) 0.166 M

Explanation:

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

The equation of the reaction is expressed as:

$H_3PO_4 \ + \ 3NaOH -----> Na_3 PO_4 \ + \ 3H_2O$

1 mole 3 mole

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

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

$H_3PO_4 \ + \ 3NaOH -----> Na_3 PO_4 \ + \ 3H_2O$

10 ml 17.50 ml

(x) M 0.200 M

Molarity = $\frac{0.2*17.5}{1000}$

= 0.0035 mole

c) What was the molar concentration of phosphoric acid in the original stock solution?

By stoichiometry, converting moles of NaOH to H₃PO₄; we have

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

= 0.00166 mole of H₃PO₄

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

∴ the molar concentration of phosphoric acid in the original stock solution = 0.166 M

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3 years ago

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2 years ago

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Answer:

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Explanation:

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This is how it starts out.

Left:

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Right

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So the place to start with this equation is to bring the Cls up to 2

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But the Nas are now out of kilter.

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Now the right has a problem. There's only 1 Na

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Check it out. It looks like we are done.

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2 years ago

what is the molarity of an HCI solution if 25.0 ml of 0.185 M NaOH is required to neutralize 0.0200 L of HCI?​

what is the molarity of an HCI solution if 25.0 ml of 0.185 M NaOH is required to neutralize 0.0200 L of HCI?