Calculate the pH of a solution made by dissolving 10 grams of hydrogen chloride in 1000 mL of water

0.56

Explanation:

Step 1:

Data obtained from the question.

Mass of HCl = 10g

Volume = 1000mL = 1L

Step 2:

Determination of the mole of HCl. This can be obtained as follow:

Molar Mass of HCl = 1 + 35.5 = 36.5g/mol

Mass of HCl = 10g

Mole of HCl =?

Number of mole = Mass/Molar Mass

Mole of HCl = 10/36.5

Mole of HCl = 0.274 mole

Step 3:

Determination of the molarity of HCl. This is illustrated below:

Mole of solute (HCl) = 0.274 mole

Volume = 1L

Molarity =?

Molarity is simply the mole of solute per unit litre of the solution. It is represented mathematically as:

Molarity = mole of solute/Volume of solution

Molarity of HCl = 0.274 mole/1L

Molarity of HCl = 0.274 mol/L

Step 4:

Determination of the hydrogen ion concentration [H+] in 0.274 mol/L HCl.

We'll begin by writing a balanced dissociation equation for HCl. This is shown below:

HCl —> H+ + Cl-

From the above equation, 1 mole of HCl produced 1 mole H+

Therefore, 0.274 mol/L of HCl will also produce 0.274 mol/L of H+

Step 5:

Determination of the pH of the solution.

The pH of a solution is simply the negative logarithm of the hydrogen ion concentration [H+] in the solution. It is represented mathematically as:

pH = - log [H+]

[H+] = 0.274 mol/L

pH = - log [H+]

pH = - log 0.274

pH = 0.56

Therefore, the pH of the solution made by dissolving 10 grams of hydrogen chloride in 1000 mL of water is 0.56

a  solution  is always transparent, light passes through with no scattering from solute particles which are molecule in size. the  solution  is homogeneous and does not settle out. a colloid is intermediate between asolution  and a  suspension. while asuspension  will separate out a colloid will not.

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