Question

Calculate the ph of a solution that was prepared with 1.46 g of hcl to produce 750 ml of aqueous solution.

Answer 1

Answer:

pH = 1.27

Explanation:

The reaction is:

HCl(aq)  ⇄  H⁺(aq) + Cl⁻(aq)

We have:

m HCl = 1.46 g

V = 750 ml = 0.750 L

M HCl = 36.458 g/mol  

We know that 1 mol is equal to:

$mol = \frac{m}{M} = \frac{1.46 g}{36.458 g/mol} = 0.040 mol$

Now, we can find the concentration of HCl:

$[HCl] = \frac{mol}{V} = \frac{0.040 mol}{0.750 L} = 0.053 mol/L$

Finally, the pH of the solution is:

$pH = -log [H^{+}] = -log [0.053] = 1.27$    

Therefore, the ph of a solution that was prepared with 1.46 g of hcl to produce 750 ml of aqueous solution is 1.27.

I hope it helps you!    

Answer 2

Answer:

pH = 1.28

Explanation:

Given that,

mass = 1.46g of HCl

volume = 750 ml = 0.75 l

MW HCl = 36.5 g

                                  36.5 g of HCl -------------------  1 mol

                                   1.46 g            --------------------   x

                                   x = (1.46 x 1) / 36.5

                                   x = 0.040 mol

Molarity = 0.040 / 0.75

Molarity = 0.053

pH = -log [H+]

pH = - log [0.053]

pH = 1.28