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

pH = 1.28

Step-by-step 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

Answer 2

pH = 1.27

Step-by-step 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 = (m)/(M) = (1.46 g)/(36.458 g/mol) = 0.040 mol`

Now, we can find the concentration of HCl:

`[HCl] = (mol)/(V) = (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!