A) what is thd pH of the solution if 0.75 mol of H2Cl is diluted to 1.00L with w

Question

A) what is thd pH of the solution if 0.75 mol of H2Cl is diluted to 1.00L with water? B) what is the pH of the solution if 0.5 mol of HL is diluted to 1.00L with water? C) what is the pH of the solution if 0.25 mol of NaL is diluted to 1.00 L with water? Please show work. I have the answers I am just confused how to get there. A) what is thd pH of the solution if 0.75 mol of H2Cl is diluted to 1.00L with water? B) what is the pH of the solution if 0.5 mol of HL is diluted to 1.00L with water? C) what is the pH of the solution if 0.25 mol of NaL is diluted to 1.00 L with water? Please show work. I have the answers I am just confused how to get there. B) what is the pH of the solution if 0.5 mol of HL is diluted to 1.00L with water? C) what is the pH of the solution if 0.25 mol of NaL is diluted to 1.00 L with water? Please show work. I have the answers I am just confused how to get there.

Explanation / Answer

pH = -log [H+]

[H+] = molar concentration of H+ ion.

molar concentration = moles of H+ / Ltr of solution.

A) 0.75 mol / 1 L = 0.75 M

your compound is HCl or H2Cl ( there can not be a compound like H2Cl)

If it is a HCl , pH = -log(0.75) => 0.12

If it is H2X , 1 M of H2X will have 2 M of H+ ( for eq H2SO4) then pH = -log ( 2 * 0.75) => -0.18

B) 0.5 mol of HI ( there is no compound as HL)

molarity = 0.5 mol / 1 Ltr = 0.5 M

pH = -log(0.5) => 0.30

C) Since NaI is neither acid nor basic , hence its solution will be neutral pH = 7

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