Respuesta :
Answer:
The pH of the solution is 2.06
Explanation:
Step 1: Data given
Mass of hydrobromic acid (HBr) = 156 mg = 0.156 grams
Molar mass HBr = 80.91 g/mol
Volume of the solution = 220 mL = 0.220 L
Step 2: Calculate moles HBr
Moles HBr = mass HBr / molar mass HBr
Moles HBr = 0.156 grams / 80.91 g/mol
Moles HBr = 0.00193 moles
Step 3: Calculate moles H+
For 1 mol HBr we have 1 mol H+
For 0.00193 moles HBr we have 0.00193 moles H+
Step 4: Calculatemolarity of H+
Molarity H+ = moles H+ / volume
Molarity H+ = 0.00193 moles / 0.220 L
Molarity H+ = 0.00877 M
Step 5: Calculate the pH
pH = -log[H+]
pH = -log (0.00877)
pH = 2.06
The pH of the solution is 2.06
Answer: 2.06
Explanation:
m=156mg=0.156g
Volume=220mL=0.22L
Molar mass =80.91g/mol
Mole= reacting mass /molar mass
Mole of HBr=0.156/80.91
Mole of HBr=0.00193moles
Since H+Br-
Therefore, one mole of H+ will give 1*0.00193
H+=0.00193moles
The molarity of H+ in 0.22L= 0.00193/0.22
Molarity of H+= 0.00876mol/L
Since PH= -log(H+)
PH= -log(0.00876)
PH=2.06
