A chemist dissolves 156. mg of pure hydrobromic acid in enough water to make up 220. mL of solution.

Calculate the pH of the solution.

Be sure your answer has the correct number of significant digits.

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