Ask Question
30 March, 07:54

A student prepares 150. mL of a 2.00 M Ba (OH) 2 aqueous solution in lab. What mass of Ba (OH) 2 is fully dissolved in the solution?

+3
Answers (1)
  1. 30 March, 08:13
    0
    Answer: 51.4g

    Explanation:

    Given that:

    Amount of moles of Ba (OH) 2 (n) = ?

    Volume of Ba (OH) 2 solution (v) = 150.0mL

    [Convert 150.0mL to liters

    If 1000 mL = 1L

    150.0mL = 150.0/1000 = 0.150L]

    Concentration of Ba (OH) 2 solution (c) = 2.00M

    Since concentration (c) is obtained by dividing the amount of solute dissolved by the volume of solvent, hence

    c = n / v

    make n the subject formula

    n = c x v

    n = 2.00M x 0.150L

    n = 0.3 mole

    Now given that,

    Amount of moles of Ba (OH) 2 (n) = 0.3

    Mass of Ba (OH) 2 in grams (m) = ?

    For molar mass of Ba (OH) 2, use the molar masses:

    Barium, Ba = 137.3g;

    Oxygen, O = 16g;

    Hydrogen, H = 1g

    Ba (OH) 2 = 137.3g + [ (16g + 1g) x 2]

    = 137.3g + [17g x 2]

    = 137.3g + 34g

    = 171.3 g/mol

    Since, amount of moles = mass in grams / molar mass

    0.3 mole = m / 171.3g/mol

    m = 0.3 mole x 171.3g/mol

    m = 51.39g

    [Round the 51.39g to the nearest tenth, so it becomes 51.4g]

    Thus, the mass of Ba (OH) 2 fully dissolved in the solution is 51.4 grams
Know the Answer?
Not Sure About the Answer?
Get an answer to your question ✅ “A student prepares 150. mL of a 2.00 M Ba (OH) 2 aqueous solution in lab. What mass of Ba (OH) 2 is fully dissolved in the solution? ...” in 📙 Chemistry if there is no answer or all answers are wrong, use a search bar and try to find the answer among similar questions.
Search for Other Answers