1.8 g of acetic acid (CH3COOH) is dissolved in 250 mL of water tò create an acidic solution. What volume of a 0.46 M calcium hydroxide solution is required to completely neutralize the acidic solution? State your answer in mL (without units). Hint: acetic acid is a weak monoprotic acid.
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![1.8 g of acetic acid (CH3COOH) is dissolved in 250 mL of water tò create an acidic solution. What
volume of a 0.46 M calcium hydroxide solution is required to completely neutralize the acidic
solution? State your answer in mL (without units). Hint: acetic acid is a weak monoprotic acid.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F603b33a4-1e5d-4689-9696-c056bb9b577e%2Fdf725fb7-e912-47ee-a639-7a646e849dcd%2Fy2iz5re_processed.jpeg&w=3840&q=75)
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First of all, we calculate the Molarity of Acetic acid solution using Following formula -
Molarity of Acetic acid = mass×1000/Molar mass×volume of solution
Here,
Molarity of Acetic acid = ?
Mass of Acetic acid = 1.8 g
Molar mass of Acetic acid = 60.052 g/mol
Volume of solution = 250 mL
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