A 0.870 g sample of a monoprotic acid is dissolved in water and titrated with 0.300 M KOH.
What is the molar mass of the acid if 23.0 mL of the KOH solution is required to neutralize the sample?
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Ответ:
The molar mass of monoprotic acid is 126.1 g/mol
Explanation:
To calculate the molarity of solution, we use the equation:
Molarity of KOH solution = 0.300 M
Volume of solution = 23.00 mL
Putting values in above equation, we get:
The chemical equation for the reaction of monoprotic acid and KOH follows:
By Stoichiometry of the reaction:
1 mole of KOH reacts with 1 mole of HA
So, 0.0069 moles of KOH will react with =
moles of HA
To calculate the molar mass for given number of moles, we use the equation:
Given mass of HA = 0.870 g
Moles of monoprotic acid = 0.0069 mol
Putting values in above equation, we get:
Hence, the molar mass of monoprotic acid is 126.1 g/mol
Ответ:
b. A data table
Step-by-step explanation:
We say that it is not a scientific model because we don't know what the table shows and because the table contains information. This information hasn't been turned into something visual, that we can call a model.