A chemist dissolves 0.9g of an unknown monoprotic (one acidic H) acid in water. The chemist finds that 14.6mL of 0.426M NaOH are required to neutralize the acid.
How many grams of acid are present?
There are 0.9g present.
How many moles of base are required to reach the equivalence point?
mol=(M)(L)
mol=(0.426mol/L)(0.0146L)
mol=0.006219mol
Therefore, 6.219 x 10-3 mol of NaOH are required.
How many moles of acid are present initially?
mol Acid = mol Base = 0.006219mol
Therefore, 6.219 x 10-3 mol of acid were present before the titration.
What is the molar mass of the acid?
m.m.= g/mol
m.m.= (0.9g)/(0.006219mol)
m.m.= 144.72g/mol
What is the chemical formula and name of this acid?
The formula is HBrO4, and the name is perbromic acid.
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