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Klio2033 [76]
3 years ago
11

A 0.623 g sample of a monoprotic acid is dissolved in water and titrated with 0.260 M KOH.

Chemistry
1 answer:
Sever21 [200]3 years ago
8 0

Answer:

126. g/mol is the molar mass of the acid .

Explanation:

HA+KOH\rightarrow KA+H_2O

Moles of KOH = n

Volume of the solution of KOH = 19.0 mL = 0.019 L

Molarity of the KOH solution = 0.260 M

Molarity=\frac{Moles}{Volume(L)}

0.260M=\frac{n}{0.019 L}

n=0.260 M\times 0.019 L=0.00494 mol

Accrding to recation, 1 mol KOH react with 1 mole of HA ,then 0.00494 mol of KOH will react with :

\frac{1}{1}\times 0.00494 mol=0.00494 mol of HA

Mass of HA = 0.623 g

Molar mass of HA = M

0.00494 mol=\frac{0.623 g}{M}

[tex[M=\frac{0.623 g}{0.00494 mol}=126. g/mol[/tex]

126. g/mol is the molar mass of the acid .

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