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05.07.2019 •
Chemistry
An 8.65 g sample of an unknown group 2a metal hydroxide is dissolved in 85.0 ml of water and titrated with 2.50 m hcl(aq). if it takes 56.9 ml of the acid to reach the end point of the titration (a) what is the molar mass of the metal hydroxide? (b) which of the following is in the metal hydroxide: ca2+, sr2+, ba2+?
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Ответ:
(a)The molar mass of the metal is 121.66 g/mol.
(b) The metal hydroxide is
.
Explanation:
The equation for the reaction is as follows.
(a) When 56.9 mL of the acid is required to reach end point of titration. Then,
Moles of acid =![Molarity \times Volume](/tpl/images/0053/8078/72ce4.png)
=![2.50 M \times \frac{56.9}{1000 L}](/tpl/images/0053/8078/3a3f7.png)
= 0.14225 moles
Hence, the number of moles of hydroxide = 1 - 0.14225 = 0.0711 moles
It is given that mass of sample is 8.65 g, then calculate the molar mass of the sample as follows.
=![\frac{8.65 g}{0.0711 mole}](/tpl/images/0053/8078/4fafe.png)
= 121.66 g/mol
The molar mass of the metal is 121.66 g/mol.
(b) The molar mass calculated is 121.66 g/mol. Therefore, calculate the molar mass of each given metal hydroxide as follows.
Thus, it can be concluded that the metal in the metal hydroxide is
.
Ответ:
Hope this helps