A chemist wishes to prepare a pure sample of silver bromide (agbr). first the chemist combines hydrobromic acid (hbr) and silver
2 answers:
Answer:
We have to heat the mixture at 100 °C or above to remove water to get pure sample.
Explanation:
The reaction between given HBr and AgOH will be:
Now after this reaction we are getting AgBr and water as products.
To get pure HBr we have o remove water. Water can be easily removed by heating the sample at or above its boiling point, 100°C.
The steps will be
a) Filter the precipitate of HBr.
b) Dry the sample by heating it in hot air oven at or above °C.
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Answer:
La masa de 2,23×10²³ átomos de azufre es 11,85 g
A partir de una comprensión detallada de la hipótesis de Avogadro, entendimos que 1 mol de cualquier sustancia contiene 6,02 × 10²³ átomos.
La afirmación anterior implica que:
6,02×10²³ átomos = 1 mol de azufre
Recordar :
1 mol de azufre = 32 g
Así, podemos decir que:
6,02×10²³ átomos = 32 g de azufre
Con la información anterior , podemos obtener la masa de 2,23×10²³ átomos de azufre. Esto se puede obtener de la siguiente manera:
6,02×10²³ átomos = 32 g de azufre
Por lo tanto,
2,23×10²³ átomos = *la imagen*
2,23×10²³ átomos = 11,85 g de azufre
Así, la masa de 2,23×10²³ átomos de azufre es 11,85 g
Explanation:
The mass of 2.23×10²³ sulfur atoms is 11.85 g
From a detailed understanding of Avogadro's hypothesis, we understood that 1 mole of any substance contains 6.02 × 10²³ atoms.
The above statement implies that:
6.02×10²³ atoms = 1 mole of sulfur
Remember :
1 mole of sulfur = 32 g
Thus, we can say that:
6.02×10²³ atoms = 32 g of sulfur
With the above information, we can obtain the mass of 2.23×10²³ sulfur atoms. This can be obtained as follows:
6.02×10²³ atoms = 32 g of sulfur
Therefore,
2.23×10²³ atoms =*the picture*
2.23×10²³ atoms = 11.85 g of sulfur
Thus, the mass of 2.23×10²³ sulfur atoms is 11.85 g
