I think the best statement to fill the blank is that "can be desalinized and used for drinking". The said statement seems the most appropriate one because the pH of saltwater is not 10 but approximately between 7.6 to 8.4. Also, saltwater is not found in glaciers, ice caps and aquifers instead it is freshwater.
The molar mass of X would be 63.55 g/mol and the chemical symbol of X would be Cu (copper).
From the equation of the reaction: F2+2XBr⟶Br2+2XF
The mole ratio of XBr to Br2 is 2:1
Mole of Br2 = mass/molar mass
= 0.7241/159.808
= 0.004531 mole
Mole of XBr = 2 x mole of Br2
= 2 x 0.004531
= 0.009062 mole
Molar mass of XBr = mass/mole
= 1.300/0.009062
= 143.456 g/mol
Since the molar mass of Br is 79.904, the molar of X would be:
143.456 - 79.904
= 63.55 g/mol
Hence, X would be Cu.
More on molar mass calculation can be found here: brainly.com/question/20691135
Chemical reactions can be detected by changes in temperature
Rf value is the ratio of the distance traveled by the solute to that of the solvent front on the paper used in chromatographic separation.
From the image it is clear the distance traveled by solvent front = 7.3 cm
Distance traveled by the component -1 of the mixture = 1.4 cm
Distance traveled by the component -2 of the mixture = 3.0 cm
Distance traveled by the component -3 of the mixture = 4.5 cm
Distance traveled by the component -4 of the mixture = 6.5 cm
Rf value of component-1 = 
Rf value of component-2 = 
Rf value of component-3 = 
Rf value of component-4 = 
b) Samples can be separated from a mixture using chromatography as the relative affinities for the compounds towards the paper (stationary phase) and the solvent(mobile phase) are different. Each component spends different amounts of time on the stationary phase depending on it chemical nature. So, the components in a mixture can be separated based on their polarities and relative degrees of adsorption on the stationary phase.
Answer:
0,051g of O₂
Explanation:
The reaction of precipitation of Fe is:
4Fe(OH)⁺(aq) + 4OH⁻(aq) + O₂(g) + 2H₂O(l) → 4Fe(OH)₃(s)
<em>-Where the Fe(OH)⁺ is Fe(II) and Fe(OH)₃ is Fe(III)-</em>
This reaction is showing you need 1 mol of O₂(g) per 4 moles of Fe(II) for a complete reaction.
85mL= 0,085L of 0,075M Fe(II) are:
0,085L*0,075M = 6,34x10⁻³ moles of Fe(II)
For a complete reaction of 6,34x10⁻³ moles of Fe(II) you need:
6,34x10⁻³ moles of Fe(II)×
=
1.59x10⁻³ moles of O₂. In grams:
1.59x10⁻³ moles of O₂×
= <em>0,051g of O₂</em>
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I hope it helps!