The answer is (2) KNO3. This depends on the solubility of these four compounds at 10℃. For NaCl, it is 35.8 g, For NaNO3, 80.8 g. KCl, 31.2 g. KNO3, 21.9g. So only KNO3 is less than 25.0 g.
        
             
        
        
        
The grams of aluminium extracted from 5000g of alumina is 2647 grams
<h3>Chemical formula of alumina:</h3>
Let's calculate the molecular mass of Al₂O₃
Al₂O₃ = 27 × 2 + 16 × 3 = 54 + 48 = 102 g/mol
Therefore,
102 g of Al₂O₃ = 54 g of aluminium  
5000g of Al₂O₃  = ?
mass of aluminium produced = 5000 × 54 / 102 
mass of aluminium produced = 270000 / 102
mass of aluminium produced  = 2647.05882353
mass of aluminium produced  = 2647 grams
learn more on mass here: brainly.com/question/14627327
 
        
             
        
        
        
Answer:
10.85 g of water
Explanation:
First we write the balanced chemical equation

Then we calculate the number of moles of nitric acid produced
n(HNO3) = 
According to the balanced equation, water needed in moles is always half the number of moles of HNO3 produced. So since we will produce 1.2044 mol of HNO3, we will need 0.6022 mol of water. Now to calculate what mass that is:
mass(water)=number of moles*molar mass=0.6022mol*18.02g/mol=10.85g
 
        
             
        
        
        
The molecular weight of the substance.
        
             
        
        
        
Answer:
HClO (l)  →  H⁺ (aq)    +       ClO⁻ (aq)
                  proton   and    hypochlorite.
Explanation:
HClO (Hypochlorous acid)
This is a weak acid that can be dissociated as this:
HClO (l)  →  H⁺ (aq)    +       ClO⁻ (aq)
                  proton   and    hypochlorite.
It is a weak acid, so it can adopt a Ka for its equilibrium
HClO +  H₂O  ⇄   H₃O⁺   +  ClO⁻          Ka
Molar mass = 52.46 g/m