The phenomenon known as "salting-out" occurs at very high ionic strengths, when protein solubility declines as ionic strength rises. As a result, salting out may be used to segregate proteins according to how soluble they are in salt solutions.
Because large levels of sodium chloride disturb the bonds and structure of the active site, the rate of enzyme activity will gradually decrease as the concentration of sodium chloride rises. As a result, some of the active sites get denaturized and the starch loses its ability to attach to them. As more enzymes get denatured and eventually cease to function, enzyme activity will steadily wane.
Let the hydrated compound be CaSO4.xH2O
mass of the caso4= 43.63g /(40+32+64+18x)* (40+32+64)= 36.45g
136+18x=( 43.63*136) / 36.45= 162.78
18x = 162.78- 136= 26.8
x = 1.48 = 1.5
Formula of hydrate = CaSO4.1.5H2O = 2CaSo4. 3H2O
Answer:
Land fill
Explanation:
A landfill is a carefully managed waste disposal site. It is the oldest method of waste disposal. In a dumpsite, biodegradable materials decay overtime.
However, non-biodegradable materials such as plastics and other polymers tend to last many years in landfills. This category of wastes pose a great threat to the environment.
Answer is: 100 mL of <span>sodium hydroxide.
Chemical reaction: 3NaOH + H</span>₃PO₄ → Na₃PO₄ + 3H₂O.
V(H₃PO₄) = 20.0 mL ÷ 1000 mL/L = 0.02 L.
n(H₃PO₄) = V(H₃PO₄) · c(H₃PO₄).
n(H₃PO₄) = 0.02 L · 2.5 mol/L.
n(H₃PO₄) = 0.05 mol.
From chemical reaction: n(H₃PO₄) : n(NaOH) = 1 : 3.
n(NaOH) = 0.15 mol.
V(NaOH) = n(NaOH) ÷ c(NaOH).
V(NaOH) = 0.15 mol ÷ 1.5 mol/L.
V(NaOH) = 0.1 L · 1000 mL/L = 100 mL.
Explanation:
The mechanisms by which amorphous intermediates transform into crystalline materials are poorly understood. Currently, attracting enormous interest is the crystallization of amorphous calcium carbonate, a key intermediary in synthetic, biological, and environmental systems. Here we attempt to unify many contrasting and contradictory studies by investigating this process in detail. We show that amorphous calcium carbonate can dehydrate before crystallizing, both in solution and in air, while thermal analyses and solid-state nuclear magnetic resonance measurements reveal that its water is present in distinct environments. Loss of the final water fraction—comprising less than 15% of the total—then triggers crystallization. The high activation energy of this step suggests that it occurs by partial dissolution/recrystallization, mediated by surface water, and the majority of the particle then crystallizes by a solid-state transformation. Such mechanisms are likely to be widespread in solid-state reactions and their characterization will facilitate greater control over these processes.