Advertisements
Advertisements
Question
Sugar dissolves in water because ______.
Options
sugar is nonpolar
water is polar
it forms hydrogen bonding with water
sugar and water are both polar
Advertisements
Solution
Sugar dissolves in water because it forms hydrogen bonding with water.
APPEARS IN
RELATED QUESTIONS
What is the effect of temperature on solubility of solids in water? Give examples.
The solubility of a gas in water ______.
The units of Henry’s law constant are ______.
The Henry’s law constant of a gas is 6.7 × 10–4 mol/(L bar). Its solubility when the partial pressure of the gas at 298 K is 0.65 bar is ______.
Which of the following 0.10 m aqueous solutions will have maximum ΔTf value?
The solubility of the following salts in water increases with increase in temperature, EXCEPT:
Henry's law constant for a gas CH3Br is 0.159 mol dm−3 atm−1 at 25°C the solubility of CH3Br in water at 25°C and a partial pressure of 0.164 atm ____________.
Which among the following is true for the value of Henry's law constant K?
Solubility of a gas in liquid increases with ______.
Value of Henry’s constant KH ______.
H2O2 is
Partial pressure of a solution component is directly proportional to its mole fraction. This is known as ______.
What is Henry's law?
According to the Le-Chatelier principle, adding heat to a solid \[\ce{<=>}\] liquid equilibrium will cause the ______.
The solubility (in mol L−1) of AgCl (Ksp = 1.0 × 10−10) in a 0.1 M KCl solution will be ______.
Solubility of which among the following solids in water changes slightly with temperature?
Calculate the solubility of gas in water at 1.2 atm and 25° C, if Henry’s law constant is 0.145 mol dm−3 atm−1 at 25° c.
How does entropy change in the following process? Explain.
Dissolving sugar in water
The solubility of N2 gas in water at 25° C and 1 bar is 6.85 × 10−4 mol L−1. Calculate KH (Henry’s law constant).
Depending on the states of solute and solvent there are ______ types of solutions.
Henry’s constant for CH3Br(g) is 0.159 mol dm−3 bar−1 25°C. Calculate its solubility in water at 25°C, if its partial pressure is 0.164 bar.
Calculate the concentration of dissolved gas in water at 25°C if partial pressure of gas at same temperature is 0.15 atm. [KH = 0.15 mol dm-3 atm-1]
Calculate the Henry’s law constant at 25°C if the solubility of gas in liquid is 2.1 × 10−2 mol dm−3 at 0.18 bar.
Calculate Henry’s law constant if solubility of nitrogen gas in water at 25°C is 6.85 × 10–4 mol dm–3.
[Partial pressure of nitrogen gas = 0.9 bar]
