Free NEET Chemistry multiple-choice questions on Solubility & Henry's Law. Attempt each question and reveal the answer with a full explanation.
At a constant temperature, if the Henry's law constant ( K H ) for a gas increases, the solubility of the gas in the liquid: Decreases Increases Remains constant First increases then decreases At high altitudes, the partial pressure of oxygen is less than that at the ground level. This leads to low concentrations of oxygen in the blood and tissues of people living at high altitudes or climbers, causing them to feel weak and unable to think clearly. This condition is known as: Anoxia Bends Acidosis Alkalosis The solubility of a gas in a liquid is directly proportional to the pressure of the gas. This is known as: Henry's law Raoult's law Dalton's law Gay-Lussac's law If the partial pressure of a gas ( P gas ) is plotted against its mole fraction in solution ( X gas ), the slope of the resulting linear graph represents: Henry's law constant ( K H ) Vapour pressure of the pure gas Molal elevation constant The gas constant ( R ) Based on Henry's Law, the solubility of a gas in a liquid at a constant temperature is directly proportional to its partial pressure. Which graph correctly depicts this? A straight line passing through the origin A rectangular hyperbola A horizontal line An exponential curve At a given temperature, if the mole fraction of a gas in a solution is doubled, the partial pressure of the gas over the solution will: Double Remain the same Be halved Increase by four times Maximum solubility of a gas in a liquid at a fixed temperature is achieved by . Increasing pressure Decreasing pressure Increasing volume of liquid Increasing temperature If the solubility of nitrogen gas in water at 0 C is 0.02 g/L at 1 atm , what is its solubility at 3 atm at the same temperature? 0.06 g/L 0.02 g/L 0.01 g/L 0.10 g/L Which gas is used in the tanks of scuba divers to reduce the risk of 'bends'? Helium Argon Neon Hydrogen Which of the following describes the effect of increasing temperature on the solubility of most gases in liquids? Solubility decreases because the process is exothermic Solubility increases because the process is endothermic Solubility decreases because the process is endothermic Solubility remains unchanged The Henry’s law constant ( K H ) values of three gases (A, B, C) in water are 145, 2 10 -5 and 35 kbar, respectively. The solubility of these gases in water follow the order: B > A > C B > C > A A > C > B A > B > C The safe limit of fluoride ions in drinking water to prevent mottled teeth but protect against tooth decay is approximately: 1.0 ppm 1.5 ppm 10 ppm 100 ppm The value of Henry's law constant K H is . Greater for gases with lower solubility Greater for gases with higher solubility Constant for all gases Not related to the solubility of gases Which gas has the lowest solubility in water at a given temperature and pressure, given their K H values: Ar = 40.3 , CO 2 = 1.67 , CH 4 = 0.413 , Vinyl chloride = 0.611 (in kbar)? Ar CO2 CH4 Vinyl chloride The partial pressure of ethane over a solution containing 6.56 10 -3 g of ethane is 1 bar . If the solution contains 5.00 10 -2 g of ethane, then what shall be the partial pressure of the gas? 7.62 bar 0.13 bar 5.00 bar 1.00 bar The value of Henry's Law constant K H is: Greater for gases with lower solubility Greater for gases with higher solubility Constant for all gases Independent of temperature Henry's law is a special case of Raoult's law when: The solute is a gas and its mole fraction approaches zero The solute is non-volatile The solution is ideal and K H = P o The temperature is at absolute zero The solubility of Na 2SO 4 10H 2O (Glauber's salt) shows a unique behavior with temperature. It increases up to a certain point and then decreases. What is this temperature called? Transition temperature Critical temperature Eutectic temperature Inversion temperature The value of Henry's law constant K H for O 2 in water increases with: Increase in temperature Decrease in temperature Increase in pressure Decrease in pressure Which gas among O 2, N 2, He, H 2 will have the highest Henry's law constant K H at a specific temperature? He O 2 N 2 H 2 The Henry's law constant for the solubility of N 2 gas in water at 298 ,K is 1.0 10 5 ,atm . The mole fraction of N 2 in air is 0.8 . The number of moles of N 2 from air dissolved in 10 ,moles of water at 298 ,K and 5 ,atm pressure is: 4.0 10 -4 4.0 10 -5 5.0 10 -4 4.0 10 -6 Which gas is most likely to deviate from Henry's Law at room temperature when dissolved in water? NH 3 N 2 O 2 He Which gas has the highest solubility in water at a given temperature? Ammonia Nitrogen Helium Oxygen The value of Henry's law constant K H for argon, methane, CO 2 and formaldehyde are 40.39, 0.413, 1.67 and 1.83 10 -5 respectively. The correct order of their solubility is: Formaldehyde > Methane > CO 2 > Argon Argon > CO 2 > Methane > Formaldehyde Methane > Formaldehyde > Argon > CO 2 Formaldehyde > Argon > Methane > CO 2 Which gas will have the highest solubility in water at 298 ,K if the Henry's Law constants ( K H ) are as follows: He = 144.97 ,kbar , H 2 = 69.16 ,kbar , N 2 = 76.48 ,kbar , O 2 = 34.86 ,kbar ? O 2 He H 2 N 2 The solubility of Na 2SO 4 in water decreases with an increase in temperature above 32.4 C . This indicates that the dissolution process in this temperature range is: Exothermic Endothermic Athermal Impossible Aquatic species are more comfortable in cold water than in warm water because: Solubility of oxygen is higher at low temperatures Solubility of oxygen is higher at high temperatures Viscosity of water is low at low temperatures Density of water is high at low temperatures The Henry's law constant for O 2 in water at 293 K is 34.86 kbar . If the partial pressure of O 2 is 0.2 bar , the solubility of O 2 in water (as mole fraction) is: 5.74 x 10 -6 1.74 x 10 -4 5.74 x 10 -4 3.48 x 10 -5 According to Henry's Law, the solubility of a gas in a liquid depends on the nature of the gas. The correct sequence of solubility for He, N 2, O 2 in water at a constant temperature is: O2 > N2 > He He > N2 > O2 N2 > O2 > He He > O2 > N2 If the solubility of a gas is 'S' at pressure 'P', then which of the following represents the correct Henry's Law graph? A straight line passing through the origin in a plot of S vs P A rectangular hyperbola in a plot of S vs P A horizontal line in a plot of S vs P A parabola in a plot of S vs P If the Henry's law constant for a gas is expressed in units of mol L -1 bar -1 , the constant represents: Solubility of the gas at unit partial pressure Partial pressure of the gas at unit concentration Mole fraction of the gas in the liquid The vapor pressure of the pure gas Which gas deviates most from Henry's Law when dissolved in water at room temperature? NH 3 N 2 H 2 He If the partial pressure of CO 2 over water is increased from 1 atm to 2 atm at 25 C , the Henry's law constant K H will: Remain unchanged Double Be halved Increase slightly The phenomenon of 'Anoxia' experienced by mountain climbers is due to: Low partial pressure of oxygen at high altitudes Low temperature at high altitudes High partial pressure of oxygen at high altitudes Increased solubility of nitrogen in blood The solubility of most solid solutes in water increases with a rise in temperature. If the dissolution process is exothermic ( H sol < 0 ), the solubility will: Decrease with increase in temperature Increase with increase in temperature Remain unchanged First increase and then decrease If a gas is bubbled through water at 298 ,K and 1 ,atm pressure, and the gas reacts chemically with water (like NH 3 or HCl ), Henry's law: Does not strictly apply Applies perfectly Predicts higher solubility than observed Is used to calculate the equilibrium constant The unit of the Henry's law constant K H in the equation P = K H C (where C is molarity) is: L atm mol -1 atm mol L -1 atm -1 Dimensionless In which of the following the hydration energy is higher than the lattice energy? MgSO 4 RaSO 4 SrSO 4 BaSO 4 HCl was passed through a solution of CaCl2 , MgCl2 and NaCl. Which of the following compound(s) crystallise(s)? Only NaCl Only MgCl2 NaCl, MgCl2 and CaCl2 Both MgCl2 and CaCl2 If the solubility of N 2 gas in water at 293 K is 0.02 g/L , what is the Henry's law constant K H if the partial pressure of N 2 is 1 atm ? (Assume density of water is 1 g/mL ) 7.84 x 10 4 atm 7.84 x 10 2 atm 1.25 x 10 5 atm 3.5 x 10 3 atm Henry's law constant for the solubility of N 2 gas in water at 298 K is 1.0 10 5 atm . The mole fraction of N 2 in air is 0.8 . The number of moles of N 2 from air dissolved in 10 moles of water at 298 K and 5 atm pressure is: 4.0 10 -4 4.0 10 -5 5.0 10 -4 4.0 10 -6 The Henry's law constant ( K H ) for O 2 in water at 293 ,K is 34.86 ,kbar . If the partial pressure of O 2 is 0.2 ,atm , what is the mole fraction of O 2 in water? ( 1 ,atm = 1.013 ,bar ) 5.81 10 -6 5.81 10 -5 3.42 10 -4 1.23 10 -5 The value of Henry's law constant K H for CO 2 gas at 298 ,K is 1.67 ,kbar . If the gas is bubbled through water at 298 ,K , how many millimoles of CO 2 gas would dissolve in 1 ,L of water? (Partial pressure of CO 2 = 0.835 ,bar ) 27.7 2.77 0.277 277 Which gas is used by scuba divers to dilute oxygen to avoid the toxic effects of high concentration of nitrogen in the blood? Helium Argon Neon Hydrogen What happens to the solubility of a gas in a liquid as the temperature is increased? It decreases It increases It remains constant It first increases then decreases The solubility of CO 2 in soft drinks is increased by sealing the bottle under high pressure. This is an application of: Henry's Law Raoult's Law Dalton's Law Charles's Law The solubility of a gas in a liquid increases with: Increasing pressure and decreasing temperature Increasing pressure and increasing temperature Decreasing pressure and decreasing temperature Decreasing pressure and increasing temperature The solubility of N 2 in water at 300 ,K and 500 ,torr partial pressure is 0.01 ,g ,L -1 . The solubility (in g ,L -1 ) at 750 ,torr partial pressure is: 0.015 0.020 0.0075 0.0125