Gases in Liquids

Q. Why an aquatic animals are more comfortable in cold water in comparison to the hot water

Q.

A solution is obtained by mixing 300 g of 25% solution and 400 g of 40% solution by mass. Calculate the mass percentage of the resulting solution.

Q.

Why is helium used in diving apparatus?

Q.

Why are aquatic species more comfortable in cold water in comparison to warm water?

Q. For dissolution of $C{O}_2\left(g\right)$ in $H_{2}O\left(l\right)$
Which of the following statement is correct?

1. Increase in temperature of the solution will decrease solubility of $C{O}_2$
2. Increase in temperature of the solution will increase solubility of $C{O}_2$
3. Increase in temperature of the solution will will have no effect on solubility of $C{O}_2$
4. On increasing temperature of the solution , solubility of $C{O}_2$ first increases and then stays constant

Q.

Why does ethanol evaporate faster than water?

Q.

State Henrys Law. What is the significance of Henrys Law Constant K_H ?.

Q. For the dissolution of gas in solvent at a given temperature, increase in pressure of gas will result in:

1. Increase in solubility
2. decrease in solubility
3. no change in solubility
4. cannot be predicted

Q.

Given that $\Delta H$ = 0 for mixing of two gases. Explain whether the diffusion of these gases into each other in a dosed container is a spontaneous process or not?

Q.

Explain the effect of temperature and pressure on the solubility of gases in water.

Q. Select the correct order of solubility for the following gases in aqueous solution:

1. $HCl>N{H}_3>O_2$
2. $HCl>O_2>N{H}_3$
3. $O_2>HCl>N{H}_3$
4. $N{H}_3>HCl>O_2$

Q. Why do aquatic animals prefer to stay at lower level of water during Summer ?

Q.

What happens when the temperature of the solution is increased?

Q.

What Is formed when Carbon Monoxide binds to the Haemoglobin Molecule?

Q.

In higher altitudes the temperature is very low so conceptually the solubility should be high, but it is not so why in this example only pressure is taken into consideration? why not temperature?

Q.

State importance of dissolved gases in natural water.

Q. How many moles of carbon dioxide gas is dissolved in a 1 L bottle of carbonated water if the manufacturer uses a pressure of 2.4 atm in the bottling process at ${25}^{\circ }C$?
Given: $K_H$ of $C{O}_2$ in water = 29.76 atm/(mol/L) at ${25}^{\circ }C$

1. 0.02
2. 0.06
3. 0.04
4. 0.08

Q. Write the solubility product expression for a sparingly soluble salt BaSO4
what is the formula for it

Q.

Solubility of a gas in a liquid increases on:

1. Increasing Pressure

2. Increasing Temperature

3. Decreasing Pressure

4. Increasing Both Pressure And Temperature

Q. Given the concentration of neon as $C_{Ne}=23.5mL/(L\text{of water)}$ at STP. Then calculate the Henry's constant at STP for neon dissolved in water. Given STP molar volume is $22414mL/mol$ and pressure is $1atm$.

1. $1.048\times {10}^{-3}mol{L}^{-1}at{m}^{-1}$
2. $3.557\times {10}^{-2}mol{L}^{-1}at{m}^{-1}$
3. $5.55\times {10}^{-4}mol{L}^{-1}at{m}^{-1}$
4. $0.114\times {10}^{-4}mol{L}^{-1}at{m}^{-1}$

Q. The use of common salts, e.g., NaCl or $CaC{l}_2$ anhydrous, is made to clear snow on the rods. This causes:

1. A lowering in the freezing point of water
2. All of these
3. A lowering in the melting point of ice
4. Ice melts at the temperature of atmosphere present at that time

Q.

Category of compound which liberates ammonia from ammonium salts are:

1. Acids

2. Alkalis

3. Acidic gases

4. Salt solutions

Q.

Marine life prefer to be at the lower level during summer

Q. The oxygen dissolved in water exerts a partial pressure of 20 kPa in the vapour above water . The molar solubility of oxygen in water is $x\times {10}^{-5}mold{m}^{-3}$. The value of x
(Round off to the Nearest Integer ) is
$[Given:\text{Henry's law constant}(K_H)=8.0\times {10}^{4}kPa\text{for}{O}_2\text{Density of water with dissolved oxygen}=1.0Kgd{m}^{-3}]$

Q. Generally solubility of gases in liquids is decreases as increasing temperature. Give reason.

Q. In a nearly saturated solution, the solutility increases with increase in temperature, then change in enthalpy of solution is

1. +ve
2. O
3. +ve or –ve
4. -ve

Q. The second law of thermodynamics states that

1. all spontaneous processes are thermodynamically irreversible.
2. entropy of the universe is continuously increasing.
3. energy of the universe remain constant.
4. energy can neither be created nor destroyed.

Q.

i)How soluble is ammonia in water?
ii)Give two reasons to show that the solution of ammonia in water contains hydroxide ions.
iii)Name a simple method you would employ to prepare ammonium salts in your laboratory.

Q. For the dissolution of gas in solvent at a given temperature, increase in pressure of gas will result in:

Q.

Is carboxyhemoglobin dangerous?