Calculate the final temperature of a mixture of 200.0 g of ice initially at -20.50 °C and 319.0 g of water initially at 91.50 °C.

Explanation:

As the ice is in contact with the water, heat is transferred from the water to the ice; part of the heat is used to bring the ice to its melting point (), part is used to melt the ice, and the rest is used to increase the temperature of the ice (which is now melted) to the equilibrium temperature.

At the same time, the temperature of the water decreases to the equilibrium temperature.

The heat needed by the ice to reach the melting point is:

where

is the mass of the ice

is the specific heat of ice

is the final temperature

is the initial temperature

Substituting,

Then, the heat needed to melt the ice when it reached the melting point is

where

is the specific latent heat of ice

Substituting,

Now, the ice has completely melted, so it's now liquid water; the heat needed to reach the equilibrium temperature is

where

is the specific heat of water

is the equilibrium temperature

is the initial temperature of ice

At the same time, the heat released by the 319.0 g of liquid water is

where

is the mass of the water

is the initial temperature of the water

Since the total energy is conserved, we have:

Therefore, substituting and re-arranging, we find the equilibrium temperature:

answer: option (a) is the correct answer.

explanation:

the measurement of hydrogen ions in a solution is known as ph.

if ph of a solution is less than 7 then the solution is acidic. if ph of a solution is greater than 7 then the solution is basic.

when the ph of a solution equals 7, then the solution is considered as neutral.

the ph of pure water is 7, therefore, it means that concentration of hydronium ions equals that of hydroxide ions.