Mixture of 120 grams of KClO3 and 300 grams of water until all of the KClO3 has dissolved. At what temperature does this occur?
1 answer:
240°C is required to dissolve 120 grams of KClO₃ in 300 g of water.
Explanation:
As per the solubility curve graph of different salts dissolved in 100 g of water, it can be noted that the KClO₃ gets saturated at 100 °C with the solubility of 59 g in it. But here the water is taken as 300 g and the salt is taken as 120 g. The graph shows the solubility of grams of salt in 100 g of water.
So, then we have to find what is the gram of salt present in 100 g of water for the present sample.
300 g of water contains 120 grams of salt.
Then, 1 g of water will contain g of salt.
Then, 100 g of water will contain of salt. This means, 100 g of water will contain 40 g of salt in it.
Then, if we check the graph, the corresponding x-axis point on the curve for the y-axis value of 40 g will give us the temperature required to dissolve the salt in water. So 80°C will be required to dissolve 40 g of salt in 100 g of water.
Then, in order to get the temperature required to dissolve 120 g in 300 g of water, multiply the temperature by 3, which will give the result as 80×3=240 °C.
So, 240°C is required to dissolve 120 grams of KClO₃ in 300 g of water.
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<u>Answer:</u> The correct statement is if you add the soluble salt KA to a solution of HA that is at equilibrium, the pH would increase.
<u>Explanation:</u>
Common ion effect is defined as the effect which occurs on equilibrium when a common ion (an ion which is already present in the solution) is added to a solution. This effect generally decreases the solubility of a solute.
Equilibrium reaction of HA and KA follows the equation:
According to Le-Chateliers principle, if there is any change in the variables of the reaction, the equilibrium will shift in the direction in order to minimize the effect.
In the equilibrium reactions, ion is getting increased on the product side, so the equilibrium will shift in the direction to minimize this effect, which is in the direction of HA.
Thus, the addition of KA will shift the equilibrium in the left direction.
Equilibrium constant depends on the temperature of the system. It does not have any effect on any change of pH.
pH is defined as the negative logarithm of hydrogen ions present in the solution
- If the solution has high hydrogen ion concentration, then the pH will be low.
- If the solution has low hydrogen ion concentration, then the pH will be high.
As, the equilibrium is shifting in the left direction, that means concentration of ions are getting decreases. This will increase the pH of the solution.
Hence, the correct statement is if you add the soluble salt KA to a solution of HA that is at equilibrium, the pH would increase.