Assuming 100% dissociation, calculate the freezing point and boiling point of 2.59 m k3po4(aq).

Explanation:

Hello,

In this case, it firstly necessary to understand how the complete (100%) dissociation of the potassium phosphate is done:

In such a way, since the freezing point depression and the boiling point elevation are computed as:

The corresponding van't Hoff factor is four as 3 potassiums and 1 phosphate as ions are obtained during the dissolution. In addition, the freezing point depression constant and boiling point elevation constant of water are 1.86 and 0.512 °C/m respectively. Moreover, the freezing point of water is 0 °C and the boiling point is 100 °C, therefore, the resulting freezing and boiling temperatures for the 2.59 m solution of potassium phosphate are:

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what is the volume occupied by 40 grams of argon gas (ar) at standard conditions? what volume, in liters, is occupied by 1.5 x 1023 

nacl or sodium chloride is an ionic compound. this is because an ionic compound pertains to a compound that consists of positively and negatively charged ions. in this case, na (sodium) has a tendency to lose one electron when it reacts with with other atoms, so the resulting sodium ion contains 11 protons and 10 electrons, thus making it positively charged (na+), when chlorine reacts, it usually gains one electron to form an ion called chloride, thus making it negatively charged ( since the ions are oppositely charged, they attract.