Explain why the solubility of KHTar in 0.100 M NaCl solution differs from that in pure water?
Explain why the solubility of KHTar in the mixed KCL - NaCl solution differs from that in the 0.100 M NaCl.
As the concentration of KCl in a solution increases, the solubility of KHTar ______________ because ___________________
Were you performing an experiment involving ionic strength?
It was a solubility lab for KHTar
I assume the answser is yes; NaCl increases the ionic strength and substances are more soluble as ionic strength increases.
What would the answer be to the second part? Explain why the solubility of KHTar in the mixed KCl- NaCl solution differs from that in 0.100 M NaCl
What is the concn of the KCl and NaCl in the mixture?
Concentration of KCl is 0.04 M and NaCl is 0.06 M
You are adding a common ion and that shifts the equilibrium to the left making it less soluble. See the link below.
http://www.digipac.ca/chemical/mtom/contents/chapter4/commonionlab.htm
To understand why the solubility of KHTar (potassium hydrogen tartrate) differs in different solutions, we need to consider the concept of solubility and how it is affected by various factors.
Solubility refers to the ability of a solute (in this case, KHTar) to dissolve in a solvent (such as water or a solution). It is typically measured as the maximum amount of solute that can dissolve in a given amount of solvent at a specific temperature.
In the case of KHTar, its solubility is influenced by several factors, including the nature of the solute and the solvent, as well as the presence of other substances in the solvent.
Now, let's consider the solubility of KHTar in a 0.100 M NaCl solution compared to pure water.
In pure water, the solubility of KHTar is relatively high. KHTar is a weak acid, and it dissociates partially in water to form its conjugate base (tartrate ion) and a hydronium ion (H3O+). The presence of water as a solvent allows for efficient ion-dipole interactions between the solute and solvent molecules, promoting the dissolution of KHTar. Therefore, KHTar has a relatively high solubility in pure water.
However, in a 0.100 M NaCl solution, the presence of salt ions (Na+ and Cl-) affects the solubility of KHTar. The addition of NaCl introduces more ions into the solution, which can interfere with the solute-solvent interactions of KHTar. In particular, the chloride ions (Cl-) can form ion-ion interactions with the tartrate ions, reducing the solubility of KHTar. This is because these ion-ion interactions compete with the ion-dipole interactions between the tartrate ions and water molecules, making it more difficult for KHTar to dissolve in the solution.
When we consider a mixed solution of KCl and NaCl, the interactions become more complex. The presence of both chloride ions (Cl-) from KCl and NaCl introduces additional potential ion-ion interactions with the tartrate ions. These interactions can further decrease the solubility of KHTar compared to the 0.100 M NaCl solution alone.
In summary, the solubility of KHTar differs between a 0.100 M NaCl solution and pure water because the presence of salt ions can disrupt the ion-dipole interactions and form ion-ion interactions with the solute, reducing its solubility. The solubility can further decrease in a mixed KCl-NaCl solution due to the added complexity of interactions with multiple types of chloride ions.