"A sample of 21.50 g of KHT is mixed with 1.000 L of pure water. After stirring the mixture for 30 minutes, there is still solid at the bottom of the container. Calculate the mass of the remaining solid. Use the value of Ksp that you obtained in your experiment."
I have the Ksp value calculated but I would like to know how to approach this problem.
..............KHT ==> K^+ + HT^-
I.............solid.........0.........0
C............solid.........x.........x
E............solid..........x.........x
Ksp = (k^+)(HT^-)
Substitute Ksp and solve for x = solubility in mols/L.
Convert to grams/L. That is how many grams will dissolve. Subtract from 21/50 g to find what did not dissolve. Post your work if you get stuck.
Wow I did this thinking I did it wrong...
After making my table and doing the calculations I ended up with 7.93 g/L from a Ksp of 1.18e-3. Does this sound right?
I don't know. You didn't post the molar mass of KHT.
mols/L KHT = moles x molar mass = grams KHT that dissolved.
21.50-grams dissolved = grams left.
To approach this problem, you first need to understand the concept of solubility product constant (Ksp). Ksp is the equilibrium constant for a solid compound dissolving in a liquid to form an aqueous solution. It is a measure of how soluble a compound is in a particular solvent at a specific temperature.
Given that you have already calculated the value of Ksp, you can use it to determine the solubility of the compound. The solubility of a compound can be defined as the maximum amount of solute that can dissolve in a given amount of solvent at a specific temperature.
In this problem, you are given a sample of KHT (potassium hydrogen tartrate) weighing 21.50 g. You then mix it with 1.000 L of pure water and stir the mixture for 30 minutes. The fact that there is still solid at the bottom of the container indicates that not all of the KHT has dissolved.
To calculate the mass of the remaining solid, you can use the concept of molar mass and stoichiometry. Here's the step-by-step approach:
1. Determine the moles of KHT in the initial sample by dividing its mass (21.50 g) by its molar mass. The molar mass of KHT can be calculated by adding the atomic masses of its constituent elements (K, H, and C4H4O6).
2. Use the balanced chemical equation for the dissociation of KHT in water to determine the stoichiometric relationship between KHT and its dissociation products (K+ and HT-, the conjugate base of KHT).
3. Since the stoichiometric ratio is usually 1:1 for a compound and its dissociation products, the moles of K+ and HT- ions will be the same as the moles of KHT that have dissolved.
4. Multiply the moles of KHT that have dissolved by the molar mass of KHT to calculate the mass of KHT that has dissolved.
5. Finally, subtract the mass of KHT that has dissolved from the initial mass of KHT to find the mass of the remaining solid.
Remember to use the value of Ksp that you obtained in your experiment for KHT. This constant represents the solubility of KHT and can be used to calculate the amount that dissolves under a given set of conditions.