II think thihe answer is to be part of the acid to be honest
Answer : The pH of buffer is 9.06.
Explanation : Given,
Concentration of HBrO = 0.34 M
Concentration of KBrO = 0.89 M
Now we have to calculate the pH of buffer.
Using Henderson Hesselbach equation :
![pH=pK_a+\log \frac{[Salt]}{[Acid]}](https://tex.z-dn.net/?f=pH%3DpK_a%2B%5Clog%20%5Cfrac%7B%5BSalt%5D%7D%7B%5BAcid%5D%7D)
![pH=pK_a+\log \frac{[KBrO]}{[HBrO]}](https://tex.z-dn.net/?f=pH%3DpK_a%2B%5Clog%20%5Cfrac%7B%5BKBrO%5D%7D%7B%5BHBrO%5D%7D)
Now put all the given values in this expression, we get:
Therefore, the pH of buffer is 9.06.
Answer:
Their similarity is that they have the same number of protons. Their difference is that they have different number of neutrons.
Explanation:
They are isotopes of the same element.
Answer:
The Ksp for this compound is 3.24 * 10^-8
Explanation:
Step 1: Data given:
Molar solubility of MgCO3 = 1.8 * 10^-4 mol /L
Step 2: Calculate molarity
For an insoluble compound, its molar solubility tells you how many moles of the compound can be dissolved per liter of aqueous solution before reaching saturation.
In this case, it means that we can only dissolve 1.8 * 10^-4 moles in a liter of water at that temperature.
Moles Mg^2+ = 1.8 * 10^-4 moles
Moles CO3^2- = 1.8 * 10^-4 moles
Since we're working with one liter of solution, we can say the molarity:
[Mg^2+] = 1.8 * 10^-4 M
[CO3^2-] = 1.8 * 10^-4 M
Step 3: Calculate Ksp
Ksp = [Mg^2+]*[CO3^2-]
Ksp = 1.8 * 10^-4 * 1.8 * 10^-4
Ksp = 3.24 * 10^-8
The Ksp for this compound is 3.24 * 10^-8
