How many moles of solute particles are present in 1 L of 1.20 M KBr?

mols = M x L

So we have 1.20 M x 1 L = 1.20 moles KBr. There are two particles/molecule; therefore, we have 1.20 x 2 = 2.40 moles of particles.

Well, let's do some mole math! To calculate the number of moles in a solution, we multiply the concentration (in moles per liter) by the volume (in liters). So in this case, we have 1.20 moles of KBr per liter. Since we have 1 liter of solution, we can say that there are "1.2 moles of moles" in that 1 L of KBr solution. But since moles can't have moles, it's just 1.2 moles. Hope that clears things up, mole-ty fast!

To determine the number of moles of solute particles in a solution, we need to consider the number of moles of the solute. In this case, the solute is KBr, which dissociates into K+ and Br- ions in water.

The given concentration of KBr is 1.20 M, which means that there are 1.20 moles of KBr in 1 liter of the solution.

Since KBr dissociates into one K+ ion and one Br- ion, the number of moles of solute particles is the same as the number of moles of KBr.

Therefore, in 1 L of a 1.20 M KBr solution, there are 1.20 moles of solute particles.

To find the number of moles of solute particles in 1 L of 1.20 M KBr, you'll need to use the formula:

moles = concentration (M) x volume (L)

In this case, the concentration is 1.20 M and the volume is 1 L, so you can substitute those values into the formula:

moles = 1.20 M x 1 L

Now, multiply the concentration (1.20 M) by the volume (1 L) to get the number of moles:

moles = 1.20

Therefore, there are 1.20 moles of solute particles in 1 L of 1.20 M KBr.