How many Moles of solute particles are present in 1 mL of aqueous 0.070 M (NH4)2CO3?
____ mol of Particles
To determine the number of moles of solute particles in a solution, we need to consider the dissociation of the compound. In this case, (NH4)2CO3 dissociates into three ions: 2 NH4+ ions and 1 CO3 2- ion.
First, let's find the moles of (NH4)2CO3 using its molarity and volume:
Molarity (M) = Moles of solute / Liters of solution
Given:
Molarity (M) = 0.070 M
Volume (V) = 1 mL = 0.001 L
Moles of (NH4)2CO3 = Molarity × Volume
= 0.070 M × 0.001 L
= 0.00007 moles
Now, since (NH4)2CO3 dissociates into 2 NH4+ ions and 1 CO3 2- ion, the total number of moles of particles in the solution is:
Total moles = 2 × Moles of NH4+ ions + Moles of CO3 2- ion
Total moles = 2 × 0.00007 moles + 0.00007 moles
= 0.00021 moles
Therefore, there are 0.00021 mol of particles present in 1 mL of aqueous 0.070 M (NH4)2CO3.
To determine the number of moles of solute particles in 1 mL of 0.070 M (NH4)2CO3, you first need to understand the number of moles present in one liter (1000 mL) of the solution. The concentration of the solution is given as 0.070 M, which means that there are 0.070 moles of (NH4)2CO3 in one liter.
To convert this to the number of moles present in 1 mL, you can use the following equation:
Number of moles = concentration (M) × volume (L)
Since we want the number of moles in 1 mL, we need to convert 1 mL to liters. There are 1000 mL in a liter, so 1 mL is equal to 0.001 L.
Now, we can substitute the values into the equation:
Number of moles = 0.070 M × 0.001 L
Calculating this gives:
Number of moles = 0.070 × 0.001 = 0.00007 moles
Therefore, there are 0.00007 moles of solute particles present in 1 mL of aqueous 0.070 M (NH4)2CO3 solution.
How many mols (NH4)2CO3 do you have? That's M x L = ? mols (NH4)2CO3.
For each mol (NH4)2CO3 you have 2 NH4^+ and 1 CO3^2-. The sum is the total.