Beaker a contains 100 ml of 1.5 mammonia. beaker b contains 100 ml of 0.50m ammonia. how does the solution in beaker a compare to the solution in beaker b?

In beaker A and B, the similarity was their containment of 100 mL, but the difference is that Beaker A had 1.5M ammonia whereas Beaker B had 0.5M ammonia. M in chemistry stands for mole, which is the unit for concentration of solutions. Thus, this can be determined as a solutions problem.

This is a chemical equation: Molarity = moles / volume (L)

Thus for beaker A,
Molarity = 1.5 M ammonia, and volume = 100 mL

1. Convert 100 mL into L
100mL = 0.1 L (use dimensional analysis)

2. Substitute known values into the equation for Molarity.
(1.5 M) = moles / (0.1 L)
Now you have to solve for moles, which through calculation, you would find that it is 0.15 moles of ammonia.

Do the same for Beaker B. We know that it has a Molarity of 0.5 M and a volume of 100 mL.

1. Convert 100 mL into L
100mL = 0.1 L (use dimensional analysis)

2. Substitute known values into the equation for Molarity.
(0.5 M) = moles / (0.1 L)
Through calculation you’d find that there are 0.05 moles of ammonia.

Thus you can conclude that in Beaker B, there are less moles of ammonia than in Beaker A. Also you could conclude that the solution of ammonia in Beaker B was less concentrated than the ammonia in Beaker A, because 1.5 M > 0.5 M.

Hope this helped!

Source: Taking AP Chemistry at the moment.

We first assume that this gas is an ideal gas where it follows the ideal gas equation. the said equation is expressed as: pv = nrt. from this equation, we can predict the changes in the pressure, volume and temperature. if the volume and the temperature of this gas is doubled, then the pressure still stays the same.

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