Answer :
The correct option is A, The correct answer is Beakers 2 and 3.
In Beaker 1, we have HCl, which is a strong acid, and [tex]NH_3[/tex], which is a weak base. Therefore, this solution will not form a buffer.
In Beaker 2, we have HCl again, but at a lower concentration, and [tex]NH_3[/tex]. [tex]NH_3[/tex]can act as a weak base and form its conjugate acid, [tex]NH_4[/tex]+. Therefore, this solution contains a weak acid ([tex]NH_4[/tex]+) and its conjugate base ([tex]NH_3[/tex]), and can act as a buffer.
In Beaker 3, we have [tex]NH_4Cl[/tex], which can dissociate to form [tex]NH_4[/tex]+ (a weak acid) and Cl- (a spectator ion). [tex]NH_3[/tex]is also present in the solution.
Concentration refers to the amount of solute (substance being dissolved) present in a given amount of solvent (substance doing the dissolving). It is usually expressed as a ratio or a percentage. Changes in concentration can affect the rate of a reaction, the solubility of a substance, and properties such as density, viscosity, and boiling and freezing points.
There are different ways to express concentration, such as molarity, molality, mass percent, volume percent, and parts per million. Molarity is the most common unit of concentration and is defined as the number of moles of solute per liter of solution. Molality, on the other hand, is the number of moles of solute per kilogram of solvent. Concentration plays a crucial role in chemical reactions and physical properties of solutions.
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Only Beakers 2 and 3 will contain a buffered solution after the addition of NH₃, because Beaker 2 will have equal amounts of NH₃ and HCl forming NH₄⁺, and Beaker 3 already contains NH₄Cl, which is NH₃'s conjugate acid.
The student's question asks which beaker(s) will contain a buffered solution after the addition of NH₃ to various solutions. A buffered solution can be created when a weak acid is mixed with its conjugate base, or a weak base is mixed with its conjugate acid. In the context of NH₃ (a weak base), the presence of its conjugate acid NH₄⁺ would create a buffer.
For Beaker 1: When 50 mL of 1.00 M NH₃ is mixed with 50 mL of 2.00 M HCl, it results in an excess of HCl, completely neutralizing the NH₃, leaving no weak base, hence no buffer.
For Beaker 2: Here, 50 mL of 1.00 M NH₃ reacts with 50 mL of 0.50 M HCl. Since the molar amounts of NH₃ and HCl are equal, all of NH₃ will be converted to NH₄⁺, forming a buffer.
For Beaker 3: The solution already contains NH₄Cl, the conjugate acid of NH₃, so adding NH₃ will create a buffered solution without the need for a reaction to occur.
Therefore, the beakers that will contain a buffered solution once the mixing is complete are Beakers 2 and 3.
