Question

you want to determine the concentration when 93 ml of a 2.03 m kf solution is diluted by adding 3920 ml h₂o. what is m₁ (molarity of the concentrated solution) for this dilution? 2.03 m 93 ml the unknown

Explanation:

Step1: Identify \( M_1 \)

The problem states the concentrated solution has a molarity of \( 2.03 \, M \) (KF solution before dilution). Wait, no—wait, the question is asking for \( M_1 \), but let's check the labels. The first box is \( 2.03 \, M \), which is the molarity of the concentrated? Wait, no, dilution: \( M_1V_1 = M_2V_2 \). But the question is "What is \( M_1 \) (molarity of the concentrated solution) for this dilution?" Wait, the labels: the first option is \( 2.03 \, M \), second \( 93 \, mL \), third unknown. Wait, no—wait, the initial solution is 93 mL of 2.03 M KF, then diluted by adding 3920 mL water. But \( M_1 \) is the molarity of the concentrated (original) solution. Wait, the original solution is 2.03 M? Wait, no, maybe I misread. Wait, the question is "What is \( M_1 \) (molarity of the concentrated solution) for this dilution?" The original solution is the 93 mL of 2.03 M KF. So \( M_1 \) is the molarity of the concentrated, which is 2.03 M? Wait, the options: first box is 2.03 M, second 93 mL, third unknown. Wait, the question is asking for \( M_1 \), and the first option is 2.03 M. Wait, maybe the question is a bit confusing, but the concentrated solution's molarity is given as 2.03 M. So \( M_1 = 2.03 \, M \).

Step2: Confirm

The concentrated solution is the initial 93 mL KF solution with molarity 2.03 M. So \( M_1 \) (molarity of concentrated) is 2.03 M.

Answer:

2.03 M