You have 3.00 L of a 3.12 M solution of NaCl(aq) called solution A. You also have 2.00 L of a 2.00 M solution of AgNO3(aq) called solution B. You mix these solutions together, making solution C.
Calculate the concentration (in M) of Ag+ ions in solution C.

In this case, since the presence of silver ions is in AgNO3 only, we can compute their moles by using the volume and concentration of the corresponding salt:

[tex]n_{Ag^+}=2.00L*2.00\frac{mol}{L}=4molAg^+[/tex]

Next, since the total volume of solution C is 5.00 L, the required concentration of silver ions turn out:

[tex]M=\frac{4.00mol}{5L} =0.8M[/tex]

Best regards!

Answer Link

You have 3.00 L of a 3.12 M solution of NaCl(aq) called solution A. You also have 2.00 L of a 2.00 M solution of AgNO3(aq) called solution B. You mix these solutions together, making solution C. Calculate the concentration (in M) of Ag+ ions in solution C.

Respuesta :

Otras preguntas

You have 3.00 L of a 3.12 M solution of NaCl(aq) called solution A. You also have 2.00 L of a 2.00 M solution of AgNO3(aq) called solution B. You mix these solutions together, making solution C.
Calculate the concentration (in M) of Ag+ ions in solution C.