Skip to main content
Pearson+ LogoPearson+ Logo
Ch.17 - Aqueous Ionic Equilibrium
All textbooksTro 4th EditionCh.17 - Aqueous Ionic EquilibriumProblem 104
Previous problem
Next problem
Chapter 17, Problem 104

Predict whether a precipitate will form if you mix 175.0 mL of a 0.0055 M KCl solution with 145.0 mL of a 0.0015 M AgNO3 solution, and identify the precipitate, if any.

Verified step by step guidance
1
<Calculate the moles of KCl in the solution using the formula: moles = concentration (M) \times volume (L).>
<Calculate the moles of AgNO3 in the solution using the formula: moles = concentration (M) \times volume (L).>
<Determine the total volume of the mixed solution by adding the volumes of the KCl and AgNO3 solutions.>
<Calculate the concentrations of K^+ and Cl^- ions from KCl, and Ag^+ and NO3^- ions from AgNO3 in the mixed solution using the formula: concentration = moles / total volume (L).>
<Use the solubility product constant (K_sp) for AgCl to determine if the product of the concentrations of Ag^+ and Cl^- ions exceeds K_sp, indicating the formation of a precipitate.>
Previous problem
Next problem
Related Practice
Textbook Question

A solution containing sodium fluoride is mixed with one containing calcium nitrate to form a solution that is 0.015 M in NaF and 0.010 M in Ca(NO3)2. Does a precipitate form in the mixed solution? If so, identify the precipitate.

1711
views
Open Question
A solution containing potassium bromide is mixed with one containing lead acetate to form a solution that is 0.013 M in KBr and 0.0035 M in Pb(C2H3O2)2. Does a precipitate form in the mixed solution? If so, identify the precipitate.
Textbook Question

Predict whether a precipitate will form if you mix 75.0 mL of a NaOH solution with pOH = 2.58 with 125.0 mL of a 0.018 M MgCl2 solution. Identify the precipitate, if any.

1276
views
Open Question
What is the minimum concentration of KOH required for precipitation to begin for each of the following cation solutions? a. 0.015 M CaCl2 b. 0.0025 M Fe(NO3)2 c. 0.0018 M MgBr2
Textbook Question

Determine the minimum concentration of the precipitating agent on the right to cause precipitation of the cation from the solution on the left. a. 0.035 M Ba(NO3)2; NaF

2167
views
1
comments
Textbook Question

Determine the minimum concentration of the precipitating agent on the right to cause precipitation of the cation from the solution on the left. b. 0.085 M CaI2; K2SO4

561
views