Ammonium chloride, NH4Cl, is a very soluble salt in water. (d) How many grams of silver nitrate do you need to add to the solution in part (c) to precipitate all of the chloride as silver chloride?

Verified step by step guidance

Step 1: Write down the balanced chemical equation for the reaction. In this case, the reaction is between ammonium chloride (NH4Cl) and silver nitrate (AgNO3) to form silver chloride (AgCl) and ammonium nitrate (NH4NO3). The balanced equation is: NH4Cl + AgNO3 -> AgCl + NH4NO3

Step 2: Determine the stoichiometry of the reaction. From the balanced equation, we can see that one mole of NH4Cl reacts with one mole of AgNO3 to form one mole of AgCl. Therefore, the stoichiometry is 1:1:1.

Step 3: Calculate the number of moles of NH4Cl in the solution from part (c). This can be done by dividing the mass of NH4Cl by its molar mass.

Step 4: Since the stoichiometry of the reaction is 1:1, the number of moles of AgNO3 needed to react with all the NH4Cl is equal to the number of moles of NH4Cl.

Step 5: Calculate the mass of AgNO3 needed by multiplying the number of moles of AgNO3 by its molar mass. This will give you the amount of AgNO3 in grams that you need to add to the solution to precipitate all of the chloride as AgCl.

Verified video answer for a similar problem:

This video solution was recommended by our tutors as helpful for the problem above.

Video duration:

Was this helpful?

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Solubility and Precipitation

Solubility refers to the ability of a substance to dissolve in a solvent, forming a solution. In this context, ammonium chloride (NH4Cl) is highly soluble in water. When a soluble salt is mixed with another solution containing ions that can form an insoluble compound, a precipitation reaction occurs, resulting in the formation of a solid precipitate.

Stoichiometry

Stoichiometry is the calculation of reactants and products in chemical reactions. It involves using balanced chemical equations to determine the relationships between the amounts of substances involved. In this case, knowing the stoichiometric ratios between ammonium chloride and silver nitrate is essential to calculate how much silver nitrate is needed to completely precipitate the chloride ions as silver chloride (AgCl).

Molar Mass

Molar mass is the mass of one mole of a substance, expressed in grams per mole (g/mol). It is crucial for converting between the number of moles of a substance and its mass. To find out how many grams of silver nitrate are required to precipitate all the chloride ions, one must first calculate the molar mass of silver nitrate (AgNO3) and use it in conjunction with stoichiometric calculations.

Recommended video:

Guided course

02:11

Molar Mass Concept

Related Practice

Textbook Question

Use average bond enthalpies from Table 8.4 to estimate the enthalpies of the following gas-phase reactions: Reaction 1: HF1g2 + H2O1g2 Δ F-1g2 + H3O+1g2 Reaction 2: HCl1g2 + H2O1g2 Δ Cl-1g2 + H3O+1g2 Are both reactions exothermic? How do these values relate to the different strengths of hydrofluoric and hydrochloric acid?

Textbook Question

Ammonia reacts with boron trifluoride to form a stable compound, as we saw in Section 8.7. (a) Draw the Lewis structure of the ammonia–boron trifluoride reaction product.

Textbook Question

Ammonium chloride, NH4Cl, is a very soluble salt in water. (c) If you dissolve 14 g of ammonium chloride in 500.0 mL of water, what is the molar concentration of the solution?

Textbook Question

Ammonium chloride, NH4Cl, is a very soluble salt in water. (a) Draw the Lewis structures of the ammonium and chloride ions.

Textbook Question

(a) Compare the bond enthalpies (Table 8.3) of the carbon– carbon single, double, and triple bonds to deduce an average pi bond contribution to the enthalpy. What fraction of a single bond does this quantity represent?

Textbook Question

(a) Use average bond enthalpies (Table 8.3) to estimate H for the atomization of naphthalene, C10H8: