A 250.0 g sample of a white solid is known to be a mixture of KNO3, BaCl2, and NaCl. When 100.0 g of this mixture is dis-solved in water and allowed to react with excess H2SO4, 67.3 g of a white precipitate is collected. When the remaining 150.0 g of the mixture is dissolved in water and allowed to react with excess AgNO3, 197.6 g of a second precipitate is collected. (a) What are the formulas of the two precipitates?

Verified step by step guidance

Identify the possible reactions that can occur when the mixture is treated with H2SO4 and AgNO3.

Consider the solubility rules to determine which compounds will form precipitates with H2SO4 and AgNO3.

For the reaction with H2SO4, recognize that BaCl2 will react to form BaSO4, a common insoluble sulfate.

For the reaction with AgNO3, recognize that both BaCl2 and NaCl can form AgCl, a common insoluble chloride.

Conclude that the first precipitate is BaSO4 and the second precipitate is 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.

Precipitation Reactions

Precipitation reactions occur when two soluble salts react in solution to form an insoluble product, known as a precipitate. This process is driven by the formation of a compound that has low solubility in water, leading to its separation from the solution. Understanding the solubility rules helps predict which combinations of ions will result in a precipitate.

Stoichiometry

Stoichiometry is the calculation of reactants and products in chemical reactions based on the conservation of mass. It involves using balanced chemical equations to determine the amounts of substances consumed and produced. In this context, stoichiometry is essential for relating the masses of the precipitates to the amounts of the original mixture components.

Chemical Formulas and Compounds

Chemical formulas represent the composition of compounds, indicating the types and numbers of atoms present. In this question, identifying the precipitates requires knowledge of the chemical formulas for the compounds involved, such as KNO3, BaCl2, and NaCl, and their reactions with H2SO4 and AgNO3. Recognizing the products formed from these reactions is crucial for determining the precipitates.

Recommended video:

Guided course

03:37

Writing Formulas of Coordination Compounds Example

Related Practice

Textbook Question

Why do we use a double arrow to show the dissociation of a weak acid or weak base in aqueous solution?

Textbook Question

How could you use a precipitation reaction to separate each of the following pairs of anions? Write the formula for each reactant you would add, and write a balanced net ionic equation for each reaction.(a)

Textbook Question

The following three solutions are mixed: 100.0 mL of 0.100 M Na2SO4, 50.0 mL of 0.300 M ZnCl2, and 100.0 mL of 0.200 M Ba(CN)2. (a) What ionic compounds will precipitate out of solution?

Textbook Question

The following three solutions are mixed: 100.0 mL of 0.100 M Na2SO4, 50.0 mL of 0.300 M ZnCl2, and 100.0 mL of 0.200 M Ba(CN)2. (b) What is the molarity of each ion remaining in the solution assuming complete precipitation of all insoluble compounds?

Textbook Question

(b) What is the mass of each substance in the original 250 g mixture?

Textbook Question

Assume that you are given a solution of an unknown acid or base. How can you tell whether the unknown substance is acidic or basic?