The drawings below represent aqueous solutions. Solution A is 2.00 L of a 2.00-M aqueous solution of Copper (II) nitrate. Solution B is 2.00 L of a 3.00-M aqueous solution of Potassium hydroxide.

Draw a picture of the solution made by mixing solutions A and B together after the precipitation reaction takes place. Make sure this picture shows the correct relative volume compared to solutions A and B, and the correct relative number of ions, along with the correct relative amount of solid formed.

Determine the concentrations (in M) of all ions left in solution (from part a) and the mass of solid formed.

answer

watching

1,294

views

For unlimited access to Homework Help, a Homework+ subscription is required.

Liked by kpham8115

You have 0 free answers left.
Get unlimited access to 3.8 million step-by-step answers.

Get unlimited access

Already have an account? Log in

Robert KubaraLv10

16 Dec 2020

Unlock all answers

Get 1 free homework help answer.

Already have an account? Log in

Join us on Discord

Chemistry Study Group

Join now

Related questions

1.When aqueous solutions of ammonium phosphate and copper(II) nitrate are combined, solid copper(II) phosphate and a solution of ammonium nitrate are formed. The net ionic equation for this reaction is:
(Use the solubility rules provided in the OWL Preparation Page to determine the solubility of compounds.)

2. When aqueous solutions of potassium hypochlorite and nitric acid are mixed, an aqueous solution of potassium nitrate and hypochlorous acid results. Write the net ionic equation for the reaction.
(Use the solubility rules provided in the OWL Preparation Page to determine the solubility of compounds.)

Use H⁺ for the hydronium ion

3. Write a net ionic equation to show that nitric acid, HNO₃, behaves as an acid in water.

4. Write a net ionic equation to show that hydrofluoric acid , HF , behaves as an acid in water.

5. Write a net ionic equation to show why solid barium hydroxide, Ba(OH)₂ (s), forms a basic solution when it dissolves in water.

Write the balanced net ionic equations for the five laboratory situations described below. Write the reactants for the equations in the left box and the products in the right box. Do not designate the states of the substances. Assume that solutions are aqueous, and represent substances in solutions as ions.

1. Solid sodium oxide is added to water.

2. Pentane is combusted in air.

3. Zinc hydroxide is added to a solution of concentrated sodium hydroxide.

4. Solid copper (II) carbonate is heated strongly.

5. Zinc metal is added to a solution of hydrochloric acid.

Fill the questions according to Data Table 7-2

5. balanced formula equation: for each combination of solutions that produced new product. write correct chemical formulas for the new compounds that could form from the ions present. Indicate which of the new compunds is a precipitate. If no reaction occurs, write NR.

6. complete ionic equation: write complete ionic equations for the precipitation reactions that you observed. show the reactants as ions, the precipitate as a solid, and the spectator ions as unchanged. balance each equation for mass and change. the total charge should be zero on each side of the equation.

7. net ionic equation: write the net ionic equations for each reaction in the preceding question.