Write the balanced COMPLETE ionic equation for the reaction when ammonium carbonate and calcium chloride are mixed in aqueous solution. If no reaction occurs, simply write only NR. Be sure to include the proper phases for all species within the reaction.

A student carries out the following experiments and records the following observations.  1.  A few drops of a solution of KOH (aq) is added to a solution of Cu(NO3)2 (aq).  A blue gelatinous solid forms immediately upon addition.   2.   A few drops of a solution of KOH (aq) is added to a solution of NaNO3 (aq).  No changes are observed.  3.  A few drops of a solution of KOH (aq) is added to an unknown solution that could contain Cu2+(aq) and/or Na+(aq) ions (the solution could contain both ions, just one of the ions, or neither ions).  A blue gelatinous solid forms immediately upon addition.   Select all of the answers that are consistent with the data from those 3 experiments.  Group of answer choices The unknown contains Cu2+(aq) and Na+(aq) The unknown contains Cu2+(aq) The unknown contains Na+(aq) The unknown contains neither Cu2+(aq) or Na+(aq)

In the laboratory you are given the task of separating Ag* and Fe* ions in aqueous solution. For each reagent listed below indicate if it can be used to separate the ions. Type "Y" for or "N" for no. If the reagent CAN be used to separate the ions, give the formula of the precipitate. If it cannot, type "No" yes Y or N Reagent Formula of Precipitate if YES 1. HBr 2. K2SO4 3. КОН

Table 1: Titration Data Volume of magnesium hydroxide solution in Erlenmeyer flask Concentration of magnesium hydroxide 0.135 mol/L solution in Erlenmeyer flask Initial volume of nitric acid solution in burette Final volume of nitric acid solution in burette 10.Use the data in Table 1 to answer the folowing (a) Write the balanced chemical equatio. (b) Calculate the molar concentration of nitric acid 20.00 mL (c) Calculate the pH of the acid. 1.06 mL 23.08 mL

How could you have used the color change property of iron(III) chloride to monitor when the reaction had reached completion? You could have added drops of iron(III) chloride directly to the reaction mixture until a change in color occurred. You could have placed a drop of iron(III) chloride directly to the reaction mixture and waited until the color disappeared. You could have placed a drop of reaction mixture every minute in one test tube containing iron(III) chloride until there was no color change. You could have placed a drop of reaction mixture into different test tubes containing iron(III) chloride every minute until there was no color change. Incorrect

QUESTION #1: TOPIC: Solving for a reactant in solution  One way in which the useful metal copper is produced is by dissolving the mineral azurite, which contains copper(II) carbonate, in concentrated sulfuric acid. The sulfuric acid reacts with the copper(II) carbonate to produce a blue solution of copper(II) sulfate. Scrap iron is then added to this solution, and pure copper metal precipitates out because of the following chemical reaction: Fe(s) +CuSO4(aq) →Cu(s) +FeSO4(aq) Suppose an industrial quality-control chemist analyzes a sample from a copper processing plant in the following way. He adds powdered iron to a 350. mL copper(II) sulfate sample from the plant until no more copper will precipitate. He then washes, dries, and weighs the precipitate, and finds that it has a mass of 93. mg. Calculate the original concentration of copper(II) sulfate in the sample. Round your answer to 2 significant digits.   ? g/L         QUESTION#2: TOPIC: Limiting reactants…

Write the balanced dissociation equation for solid iron(III) nitrate in aqueous solution. If it does not dissociate, simply write only NR. Be sure to include the proper phases for all species within the reaction.

Please help...the current balanced equation is incorrect

Part 1 of 2 To a flask, 15.0 mL of 1.25 M HF is added. Then, 3.05 M NaOH is used to titrate the acid sample. Write the balanced net ionic equation for the acid- base reaction. Be sure to include states of matter. Part 2 of 2 00 X 00 ローロ X 3 To determine the concentration of a sample of Ca(OH)2, 1.45 M HCl is added drop-wise using a buret. Write the balanced net ionic equation for the acid- base reaction. Be sure to include states of matter. 0-0 h S

How can we answer these questions on solution stoichiometry and equilibrium?