. Sodium carbonate is combined with calcium nitrate. a. Write the molecular, ionic equation, and net ionic equation for the reaction that occurs. b. Is there a precipitate? If so, what is the molecular formula of the precipitate and which are spectator ions? c. If 10.0 g of sodium carbonate and 10.0 g of calcium nitrate are combined, What is the limiting reactant?

6. Sodium sulfide reacts with hydrochloric acid to produce hydrogen sulfide and sodium chloride. How many grams of sodium sulfide are required for complete reaction with 15.0 mL of 0.250 M hydrochloric acid? The molar mass of sodium sulfide is 78.046 g/mol. (Hint: start by writing the balanced equation for the reaction.)

10.0 mL of a 0.30-M sodium phosphate solution reacts with 20.0 mL of a 0.20-M lead(II) nitrate solution (assume no volume change) a) What precipitate will form? b) Write out the molecular equation, complete ionic equation, net ionic equation. c) Which reactant is the limiting reactant? d) What mass of precipitate will form?   For part d, please show main steps.

Write the balanced equation for the following situation. In addition, list the reaction type. You must tell the amount of every substance that remains in the container at the end of the reaction. Assume that all reactions go to completion. If only stoichiometry, tell how much excess reactant is used. Reaction Type:a. Combination Reactionb. Decomposition Reactionc. Single Displacement / THIS IS ONE TYPE OF Oxidation Reduction Reaction d. Precipitation Reactione. Gaseous Reactionf. Neutralization Reactiong. Combustion Reaction 61.802 cg of nitrogen gas is reacted with 61.802 cg of hydrogen gas to form ammonia

When a solution of ammonium chloride is added to a solution of lead (II) nitrate, a white precipitate of lead (II) chloride forms (Ammonium chloride and lead nitrate exist as dissociated ions in aqueous solution.) a. Write the complete ionic equation for this reaction. b. Write the net ionic equation for this reaction. c. Identify the spectator ions

For each of the following sets of reactants, write the balanced equation for the single displacement reaction that occurs. If you determine that a reaction will not occur, write “NR”, and provide a brief explanation.  a. Aluminum metal + aqueous nickel(II) nitrate b. Gold metal + hydrobromic acid

Write the balanced equation for the following situation. List the reaction type.Tell the amounts of every substance that remains in the container at the end of the reaction. Assume that all reactions go to completion. If only stoichiometry, tell how much of the excess reactant is used!!!!  Reaction Type:a. Combination Reactionb. Decomposition Reactionc. Single Displacement / THIS IS ONE TYPE OF Oxidation Reduction Reaction d. Precipitation Reactione. Gaseous Reactionf. Neutralization Reactiong. Combustion Reaction Follow the format used in the image. 5.92 g of sodium oxalate is reacted with 5.92 of calcium chloride

Aqueous solutions of magnesium nitrate (Mg(NO3)2) and sodium carbonate (Na2CO3) are mixed. Consult the solubility rules to predict the outcome of the reaction, and select from the list of options below, the one that matches your prediction most closely. O A. There will be no reaction. O B. Both MgCO3 and NaNO3 will precipitate. O C. MGCO3 will precipitate and NANO3 will remain in solution. O D. NANO3 will precipitate and MGCO3 will remain in solution.

3. In order to perform a chemical reaction, 225 mL of 0.500 M lead (II) nitrate is required. How much 5.00 M stock solution is required to make the proper solution? mL 4. How much water needs to be added to an 18.0 M stock solution of sodium hydroxide in order to make 450.0 mL of 0.250 M sodium hydroxide solution? mL of water