For each confirmatory precipitate (PbCl_2, CuS, ZnS, and CaCO_3), write a net ionic equation for...
Question:
For each confirmatory precipitate ({eq}PbCl_2 {/eq}, CuS, ZnS, and {eq}CaCO_3 {/eq}), write a net ionic equation for the formation of the precipitate.
Net-Ionic Equation:
The simplest way to express the formation of a precipitate is by using net-ionic equations. A net-ionic equation only consists of the ions involved in precipitate formation. It can be determined by writing the molecular and complete ionic equations. These complete equations also include the spectator ions. Once the precipitate has been identified, we can omit writing the spectator ions to establish the net-ionic equation.
Answer and Explanation: 1
Become a Study.com member to unlock this answer! Create your account
View this answer
We can write the net-ionic equation for each reaction by writing the constituent ions on the reactants and the solid precipitate on the product....
See full answer below.
Ask a question
Our experts can answer your tough homework and study questions.
Ask a question Ask a questionSearch Answers
Learn more about this topic:
Get access to this video and our entire Q&A library
Precipitation Reactions: Predicting Precipitates and Net Ionic Equations
from
Chapter 10 / Lesson 9
129K
Study precipitate reactions. Determine precipitate solubility according to solubility rules. Learn to write ionic equations by following a molecular reaction.
Related to this Question
- Write a net ionic equation for any reaction that produces a precipitate.
- Write the net ionic equation to show the formation of a precipitate (insoluble salt) when FeCl3(aq) and NH4NO3(aq) are mixed. Write no reaction if there is no precipitate.
- Write the net ionic equation to show the formation of a solid insoluble salt when the following solutions are mixed. Write no reaction if there is no precipitate. (a) A g N O 3 ( a q ) and L i F ( a q ) (b) N a N O 3 ( a q ) and K B r ( a q ) (c)
- Write the net ionic equation to show the formation of a precipitate (insoluble salt) when solutions of Ca(NO3)2(aq) and Na2S(aq) are mixed. If no precipitate is formed, explain why.
- Find the net ionic equation to show the formation of a precipitate (insoluble salt) when Li2SO4(aq) and BaCl2(aq) are mixed.
- Write the net ionic equation to show the formation of a precipitate(insoluble salt) when the following solutions are mixed. Write -no reaction- if there is no precipitate. A.) Ni(NO3)2(aq) and Na2S(a
- Write the net ionic equation to show the formation of a precipitate (insoluble salt) when solutions of FeCl3(aq) and NH4NO3(aq) are mixed. If no precipitate is formed, explain why.
- Write the net ionic equation to show the formation of a precipitate (insoluble salt) when solutions of Na3PO4(aq) and Pb(NO3)2(aq) are mixed. If no precipitate is formed, explain why.
- Finish the reaction, then balance and determine the net ionic equation for this precipitate reaction: AgClO3 + CaCl2 =
- Determine whether the following reaction will form a precipitate. If a precipitate is formed, identify it and write the complete ionic and net ionic equations for the reaction. Fe(NO3)2(aq) + Na3PO4(aq) arrow
- Determine whether the following reaction will form a precipitate. If a precipitate is formed, identify it and write the complete ionic and net ionic equations for the reaction. LiCH3COO(aq) + MgCl2(aq) arrow
- Determine whether the following reaction will form a precipitate. If a precipitate is formed, identify it and write the complete ionic and net ionic equations for the reaction. K2S(aq) + CaI2(aq) arrow
- Determine whether the following reaction will form a precipitate. If a precipitate is formed, identify it and write the complete ionic and net ionic equations for the reaction. Al(ClO3)3(aq) + Na2SO3(aq) arrow
- Determine whether the following reaction will form a precipitate. If a precipitate is formed, identify it and write the complete ionic and net ionic equations for the reaction. BaCl2(aq) + (NH4)2SO4(aq) arrow
- For the precipitate that formed, write the complete molecular reaction, the complete (full) ionic equation, and lastly, the net ionic equation for the following: BaCl_2 + NalO_3 to
- Predict whether a precipitate will form when the following aqueous solutions are mixed. If a precipitate will form, write out the formula of the precipitate and a net ionic equation that describes its formation. (NH4)2CO3(aq) + Ba(NO3)2 arrow
- For the precipitate that formed, write the complete molecular reaction, the complete (full) ionic equation, and lastly, the net ionic equation for the following: Zn(NO_3)_2 + NaOH to
- Write the balanced molecular, total, and net ionic equations for the reaction that forms a precipitate in the following solutions.
- Predict whether a precipitate will form when the following aqueous solutions are mixed. If a precipitate will form, write out the formula of the precipitate and a net ionic equation that describes its formation. CaCl2(aq) + K3PO4(aq) arrow
- Predict whether a precipitate will form when the following aqueous solutions are mixed. If a precipitate will form, write out the formula of the precipitate and a net ionic equation that describes its formation. KCl(aq) + Na2SO4(aq) arrow
- Predict whether a precipitate will form when the following aqueous solutions are mixed. If a precipitate will form, write out the formula of the precipitate and a net ionic equation that describes its formation. Pb(NO3)2(aq) + K2SO4(aq) arrow
- Predict whether a precipitate will form when the following aqueous solutions are mixed. If a precipitate will form, write out the formula of the precipitate and a net ionic equation that describes its formation. NaC2H3O2(aq) + SbCl3(aq) arrow
- Write the net ionic equations for the reactions that occur when: A precipitate forms when 1 M chromium(III) nitrate is mixed with 1 M barium hydroxide.
- Write the balanced ionic equation and balanced net ionic equation for the following. Write the correct name of any precipitate formed. HgCl2(aq) + KOH (aq)
- Write the balanced ionic equation and the balanced net ionic equation for the following. Write the correct name of any precipitate formed. Ba(NO3)2(aq) + Al(SO4)3(aq)
- Determine if the following reactions will form a precipitate when mixed. If one is formed, write the BALANCED formula unit, the COMPLETE IONIC, and NET IONIC equations. If a precipitate doesn't form, write NR for no reaction. PLEASE include the physical s
- Determine if the following reaction will form a precipitate. If a precipitate is formed, write the complete ionic and net ionic equations for the reaction. If a precipitate does not form, explain why. Al2(SO4)3(aq) + Na2CO3(aq) arrow
- Determine if the following reaction will form a precipitate. If a precipitate is formed, write the complete ionic and net ionic equations for the reaction. If a precipitate does not form, explain why. K3PO4(aq) + CaCl2(aq) arrow
- Determine if the following reaction will form a precipitate. If a precipitate is formed, write the complete ionic and net ionic equations for the reaction. If a precipitate does not form, explain why. NaCH3COO(aq) + MgCl2(aq) arrow
- Determine if the following reaction will form a precipitate. If a precipitate is formed, write the complete ionic and net ionic equations for the reaction. If a precipitate does not form, explain why. Pb(ClO4)2(aq) + HI(aq) arrow
- Determine if the following reaction will form a precipitate. If a precipitate is formed, write the complete ionic and net ionic equations for the reaction. If a precipitate does not form, explain why. Ba(NO3)2(aq) + NH4OH(aq) arrow
- For the precipitate that formed, write the complete molecular reaction, the complete (full) ionic equation, and lastly, the net ionic equation for the following: BaCl_2 + NaOH to
- Write the balanced ionic equation and the balanced net ionic equation for the following. Write the correct name of any precipitate formed. NH4OH(aq) + LiCl(aq) ---> ______
- Write the net ionic equation for the reaction of sodium sulfate and barium chloride. Assume that a precipitate is formed.
- Write the ionic equation for the reaction of lead (II) nitrate reacting with the acidic solution to form a precipitate.
- What is the stoichiometric coefficient of the precipitate in the net ionic equation when Li_2S(aq) is mixed with Cu(NO_3)_2(aq)?
- A precipitate forms when solutions of sodium carbonate and calcium nitrate are combined. Write the net ionic equation for this reaction.
- Is a precipitate formed by the reaction between Ba(NO3)2 and NaBr? If so, write a balanced molecular equation and a net ionic equation for the reaction. If not, explain why not.
- For the precipitate that formed, write the complete molecular reaction, the complete (full) ionic equation, and lastly, the net ionic equation for the following: BaCl_2 +Al_2(SO_4)_3 to
- Write the balanced ionic equation and the balanced net ionic equation for the following. Write the correct name of any precipitate formed. Pb(NO3)2 + MgCl2
- Write the formula for the precipitate that forms when the following reactants are combined: HCl(aq) + H_2O(l)
- Write the net ionic equation for the reaction of sodium phosphate and barium chloride. Assume that a precipitate is formed.
- Predict the precipitate produced by mixing an Al(NO_3) solution with NaOH solution. Write the net ionic equation for the reaction. (Include the state of matter.) Al^3+(aq)+3OH^-(aq)-->Al(OH)_3(s)
- For the precipitate that formed, write the complete molecular reaction, the complete (full) ionic equation, and lastly, the net ionic equation for the following: NaOH + Al_2(SO_4)_3 to
- Write the net ionic equation for the reaction of sodium iodide and silver nitrate. Assume that a precipitate is formed.
- Write a balanced molecular and net ionic equation for the potential precipitation reaction. Indicate if there is no precipitate. L i 2 C O 3 ( a q ) + N a O H ( a q )
- Write a balanced molecular and net ionic equation for the potential precipitation reaction. Indicate if there is no precipitate. K 3 P O 4 ( a q ) + S r ( N O 3 ) 2 ( a q )
- Write a balanced molecular and net ionic equation for the potential precipitation reaction. Indicate if there is no precipitate. A g N O 3 ( a q ) + ( N H 4 ) 2 S O 4 ( a q )
- Write a balanced molecular and net ionic equation for the potential precipitation reaction. Indicate if there is no precipitate. B a C l 2 ( a q ) + Z n S O 4 ( a q )
- Write a balanced molecular and net ionic equation for the potential precipitation reaction. Indicate if there is no precipitate. M g ( N O 3 ) 2 ( a q ) + N a O H ( a q )
- Write a balanced molecular and net ionic equation for the potential precipitation reaction. Indicate if there is no precipitate. N a 2 S ( a q ) + Z n C l 2 ( a q )
- Is a precipitate formed by the reaction between Pb(NO3)2 and NaBr? If so, write a balanced molecular equation and a net ionic equation for the reaction. If not, explain why not.
- Write the formula of the precipitate formed when the following reactants are combined: NaOH(aq) + Na_2CO_3(aq)
- Write the formula of the precipitate formed when the following reactants are combined: NaOH(aq) + H_2O(l)
- Write the formula of the precipitate formed when the following reactants are combined: NaOH(aq) + MgSO_4(aq)
- Predict the precipitate produced by mixing an Al(NO_3)3 solution with a NaOH solution. Write the net ionic equation for the reaction. (Include the states of matter.)
- Is a precipitate formed by the reaction between Cu(NO3)2 and NaBr? If so, write a balanced molecular equation and a net ionic equation for the reaction. If not, explain why not.
- Write the net ionic equation for the following reaction. Identify the spectator ions and the precipitate formed. K3PO4(aq) + 3Sr(NO3)2(aq) arrow
- Write the net ionic equation to show the formation of a solid (insoluble ionic compound) when the following solutions are mixed: AgNO3(aq) and NaCl(aq).
- Complete the equations and balance them, showing the phases of the products. If precipitate is found, give the net ionic equation. A. BaCl2(aq) + Na2SO4(aq) B. Mg(NO3)2(aq) + KOH(aq)
- Write the formula of the precipitate formed when the following reactants are combined: HCl(aq) + MgSO_4(aq)
- Is a precipitate formed by the reaction between Ba(NO3)2 and NaOH? If so, write a balanced molecular equation and a net ionic equation for the reaction. If not, explain why not.
- Is a precipitate formed by the reaction between Ba(NO3)2 and Na2SO4? If so, write a balanced molecular equation and a net ionic equation for the reaction. If not, explain why not.
- Write the net ionic equation for the reaction of adding Zn(NO3)2 to NaOH gives a clear solution, then white precipitate forms.
- Is a precipitate formed by the reaction between AgNO3 and NaBr? If so, write a balanced molecular equation and a net ionic equation for the reaction. If not, explain why not.
- Write the complete ionic equation and the net ionic equation from the following molecular equation, then select which compound is the precipitate or the compound that is insoluble according to the solubility rule for the corresponding ionic equation: AgNO
- Write the balanced ionic equation and the balanced net ionic equation for the following. Write the correct name of any precipitate formed. NaCl + Fe(NO3)2
- Write the balanced ionic equation and the balanced net ionic equation for the following. Write the correct name of any precipitate formed. AgNO3 + KCl
- Is a precipitate formed by the reaction between AgNO3 and Na2SO4? If so, write a balanced molecular equation and a net ionic equation for the reaction. If not, explain why not.
- Write the net ionic equation to show the formation of a solid (insoluble ionic compound) when the following solutions are mixed: K2CO3(aq) and CaCl2(aq).
- Is a precipitate formed by the reaction between Pb(NO3)2 and Na2SO4? If so, write a balanced molecular equation and a net ionic equation for the reaction. If not, explain why not.
- Write the net ionic equation for the reaction of adding NH3 to Zn(OH)2 gives a white precipitate that disappears, and the solution becomes clear.
- A solution of N a 2 S is mixed with a solution of C u C l 2 . A black precipitate is formed. Write the net ionic equation for the reaction, and identify the black precipitate.
- Is a precipitate formed by the reaction between AgNO3 and NaOH? If so, write a balanced molecular equation and a net ionic equation for the reaction. If not, explain why not.
- If the following reaction occurs and forms a precipitate, write out net ionic equation and list spectator ions. CuSO₄(aq) + BaCl₂(aq) → CuCl₂(aq) + BaSO₄(s)
- Write the overall ionic equation and the net ionic equation for the reaction between BaCl_2 and Na_2SO_4 in aqueous solution. Identify the spectator ion and the precipitate ion for this reaction.
- Write the net ionic equation for the reaction of sodium acetate and silver nitrate. Assume that a precipitate is formed.
- Is a precipitate formed by the reaction between Ba(NO3)2 and Na2CO3? If so, write a balanced molecular equation and a net ionic equation for the reaction. If not, explain why not.
- Write the formula for the precipitate that forms (if any) in the reaction between K2CO3 and BaCl2.
- Write the complete ionic equation and the net ionic equation from the following molecular equation, then select which compound is the precipitate or the compound that is insoluble according to the solubility rule for the corresponding ionic equation: Pb(N
- Write the formula of the precipitate formed when the following reactants are combined: AgNO_3(aq) + H_2O(l)
- Is a precipitate formed by the reaction between Pb(NO3)2 and NaOH? If so, write a balanced molecular equation and a net ionic equation for the reaction. If not, explain why not.
- Is a precipitate formed by the reaction between AgNO3 and Na2CO3? If so, write a balanced molecular equation and a net ionic equation for the reaction. If not, explain why not.
- Is a precipitate formed by the reaction between Cu(NO3)2 and NaOH? If so, write a balanced molecular equation and a net ionic equation for the reaction. If not, explain why not.
- Write the net ionic equation for the reaction that occurs when solutions of MgCl2 and AgNO3 are mixed.
- Write the formula for the precipitate that forms (if any) in the reaction between K2CO3 and Pb(NO3)2.
- Is a precipitate formed by the reaction between Cu(NO3)2 and Na2SO4? If so, write a balanced molecular equation and a net ionic equation for the reaction. If not, explain why not.
- Is a precipitate formed by the reaction between Pb(NO3)2 and Na2CO3? If so, write a balanced molecular equation and a net ionic equation for the reaction. If not, explain why not.
- Write the complete ionic equation and the net ionic equation from the following molecular equation, then select which compound is the precipitate or the compound that is insoluble according to the solubility rule for the corresponding ionic equation: CaCl
- Complete and balance the following equation. If there is a precipitate or other net ionic product, write the net ionic equation. HNO3(aq) + NaHCO3(aq) arrow
- Complete and balance the following equation. If there is a precipitate or other net ionic product, write the net ionic equation. SrCl2(aq) + KOH(aq) arrow
- Complete and balance the following equation. If there is a precipitate or other net ionic product, write the net ionic equation. Ca(OH)2(aq) + H3PO4(aq) arrow
- Write the formula for the precipitate that forms (if any) in the reaction between Na2SO4 and BaCl2.
- Write the net ionic equation for the precipitation of barium carbonate from aqueous solution:
- Complete and balance the following equation. If there is a precipitate or other net ionic product, write the net ionic equation. Na2SO4(aq) + BaI2(aq) arrow
- Write the formula for the precipitate that forms (if any) in the reaction between Na2SO4 and Pb(NO3)2.
- A white precipitate forms when aqueous barium chloride is mixed with aqueous sodium sulfate. a. Write the molecular equation for the reaction. b. Write the net ionic equation for the reaction.
- Write the products and determine which of these reactions result in the formation of a precipitate. a) NaNO3(aq) + CaS(aq) b) MgSO4(aq) + CaS(aq)
- Write the formula of the precipitate formed when the following reactants are combined: NaOH(aq) + NaCl(aq)
- Write the net ionic equation for the reaction which occurs when potassium sulfate reacts with barium nitrate to form a precipitate. Include states in the equation.
Explore our homework questions and answers library
Browse
by subject