Homework Answers
Answer:-
These questions are answered by using simple concept of chemical reaction involving precipitate formation and then net ionic equations are written.
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please explain steps (a-d)
Exercises 1. Complete and balance the following reactions. Using the solubility rules...
---Complete and balance the precipitation reactions. Include physical states. Refer to the solubility rules as necessary....
---Complete and balance the precipitation reactions. Include physical states. Refer to the solubility rules as necessary. precipitation reaction: K3PO4(aq)+MgCl2(aq)⟶Mg3(PO4)2+6KCl(aq) ----Consider the chemical reaction. 3MgCl2(aq)+2Na3PO4(aq)⟶Mg3(PO4)2(s)+6NaCl(aq) Write the net ionic equation for the chemical reaction, including phases. net ionic equation:
Complete and balance the following molecular equations, being careful to apply the solubility rules. Write balanced...
Complete and balance the following molecular equations, being careful to apply the solubility rules. Write balanced ionic and net ionic equations for the reactions. (a) FeSO4(aq) + KPO.(aq) → (b) AgC H2O2(aq) + AlCl3(a) + (c) chromium(III) chloride + barium hydroxide 44 a l ire al 150 A Garotadas a nadad a la
use solubility rules to write net ionic (1) Use the solubility rules and write net ionic equations for the followin...
use solubility rules to write net ionic
(1) Use the solubility rules and write net ionic equations for the following reactions (a) Pb(NO3)2 (aq) + Na2SO4 (b) BaCl2 (aq) + ZnSO4 (aq) (c) (NH4)2CO, (aq) + CaCl2 (aq) (d) Na S (aq) + ZnCl2 (aq)
1IC LUDOUCO 1. Complete and balance the following net ionic equations. If no reaction occurs, write...
1IC LUDOUCO 1. Complete and balance the following net ionic equations. If no reaction occurs, write NR. a. Mg?+ + OH (imited -- b. Cu²+ + SCN" - c. Co2+ + NH3(aq) limited + H20 - d. Ba2+ + so; - e. Pb2+ + NH3(aq) excess + H20 – f. Fel+ + SO-- 2. Complete and balance the following net ionic equations. If no reaction occurs, write NR. Tables 4 and 5 of Experiment 7 list amphoteric metal hydroxides that...
1. For each of the following pairs of aqueous solutions, use the solubility rules to determine...
1. For each of the following pairs of aqueous solutions, use the solubility rules to determine whether or not a precipitate will form when they are mixed. Write the names and formulas of any precipitates that form. Refer to the table below (same as Table 4.1 on page 153 of the textbook) for the solubility rules. If yes, write Formula ofl Precipitate Chemical Name of Precipitate Reactants in an aqueous Will a precipitate solution form? a) calcium nitrate + ammonium...
#3 action of a double-replacement reaction 2. Using the solubility rules, predict the solubility of each...
#3
action of a double-replacement reaction 2. Using the solubility rules, predict the solubility of each of the following compounds in wan solution), s = insoluble solid) the following compounds in water (aq-soluble (aqueous a) CaCO3 b ) Al(OH), S c ) Cu(NO3)290_ d) HgCl2 99 - double displacement reaction takes place between two ionic compounds that are dissolved in an aqueous solution and form two new compounds. For example, sodium phosphate and silver nitrate combine to yield sodium nitrate...
1. For the following reactions, determine the products when two solutions are mixed. Use the solubility...
1. For the following reactions, determine the products when two solutions are mixed. Use the solubility rules to predict whether a precipitate would form. If no reaction occurs, write "NR”. Be sure to balance your reaction and include all states of matter. The first one has been done for you. a) 3 Ba(NO3)2 (aq) + Al2(SO4)3 (aq) → 2 AI(NO3)3 (aq) + 3 BaSO4 (s) b) LINO3(aq) + Mg(C2H302)2 (aq) → c) NiSO4 (aq) + K3PO4 (aq) → d) Na2S...
4. Using the table below which give the solubility rules for ionic compounds, predict whether each...
4. Using the table below which give the solubility rules for ionic compounds, predict whether each of the reactions below will produce a precipitate and, if so, what is the precipitate. If there is more than one precipitate, write down both of them. (2 points per reaction, 10 points total) Table 1 Solubility Rules for lonic Compounds Soluble in Water Insoluble in Water Any salt with Li+, Na+, K+, NH4+, NO3- Most chlorides, C oblava a AgCl, PbCl2, and HgCl2...
Complete and balance the precipitation reactions. Include physical states in your equations. Click here for solubility...
Complete and balance the precipitation reactions. Include
physical states in your equations. Click here for solubility
rules.
i need help with both of these questions please .
Complete and balance the precipitation reactions. Include physical states in your equations. Click here for solubility rules. AgNO, aq)+ NaCl aq)-> Tip: If you need to clear your work and reset the equation, click the button that looks like two red arrows. 2. Complete and balance the molecular equation, including phases, for the...
Use your knowledge about solubility rules and reactions to write (1) a balanced chemical equation (molecular...
Use your knowledge about solubility rules and reactions to write
(1) a balanced chemical equation (molecular equation), (2) a total
ionic equation, and (3) a net ionic equation for th reactions
below. Include the appropriate phase for each species.
(m) NaCO3(aq) + SrCla) - (n) Na2CO3(aq) + H2SO4(aq) (o) SrCl(aq) + H2SO4(aq) →
Complete and balance the following molecular equations, being careful to apply the solubility rules. Write balanced ionic and net ionic equations for the reactions. (a) FeSO4(aq) + KPO.(aq) → (b) AgC H2O2(aq) + AlCl3(a) + (c) chromium(III) chloride + barium hydroxide 44 a l ire al 150 A Garotadas a nadad a la
use solubility rules to write net ionic
(1) Use the solubility rules and write net ionic equations for the following reactions (a) Pb(NO3)2 (aq) + Na2SO4 (b) BaCl2 (aq) + ZnSO4 (aq) (c) (NH4)2CO, (aq) + CaCl2 (aq) (d) Na S (aq) + ZnCl2 (aq)
1IC LUDOUCO 1. Complete and balance the following net ionic equations. If no reaction occurs, write NR. a. Mg?+ + OH (imited -- b. Cu²+ + SCN" - c. Co2+ + NH3(aq) limited + H20 - d. Ba2+ + so; - e. Pb2+ + NH3(aq) excess + H20 – f. Fel+ + SO-- 2. Complete and balance the following net ionic equations. If no reaction occurs, write NR. Tables 4 and 5 of Experiment 7 list amphoteric metal hydroxides that...
1. For each of the following pairs of aqueous solutions, use the solubility rules to determine whether or not a precipitate will form when they are mixed. Write the names and formulas of any precipitates that form. Refer to the table below (same as Table 4.1 on page 153 of the textbook) for the solubility rules. If yes, write Formula ofl Precipitate Chemical Name of Precipitate Reactants in an aqueous Will a precipitate solution form? a) calcium nitrate + ammonium...
#3
action of a double-replacement reaction 2. Using the solubility rules, predict the solubility of each of the following compounds in wan solution), s = insoluble solid) the following compounds in water (aq-soluble (aqueous a) CaCO3 b ) Al(OH), S c ) Cu(NO3)290_ d) HgCl2 99 - double displacement reaction takes place between two ionic compounds that are dissolved in an aqueous solution and form two new compounds. For example, sodium phosphate and silver nitrate combine to yield sodium nitrate...
1. For the following reactions, determine the products when two solutions are mixed. Use the solubility rules to predict whether a precipitate would form. If no reaction occurs, write "NR”. Be sure to balance your reaction and include all states of matter. The first one has been done for you. a) 3 Ba(NO3)2 (aq) + Al2(SO4)3 (aq) → 2 AI(NO3)3 (aq) + 3 BaSO4 (s) b) LINO3(aq) + Mg(C2H302)2 (aq) → c) NiSO4 (aq) + K3PO4 (aq) → d) Na2S...
4. Using the table below which give the solubility rules for ionic compounds, predict whether each of the reactions below will produce a precipitate and, if so, what is the precipitate. If there is more than one precipitate, write down both of them. (2 points per reaction, 10 points total) Table 1 Solubility Rules for lonic Compounds Soluble in Water Insoluble in Water Any salt with Li+, Na+, K+, NH4+, NO3- Most chlorides, C oblava a AgCl, PbCl2, and HgCl2...
Complete and balance the precipitation reactions. Include
physical states in your equations. Click here for solubility
rules.
i need help with both of these questions please .
Complete and balance the precipitation reactions. Include physical states in your equations. Click here for solubility rules. AgNO, aq)+ NaCl aq)-> Tip: If you need to clear your work and reset the equation, click the button that looks like two red arrows. 2. Complete and balance the molecular equation, including phases, for the...
Use your knowledge about solubility rules and reactions to write
(1) a balanced chemical equation (molecular equation), (2) a total
ionic equation, and (3) a net ionic equation for th reactions
below. Include the appropriate phase for each species.
(m) NaCO3(aq) + SrCla) - (n) Na2CO3(aq) + H2SO4(aq) (o) SrCl(aq) + H2SO4(aq) →
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