Question

When solutions of (NH4)2SO4 and Ba(NO3)2 are mixed, a precipitate of BaSO4 forms, leaving soluble NH4NO3...

When solutions of (NH4)2SO4 and Ba(NO3)2 are mixed, a precipitate of BaSO4 forms, leaving soluble NH4NO3 in the solution. Write the ionic equation for the reaction.

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

The actual balanced molecular reaction would be,
(NH4)2SO4  (aq) + Ba(NO3)2  (aq) --------> BaSO4 (s) + 2 NH4NO3 (aq)
First write the total ionic equation and do not split the insoluble solids
2NH4+ (aq) +SO42- (aq)+Ba2+ (aq)+2NO3- (aq) -----> BaSO4 (s)+2NH4+(aq)+2NO3- (aq)
cancel out the similar terms on both the sides of the equation i.e) spectator ions and write the final
equation.
Therefore the net ionic equation is,
Ba2+ (aq) + SO42- (aq) --------> BaSO4 (s)

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
When aqueous solutions of (NH4)2CrO4 and Ba(NO3 )2 are combined, BaCrO4 precipitates. Calculate the mass, in...
When aqueous solutions of (NH4)2CrO4 and Ba(NO3 )2 are combined, BaCrO4 precipitates. Calculate the mass, in grams, of the BaCrO4 produced when 1.38 mL of 0.123 M Ba(NO3 )2 and 3.7 mL of 0.678 M (NH4)2CrO4 are mixed. Calculate the mass to 3 significant figures.
When aqueous solutions of (NH4)2CrO4 and Ba(NO3 )2 are combined, BaCrO4 precipitates. Calculate the mass, in...
When aqueous solutions of (NH4)2CrO4 and Ba(NO3 )2 are combined, BaCrO4 precipitates. Calculate the mass, in grams, of the BaCrO4 produced when 3.5 mL of 0.164 M Ba(NO3 )2 and 4 mL of 0.742 M (NH4)2CrO4 are mixed. Calculate the mass to 3 significant figures.
when 75.0 ml of .150 m NaCl solution and 75.0mL of a 0.250 M Pub(NO3)2 are...
when 75.0 ml of .150 m NaCl solution and 75.0mL of a 0.250 M Pub(NO3)2 are mixed, a white precipitate forms. a. Identify the precipitate in the reaction. b. write out the balanced molecular equation and net ionic equation for the reaction. c. Calculate the mass (in g) of precipitate formed. d. calculate the concentration s of the remaining ions in solution. (what is the total volume after the solutions are mixed? How many moles of each ion remain in...
When mixing two aqueous solutions of Na2CrO4 and AgNO3, a precipitate and a soluble salt form...
When mixing two aqueous solutions of Na2CrO4 and AgNO3, a precipitate and a soluble salt form according to the following equation. Na2CrO4(aq)+AgNO3(aq)=Ag2CrO4+NaNO3 Identify the precipitate and the soluble salt, using the solubility rules. (2 pts) Precipitate: Soluble salt: Classify the species mentioned in the above equation as strong electrolytes and weak electrolytes. (4 pts) Strong electrolytes: Weak electrolytes: Balance the above reaction and write the balanced formula equation. Include the status of each product (solid or aqueous). (3 pts) Write...
Determine whether a solid forms when solutions containing the following salts are mixed. If so, write...
Determine whether a solid forms when solutions containing the following salts are mixed. If so, write the ionic equation and the net ionic equation. Part A Na3PO4(aq) and AgNO3(aq). If a solid forms when solutions containing these salts are mixed, write the ionic equation. Part B Na3PO4(aq) and AgNO3(aq). If a solid forms when solutions containing these salts are mixed, write the net ionic equation. Part C MnSO4(aq) and Na2CO3(aq).If a solid forms when solutions containing these salts are mixed,...
When 100 mL of Ba(NO3)2 solution at 25 degrees Celsius is mixed with 100 mL solution...
When 100 mL of Ba(NO3)2 solution at 25 degrees Celsius is mixed with 100 mL solution CaSO4 solution at 25 degrees Celsius in calorimeter, the white solid BaSO4 forms and the temperature of the mixture increases to 28.1 degrees Celsius. Assuming that the calorimeter absorbs only a negligible quantity of heat and the specific heat capacity of the solution is 4.184 J/g.degrees Celsius, and that the density of the final solution is 1.0 g/mL, calculate the enthalpy change of this...
5. When 1.00L of a 1.00 M Ba(NO3)2 solution at 25.0oC is mixed with 1.00 L...
5. When 1.00L of a 1.00 M Ba(NO3)2 solution at 25.0oC is mixed with 1.00 L of a 1.00 M Na2SO4 solution at 25.0oC in a calorimeter, the white solid, BaSO4 forms and the temperature of the mixture increases to 28.1oC. Assuming that the calorimeter absorbs only a negligible quantity of heat, that the specific heat capacity of the solution is 4.18 J/oC g and that the density of the final solution is 1.0 g/mL, calculate the enthalpy change per...
Which of the following solutions will form a precipitate when added to Ba(NO3)2? KOH, NaC2H3O2, KNO3,...
Which of the following solutions will form a precipitate when added to Ba(NO3)2? KOH, NaC2H3O2, KNO3, NaI, or MgSO4
Determine whether a solid forms when solutions containing the following salts are mixed. If so write...
Determine whether a solid forms when solutions containing the following salts are mixed. If so write the ionic equation and the net ionic equation 1-Na3 PO4(aq) and AgNO3 express your answer as a chemical equation identify all of the phases in your answer if no reaction if no solid is formed Ionic equation=--------- 2-Na3PO4(aq) and AgNO3 Net ionic equation=________ 3- K2SO4(aq) and Na2CO3 Ionic equation=_________ 4- K2 SO.4 and Na 2 CO3(aq) Net ionic equation 5- Pb(NO3) 2 (aq) and...
Use the solubility generalizations on the information page to predict if one or more precipitates will...
Use the solubility generalizations on the information page to predict if one or more precipitates will form when aqueous solutions of chromium(III) sulfate (Cr2(SO4)3) and barium acetate (Ba(CH3COO)2) are mixed. Write the formula of any precipitate that could form in one of the blanks. If a box is not needed, leave it empty. If no precipitate is predicted, leave both blanks empty ___________ ... ____________. Soluble Ionic Compounds 1. All sodium (Na+), potassium (K+), and ammonium (NH4+) compounds are SOLUBLE....
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT